STOICHIOMETRY PROBLEMS

1.Write down the molecular equation and ionic equation, then state the name of the products.
a.A solution of barium hydroxide reacts with hydrochloric acid
b.Acetic acid reacts with a solution of sodium hydroxide.
c.Sulfuric acid reacts with a solution of ammonia.
d.Calcium oxide reacts with hydrochloric acid.
e.Carbon dioxide is added to calcium hydroxide solution.
f.Hydrochloric acid is added to calcium.
g.Dilluted sulfuric acid is added to magnesium.
h.Concentrated of sulfuric acid is added to iron.
i.Dilluted nitric acid is added to zink.
j.Concentrated nitric acid is added to silver.
k.A solution of silver nitrate reacts with a solution of table salt produces a precipitate.
l.A solution of ammonium chloride is added to a solution of sodium hydroxide, a gas will be produced.

2.Hydrochloric acid is added to 1,3 grams of zink (Ar 65). If molarity of acid is 3 mol/L, answer the following questions.
a.Write down the molecular equation and the ionic equation.
b.Determine the minimum volume of acid needed in this reaction.
c. Calculate the gas produced at:
1)STP
2)1 atm and 27 degree's celcius
3)the same T and P with nitrogen gas that its mass of 1 L is 2 grams.
d.If zink used is 80% from its ore, calculate the mass of ore used.

3.An aliage contains 90% of aluminium (Ar 27) and 10% of cuprum (Ar 63,5) is used to produce hydrogen gas. Hydrochloric acid is added to this aliage and produces 6,72 L gas at STP.
a.Write down the molecular equation and ionic equation.
b.Calculate the mass of aliage.
c.If the minimum volume of acid used is 200 mL, predict the molarity of this acid.

4.A mol of metal, M reacts with sulfuric acid 2M, produced 33,6 L hydrogen gas at STP. Answer the questions below.
a.Determine the formula of salt produced.
b.Determine the oxidation number of M.
c.Write down the molecular equation and ionic equation.
d.Calculate the minimum volume of acid needed.

5.FeS(Mr=88)is reacted with hydrochloric acid according to the following reaction:
FeS(s)+2HCL(aq) → FeCl2(aq)+H2S(g)
If this reaction produced 8 L of H2S gas, and at the same T and P, 1 mol of H2S gas = 20 L, answer the questions below.
a.Write down the ionic equation.
b.Calculate the mass of FeS.
c.If an ore contains 70,4% FeS, calculate the mass of ore.
d.The acid used is 4M. Determine the minimum volume of acid needed.

SOLUBILITY QUIZ

1. Please, consider saturated sodium chloride solution, NaCl(aq). Quite a bit of sodium chloride can be dissolved in water, about 6 moles/L. The number of moles of ions in the solution is ....
a. 0 M
b. 3 M
c. 6 M
d. 9 M
e. 12 M
2. In the saturated solution of NaCl, the type of particles in the solution is (are) ....
a. atoms
b. molecules
c. ions
d. atoms and ions
e. molecules and ions
3. What happens if we increase the concentration of Cl- by adding some concentrated hydrochloric acid (12M HCl)?.
a. the number of Cl- ions increases
b. there is a less saturated solution
c. all of ions are still in the saturated solution
d. NaCl crystal is produced
e. all ions precipitate to form crystal
4. The solubility of NaCl in water at room temperature is ....
a. 1 moles/L
b. 3 moles/L
c. 6 moles/L
d. 9 moles/L
e. 12 moles/L
5. To determine the solubility of solute in water, a solution must be prepared that is ….
a. saturated
b. unsaturated
c. diluted
d. concentrated
e. supersaturated
6. Which condition is essential to prepare a saturated solution of an ionic salt?
a. excess solute
b. any amount of solute
c. any amount of solvent
d. a temperature of 250C
e. a fixed volume of solvent
7. The solubility of a solute is best determined from which type of solution?
a. Any solution at 250C
b. A saturated solution
c. An unsaturated solution
d. A supersaturated solution
e. A concentrated solution
8. Molecular solutions do not conduct electricity because they contain ….
a. molecules only
b. cations and anions
c. molecules and anions
d. molecules and cations
9. Which of the solutes below is both ionic and most soluble?
a. CH3OH
b. Ca(OH)2
c. Ba(OH)2
d. Fe(OH)3
e. Zn(OH)2
10. Which of the solutes below is molecular?
a. RbOH
b. CH3OH
c. Ca(OH)2
d. Fe(OH)3
e. Sr(OH)2
11. Which one of the following would form an ionic solution when dissolved in water?
a. I2
b. CH3OH
c. Ca(NO3)2
d. Cl2H22O11
12. Which of the solutes below can form an ionic solution with the highest conductivity?
a. PbI2
b. CCl4
c. CH3OH
d. KNO3
e. HCOOH
13. Which of the following solutes will produce a molecular solution?
a. HBr
b. Na2S
c. HCl
d. KOH
e. CH3OH
14. In a 500 mL sample of 0.020 M K3PO4, the [PO43-] is ….
a. 0.005 M
b. 0.010 M
c. 0.020 M
d. 0.030 M
e. 0.040 M
15. What is the [Cl-] when 1.50 g of NaCl is dissolved in enough water to make 1000. mL of solution?
a. 0.0150 M
b. 0.0128 M
c. 0.0256 M
d. 0.330 M
e. 0.0390 M
16. What is the concentration of the ions in 3.0 L of 1.0 M Al2(CO3)3 ?
[Al3+] [CO32-]
a. 0.33 M 0.50 M
b. 0.66 M 1.0 M
c. 2.0 M 3.0 M
d. 3.0 M 4.5 M
e. 3.5 M 5.0 M
17. In an experiment, 0.500 mol of Fe(NO3)3 is dissolved in water to produce a 2.00L solution. The [NO3-] in this solution is ….
a. 0.250 M
b. 0.500 M
c. 0.750 M
d. 1.50 M
e. 2.00 M
18. What will be the [Cl-] when equal volumes of 0.10 M MgCl2 and 0.30 M AlCl3 are combined?
a. 0.30 M
b. 0.35 M
c. 0.55 M
d. 0.90 M
e. 1.10 M
19. Which value best represents the total ion concentration when 0.10 moles of K3PO4 is present in 0.5 L of solution?
a. 0.1 M
b. 0.2 M
c. 0.4 M
d. 0.6 M
e. 0.8 M
20. In 1.5 M (NH4)2SO4 , the ion concentrations are ….
a. [NH4+]=0.75M and [SO42-]=0.75M
b. [NH4+] =1.5M and [SO42-] =1.5M
c. [NH4+] = 1.5M and [SO42-]=3.0M
d. [NH4+] =3.0M and [SO42-]=1.5M
e. [NH4+] = 3.0M and [SO42-]=3.0 M
21. The equation that represents the equilibrium in a saturated solution of Fe2(SO4)3 is ….
a. Fe2(SO4)3(s)⇄3Fe2+(aq)+2SO42-(aq)
b. Fe2(SO4)3(s)⇄ 2Fe2+(aq)+3SO42-(aq)
c. Fe2(SO4)3(s)⇄ 3Fe3+(aq)+2SO42-(aq)
d. Fe2(SO4)3(s)⇄2Fe3+(aq)+3SO42-(aq)
22. Which of the following represents the equilibrium in a saturated solution of Cr2(SO4)3?
a. Cr2(SO4)3(s) ⇄ Cr2+(aq) + SO43-(aq)
b. Cr2(SO4)3(s) ⇄ Cr3+(aq) + SO42-(aq)
c. Cr2(SO4)3(s) ⇄ 2Cr2+(aq)+3SO43-(aq)
d. Cr2(SO4)3(s) ⇄2Cr3+(aq)+3SO42-(aq)
23. Which of the following is commonly used to describe the solubility of a solute?
a. mass of solute/moles of solute
b. moles of solution/mass of solute
c. mass of solute/volume of solution
d. mass of solution/volume of solutee. moles of solution/volume of solvent
24. Which of the following units is commonly used to describe solubility?
a. mL/s
b. g/min
c. g/L
d. M/L
e. L/mol
25. Which of the following would best describe the solubility of a solute?
a. litres per gram
b. moles per litre
c. grams per mole
d. grams per seconde. moles per grams
26. The Ksp expression for a saturated solution of Ca3(PO4)2 is ….
a. Ksp = [Ca2+][PO43-]
b. Ksp = [Ca2+]3[PO43-]2
c. Ksp = [Ca2+]2[PO43-]3
d. Ksp = [3Ca2+][2PO43-]
e. Ksp = [3Ca2+]3[2PO43-]2
27. The Ksp expression for calcium hydroxide is ….
a. Ksp = [Ca2+][OH-]2
b. Ksp = 1 / [Ca2+][OH-]2
c. Ksp = [Ca2+][2OH-]2
d. Ksp = 1 / [Ca2+][2OH-]2
28. If equal volumes of 0.2 M KBr and 0.2M FeSO4 are mixed, then ….
a. no precipitate will be observed
b. a precipitate of FeBr2 will be observed
c. a precipitate of K2SO4 will be observed
d. a precipitate of both K2SO4 and FeBr2 will be observed
29. Which of the following occurs when equal volumes of 0.20 M MgS and 0.20 M ZnSO4 are mixed?
a. A precipitate does not form
b. A precipitate of ZnS forms
c. A precipitate of MgSO4 forms
d. Precipitates of MgSO4 and ZnS form
30. What will happen when equal volumes of 0.20 M (NH4)2S(aq) and 0.20 M Sr(OH)2(aq) are mixed?
a. SrS precipitates.
b. NH4OH precipitates.
c. Both NH4OH and SrS precipitate.
d. No precipitate forms.
31. The complete ionic equation for the reaction between MgCl2(aq) and AgNO3(Aq) is ….
a. Ag+(aq) + Cl-(aq) → AgCl(s)
b. 2AgNO3(aq) + MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)
c. 2Ag+(aq)+Mg2+(aq)+2NO3-(aq) +2Cl-(aq) → MgCl2(s) + 2Ag+(aq)+2NO3-(aq)
d. 2Ag+(aq)+2NO3- (aq) +Mg2+(aq)+2Cl-(aq) → 2AgCl(s) + Mg2+(aq)+ 2NO3- (aq)
32. A precipitation reaction occurs when equal volumes of 0.2 M Pb(NO3)2 and 0.2 M KI are mixed. The net ionic equation for this reaction is ….
a. Pb2+(aq) + 2I-(aq) → PbI2(s)
b. PbI2(s) → Pb2+(aq) + 2I-(aq)
c. K+(aq) + NO3-(aq) → KNO3(s)
d. KNO3(s) → K+(aq) + NO3-(aq)
e. Pb(NO3)2(s) → Pb2+(aq) + NO3- (aq)
33. Which equation represents the correct reaction between Na2CO3 and Ba(NO3)2?
a. Na+(aq) + NO3-(aq) → NaNO3(s)
b. Ba2+(aq) + CO32-(aq) → BaCO3(s)
c. Na2CO3(s) → 2Na+(aq) + CO32-(aq)
d. Ba(NO3)2(aq) + Na2CO3(aq) → BaCO3(aq) + 2NaNO3(s)
34. If the solubility of Pb (OH) 2 is 0.155g/L, then the concentration of each ion in a saturated solution of a Pb(OH) 2 is ….
a. [Pb2+] = 0.155 g/L and [OH-] = 0.155 g/L
b. [Pb2+] = 0.052 g/L and [OH-] = 0.103 g/L
c. [Pb2+] = 6.43 x 10-4 mol/L and [OH-] = 1.29 x 10-3 mol/L
d. [Pb2+] = 6.43x10-4mol/L and [OH-] = 6.43 x 10-4 mol/L
35. Which of the following precipitates may form when equal volumes of AgNO3, SrCl2, and Na2CO3 are mixed together?
a. SrCO3 and AgCl
b. Ag2CO3 and AgCl
c. SrCO3 and Ag2CO3
d. SrCO3, Ag2CO3, and AgCl

COLLOID QUIZ

1. In a solution the substance that is being dissolved is called the ….
a. solvent
b. emulsifier
c. solute
d. filtrate
e. precipitate

2. Which of the following correctly describes a solute and a solvent?
a. A solute dissolves a solvent.
b. A solute is dissolved in a solvent
c. A solvent is dissolved in a solute.
d. (a) and (b).
e. (a) and (c)

3. What is a term used to describe a mixture of tiny particles that are evenly mixed and do not settle out?
a. Solvent
b. Solution
c. Solute
d. Aquous
e. Sea water

4. The best method to separate the solute from the solvent in a solution would be ….
a. distillation
b. filtration
c. sedimentation
d. precipitation
e. crystallization

5. What makes water such a good solvent?
a. Water is a good solvent because it is a negatively charged ion.
b. Water is such a good solvent because it repels most molecules
c. Water is such a good solvent because it is such a small molecule
d. Water is a good solvent due to its polarity and small molecular size

6. An example of a solution is ….
a. sugar and water
b. sand and water
c. milk
d. creamer
e. oil

7. How do concentrated solutions differ from dilute solutions?
a. Concentrated solutions contain more solute in a solvent than
equal amounts of dilute solution
b. Concentrated solutions contain less solute in a solvent than equal amounts of dilute solution.
c. Concentrated solutions contain more solvent than a dilute solution.
d. Concentrated solutions contain more solution than a dilute solution.

8. What happens when more solute is added to a saturated solution?
a. The solution becomes unsaturated.
b. The solution has to make more room for particles.
c. There is less room for the particles in the solution.
d. No more solute can dissolve.

9. Which drink probably contains the most particles?
a. a drink that contains 10 percent juice
b. a drink that contains 90 percent juice
c. a drink that contains 90 percent water
d. a drink that contains 100 percent water

10. What happens to the amount of oxygen dissolved in the ocean's surface as the water is warmed by Earth's atmosphere?
a. The amount of oxygen in the water remains unchanged.
b. The amount of oxygen in the water increases.
c. The amount of oxygen in the water decreases.
d. Fish in the water need oxygen to survive.

11. What is the size of particles in a solution?
a. More than 10,000 Angstroms
b. Between 10,000 and 100,000 Angstroms
c. Between 10 and 10,000 Angstroms
d. Molecule size

12. A solution that cannot hold any more solute at room temperature is …
a. a weak solution
b. a concentrated solution
c. a saturated solution
d. a supersaturated solution

13. What is a colloid?
a. A colloid is a kind of solution.
b. A colloid is a kind of solvent.
c. A colloid is a kind of mixture.
d. A colloid is a kind of suspension.

14. What is one property of a suspension that is different from that of a solution or a colloid?
a. If left to rest, the particles of a suspension will settle out.
b. The particles of a suspension reflect light.
c. A suspension is always clear
d. Suspensions are colorless

15. How is a colloid different than a suspension?
a. Particles are homogeneous in a colloid, but heterogeneous in a suspension.
b. Particles will scatter light in a suspension, but not in a colloid.
c. Colloids are solutions, suspensions are not.
d. Suspensions can be separated using filter paper, colloids can not.

16. Which of the following statements about suspensions is correct?
a. The particles in a suspension will not scatter light.
b. The particles in a suspension settle upon standing.
c. The particles in a suspension are homogeneous.
d. All of the above

17. The most likely cause of colloidal particles not settling out over time is ….
a. their small size
b. their bonding to the solvent particles
c. their constant motion
d. electrostatic repulsion
e. all of the above

18. An example of a colloid formed by a gas dispersed in a liquid is (2 correct)
a. foam
b. hipped cream
c. a marshmallow
d. milk

19. An example of an aerosol colloid is ….
a. paint
b. gelatine
c. hair spray
d. fog and gelatine
e. mayonnaise and paint

20. An example of a sol colloid is ….
a. paint
b. smoke
c. emulsion
d. fog
e. fog andsmoke

21. Butter is an example of colloid which the dispersing medium is … and the dispersed substance is ….
a. liquid – solid
b. gas – liquid
c. solid – liquid
d. solid – gas
e. liquid – gas

22. The type of colloid of paint is ….
a. aerosol
b. sol
c. foam
d. emulsion
e. solid emulsion

23. If the dispersing medium is gas and the dispersed substance is solid, the example of this is ….
a. smoke
b. soap
c. cloud
d. cream
e. butter

24. Solid emulsion consists of ….
Dispersing Medium Dispersed Substance
a. Gas Liquid
b. Gas Solid
c. Liquid Gas
d. Liquid Solid
e. Solid Liquid

25. An emulsion is always between ….
a. two solids
b. a solid and liquid
c. two gases
d. two liquids
e. a solid anf gas

26. An example of a colloid which is an emulsion is ….
a. wipped cream
b. mayonnaise
c. fog
d. gelatin

27. Oil floats on water. The most accurate reason for this is ….
a. oil is less dense than water
b. oil is immiscible (does not dissolve) in water
c. oil is both less dense and immiscible with water
d. water is heavier than oil

28. Oil and water can not mix each other, because ….
a. oil and water have different type of molecules
b. both substances can not attract one of another
c. oil is a non polar molecule and water is polar
d. oil is a polar molecule and water is non polar

29. To mix oil and water, we need ….
a. an emulgator
b. much water
c. much oil
d. diluting oil

30. as an emulgator, we can use ….
a. pure water
b. soap
c. pure oil
d. mineral
e. soap or mineral

31. Soap can be used as an emulgator because ….
a. it can hold water molecules
b. it can hold oil molecules
c. it can hold water and oil
d. the polar part can hold water and the non polar part can hold oil

32. The formula of a soap is ….
a. CH3COOH
b. CH3COONa
c. C17H35COOH
d. C17H35COONa
e. (C17H35COO)2Ca

33. The correct statement about a soap is ….
a. a salt
b. contains – COOH
c. has a short chain
d. the carbon chain is a polar part

34. To know that the particles of colloid always move around ….
a. Tyndall effect
b. Brown motion
c. electrophoresis
d. destilation

35. The … is the scattering of light rays as they pass through a colloid.
a. Brown Motion
b. Tyndall Effect
c. dialysis
d. electrodialysis
e. electrophoresis

36. The correct statements about colloids are …. (2 correct)
a. are permanent suspensions
b. are temporary suspensions
c. exhibit the Tyndall effect
d. do not exhibit the Tyndall effect

37. Electrophoresis can be used to know ….
a. a charge of a colloid
b. a mixture is a colloid
c. a type of colloid
d. a colloid is acid or base
e. a colloid is stable

38. In electrophoresis process, if a colloid moves to the negative electrode, the charge is ….
a. negative
b. positive
c. neutral
d. can be positive
e. can be negative

39. A charge of a colloid is tested by using electrophoresis process. The colloid moves to the positive electrode and there is a coagulation. The correct information about this evidence is ….
a. the charge is positive
b. the colloid becomes neutral
c. the charge is damage
d. the charge is opened
e. the charge is neutralized and the colloid is coagulated

40. The excess of electrolytes in a colloid can be removed by ….
a. electrolysis
b. decantation
c. electrophoresis
d. dialysis
e. precipitation

41. Dialysis: phenomenon in which small solute particles as well as solvent particles pass through a semipermeable membrane. This method can be used to ….
a. purify a colloid
b. know a colloid charge
c. dilute a colloid
d. separate a colloid
e. remove a colloid charge

42. The charge of a colloid is happened because of the ability of colloid particles to … other particles around the colloid.
a. attract
b. bond
c. link
d. adsorb
e. dissolve

43. Coagulation - the destruction of a colloid by destroying electrostatic repulsion by the following methods, except ….
a. evaporating
b. heating
c. speeds up particles and collisions remove outer layers of ions
d. addition of an electrolyte
e. removes layers of ions

44. A colloid can be destroyed by ….
a. heating
b. adding an electrolyte
c. coagulating
d. all of the above

45. The formation of “Delta” in the river because of mixing between ….
a. electrolytes from the river and colloid from the sea
b. electrolytesfrom both river and sea
c. colloid from both river and sea
d. colloid from the river and electrolytes from the sea

46. When two colloids that have different charge mix together, … will happen.
a. coagulation
b. dillution
c. evaporation
d. polarization
e. precipitation

47. If the layers of ions are removed from a colloid, … will happen.
a. coagulation
b. dillution
c. precipitation
d. solvation
e. polarization

48. Sol which has a negative charge can be coagulated fastly by adding … electrolyte
a. NaCl(aq)
b. CaCl2(aq)
c. AlCl3(aq)
d. Na2SO4(aq)
e. Na3PO4(aq)

49. Sol which has a positive charge will coagulate fastly by adding ….
a. Na3PO4
b. CaCl2
c. AlCl3
d. Ba(NO3)2
e. HCl

50. There is an unstable colloid which need to be covered with other colloid. The example of this colloid is ….
a. ink
b. milk
c. gel
d. aerosol
e. emulsion

51. A certain colloid can cover another colloid. The main colloid can … the outer colloid.
a. attract
b. bond
c. link
d. adsorb
e. dissolve

52. Sulfur sol in water is ….
a. a liofil
b. a liofob
c. a hydrofil
d. hydrofob

53. Gelatine is classified as ….
a. gel – liofil
b. sol - liofob
c. aerosol – liofil
d. aerosol – liofob

54. The correct statement about the difference between liofil and liofob is ….
a. liofil is more stable than liofob
b. liofil is more polar than liofob
c. liofil is more acidic than liofob
d. liofob is much better than liofil
e. liofob is much concentrate than liofil

55. Vitamine D is a nonpolar vitamine and so are ….
1. water soluble
2. fat soluble
3. hydrophobic
4. hydrophilic

a. 1 and 2
b. 1 and 3
c. 2 and 3
d. 2 and 4
e. 1 and 4

56. Sulfur sol can be made by … method.
a. dispersion
b. condensation
c. evaporation
d. saturation
e. coagulation

57. Sulfur sol in water can be made by
a. mixturing sulfur and water
b. using sugar to make sulfur particles are more homogen in water
c. heating sulfur in water
d. cooling sulfur before mixing

58. Sugar is needed to make a sulfur colloid. The function of sugar is ….
a. to separate sulfur molecules one of another
b. to make water easier mix with sulfur
c. to improve polarity of sulfur
d. to increase polarity of water
e. to decrease attraction between sulfur and water

59. The following colloid can be made by condensation.
1. gold sol from solid
2. paint from solid
3. AgCl sol from solution
4. sulfur sol from SO2 gas

The correct answers are ….
a. 1 and 2
b. 3 and 4
c. 1 and 3
d. 2 and 4
e. 1, 2, and 4

60. The correct answer of a colloid that made by peptisation is ….
a. Al(OH)3 is added into water
b. Al(OH)3 is added into AlCl3
c. AlCl3 is added into water
d. AlCl3 is added into HCl
e. AlCl3 is added into Al(NO3)3

61. The following colloid can be made by hydrolysis.
a. Fe(OH)3
b. AgCl
c. Au
d. S

62. Hydrolisis of FeCl3(aq) forms ....
a. H2O
b. Fe3+
c. Cl-
d. Fe(OH)3 and HCl
e. Fe(OH)3 and H+

63. Ag sol can be made from Ag+(aq) and Fe2+(aq) according to the following reaction:
Ag+(aq)+Fe2+(aq)Ag(s)+Fe3+(aq)
This method is named ....
a. dispersion
b. condensation
c. hydrolisis
d. condensation, redox
e. dispersion, physics

64. The process that can be classified as condensation is ….
a. As2S3 sol from H2S(g) + As2O3(aq)
b. S8(s) + sugar, + water
c. Gelatin(s) + hot water
d. Al(OH)3(s) + AlCl3(aq)
e. Au electrode in AuCl3(aq)

65. If Al2(SO4)3 dissolves in water, there is a colloid formed which can clean water. This colloid is ….
a. Al2(SO4)3
b. Al(OH)3
c. H2SO4
d. HAl(SO4)2
e. Al

66. The following chemicals that contains aluminium and can be used for cleaning water is ....
a. bauxite
b. tawas
c. cryolite
d. kaoline
e. aluminate

67. Al2(SO4)3 can clean water, because ....
a. It hydrolises
b. The result of hydrolisis is a colloid
c. a colloid of Al(OH)3 in water absorbs dust, poison etc.
d. aluminium reacts with water
e. aluminium hydroxide is a base

HYDROLISIS QUIZ

1. Which salt dissolved in water will give the highest pH?
a. NaCl
b. KBr
c. NaNO3
d. NH4Cl
e. NaF
2. The Ka of the weak acid HNO2 is 7.4 x 10-4. What is the Kb of its conjugate base, NO2-?
a. 7.4 x 10-4
b. 1.35 x 103
c. 1.35 x 10-11
d. 1.0 x 10-14
e. 1.8 x 10-5
3. What is the hydrolysis constant of the OBr- ion? The ionization constant of HOBr is 2.0 x 10-9.
a. 5.0 x 10-5
b. 5.0 x 10-6
c. 2.0 x 10-6
d. 5.0 x 10-9
e. 2.0 x 10-4
4. What is the hydroxide ion concentration of 0.110 M OCl-? The ionization constant of HOCl is 3.0 x 10-8.
a. 3.0 x 10-8
b. 5.1 x 10-4
c. 5.1 x 10-5
d. 1.7 x 10-4
e. 1.9 x 10-4
5. What is the hydronium ion concentration in a 0.440 M OI- solution? (Ka HOI = 2.0 x 10-11)
a. 6.7 x 10-13
b. 4.5 x 10-6
c. 3.3 x 10-3
d. 3.3 x 10-12
e. 8.0 x 10-12
6. What is the hydronium ion concentration of a 0.04 M solution of Ni2+ solution of nickel(II) perchlorate? The acidity constant of the following reaction is 5x10-10.
Ni2+(aq) + 2 H2O
Ni(OH)+(aq) + H3O+
a. 1 x 10-5
b. 1 x 10-4
c. 4 x 10-6
d. 2 x 10-5
e. 4 x 10-5
7. What is the hydronium ion concentration of a 0.1 M solution of Zn2+ solution of zinc perchlorate? The acidity constant of the following reaction is 3 x 10-10.
Zn2+(aq) + 2 H2O
Zn(OH)+(aq) + H3O+
a. 5 x 10-5
b. 2 x 10-4
c. 5 x 10-6
d. 2 x 10-6
e. 2 x 10-5
8. Consider the following salts. Which one(s) when dissolved in water will produce a neutral solution?
1) CoBr2
2) (NH4)2S
3) CaBr2
a. 2 and 3
b. only 2
c. only 1
d. 1 and 2
e. only 3
9. Consider the following salts. Which one(s) when dissolved in water will produce an acidic solution?
1) NH4Cl
2) KHSO4
3) NaCN
a. only 1
b. 2 and 3
c. only 3
d. only 2
e. 1 and 2
10. Consider the following salts. Which one(s) when dissolved in water will produce a basic solution?
1) NaNO3
2) K2S
3) Na2CO3
a. only 3
b. only 1
c. 1 and 2
d. only 2
e. 2 and 3
11. What is the pH of a 0.10 M C6H5O- solution? The Ka of C6H5OH is 1.0x10-10
a. 11.50
b. 10.51
c. 10.82
d. 11.20
e. 11.04
12. Sodium propionate, NaC3H7O2, is used as a food preservative. Calculate the pH of a 0.20 M solution of sodium propionate given Ka = 3.4 x 10-5 for propionic acid.
a. 8.89
b. 7.92
c. 7.64
d. 8.61
e. 9.22
13. What is the pH of a 0.68 M CN- solution? (Ka of HCN = 4.4 x 10-10)
a. 11.60
b. 11.10
c. 10.80
d. 11.30
e. 10.60
14. What is the pH of a 0.44 M OI- solution? (Ka of HOI=2.0x10-11)
a. 12.17
b. 12.46
c. 11.62
d. 11.83
e. 12.01
15. What is the molarity of a potassium hydroxide solution if 50.0 mL of it neutralizes 25.0 mL of a .250 M solution of sulfuric acid?
a. 0.10 M
b. 0.15 M
c. 0.20 M
d. 0.25 M
e. 0.30 M

pH OF ACID AND BASE QUIZ

1. The pH of water at 298K is ….
a. equal to pOH
b. less than 7
c. greater than 7
d. equal to ½ pKw
e. less than ½ pKw
2. HCl(aq) 0,02 M 100 mL. The pH of this solution is ….
a. 2
b. 2 – log 2
c. 2 + log 2
d. 3 – log 2
e. 3 + log 2
3. If 4 g of NaOH(s) is added to water and the volume of solution is 250 mL, the pH is …. (Ar Na=23,O=16,H=1)
a. 13 – 2 log 2
b. 13 – log 2
c. 13
d. 13 + log 2
e. 13 + 2 log 2
4. HCl(aq) 0,1 M 10 mL + HCl 0,3 M 10 mL. The pH is ….
a. 1
b. 1 – log 2
c. 1 + log 2
d. 2 – log 2
e. 2
5. NaOH(aq) 0,2 M 20 mL + Ba(OH)2(aq) 0,4 M 20 mL. The pH is ….
a. 1
b. 1 – log 2
c. 1 – log 3
d. 2 – log 2
e. 2 – log 3
6. The pOH of a solution that has [H+] = 1.7 x 10-9M is ….
a. 5.22
b. 8.78
c. 4.39
d. 3.56
e. 11.64
7. A solution of 0.012 M niacin has a hydronium ion concentration of 4.1 x 10-4 M. The pH of the solution is ….
a. 4.61
b. 2.80
c. 3.39
d. 3.61
e. 4.39
8. The pH of an aqueous solution which is 0.0020 M HClO4 is ….
a. 1.30
b. 2.30
c. 2.70
d. 2.00
e. 1.70
9. The hydroxide ion concentration of the oceans is about 1.4 x 10-6. What is the pH?
a. 5.85
b. 8.85
c. 7.85
d. 7.15
e. 8.15
10. The hydroxide ion concentration of lemon juice is about 2.0 x 10-12. What is the pH?
a. 12.30
b. 1.30
c. 10.70
d. 2.70
e. 2.30
11. The pH of human muscle fluids is 6.80. The [H3O+] in muscle fluid at 25oC is ….
a. 1.6 x 10-8
b. 1.6 x 10-7
c. 1.6 x 10-6
d. 6.6 x 10-7
e. 6.6 x 10-8
12. The pH of the contents of the human stomach is about 1.0. The value of [H3O+] in the stomach at 25oC is ….
a. 1
b. 0.1
c. 1 x 10-13
d. 1 x 10-14
e. 0.01
13. The pH of a saturated solution of Mg(OH)2 is 10.50. The molarity of the magnesium ion is ….
a. 5.0 x 10-10
b. 3.2 x 10-4
c. 1.6 x 10-3
d. 3.2 x 10-3
e. 1.6 x 10-4
14. A solution of morphine (a narcotic) has a pH of 9.61. The [OH-] is ….
a. 4.1 x 10-6
b. 2.4 x 10-11
c. 4.1 x 10-4
d. 2.4 x 10-10
e. 4.1 x 10-5
15. The pOH of a 0.001 M solution of ammonia is _____ the pOH of a 0.001 M solution of potassium hydroxide.
a. less than
b. greater than
c. the same as
d. equal to
16. The pOH of an NH3 solution is ….
a. equal to 7
b. greater than 7
c. less than 7
d. around 7
e. far to 7
17. If the pH of a solution is equal to 11, the solution is ….
a. amphoteric
b. neutral
c. acidic
d. basic
18. As the [H+] increases ….
a. the pH decreases
b. the pH increases
c. the [OH-] decreases
d. the [OH-] increases
19. A solution whose pH is equal to 4.0 has a hydrogen ion concentration of ….
a. 1 x 104 M
b. 1 x 10-4 M
c. 1 x 10-10 M
d. 1 x 1010 M
20. If the pH of a solution is equal to 3, the hydroxide ion concentration is ….
a. 1 x 1011 M
b. 1 x 103 M
c. 1 x 10-3 M
d. 1 x 10-11 M
21. The pH of a solution whose hydroxide ion concentration is 0.0010 M is ….
a. 11.00
b. 9.00
c. 3.00
d. -3.00
e. -11.00
22. A solution whose pH is equal to 12 ….
a. has more hydroxide ions than hydrogen ions
b. is acidic
c. has more hydrogen ions than hydroxide ions
d. has a pOH equal to 12
23. A solution with a pH equal to 2 has a pOH equal to ….
a. 2
b. 12
c. 16
d. 4
24. The pH of a solution whose hydronium ion concentration is 1 x 10-5 M is ….
a. 5
b. 7
c. 9
d. 11
e. 13
25. A solution whose pOH is equal to 6 has a hydrogen ion concentration of ….
a. 1 x 10-5 M
b. 1 x 10-8 M
c. 1 x 10-6 M
d. 1 x 108 M
e. 1 x 109 M
26. In a particular solution, [H+] = 1.7 X 10-9M. The pH is ….
a. 23
b. 8.77
c. 4.39
d. 7.00
e. 12.64
27. A solution has [H+] = 1.54 X 10-4M. How many significant figures does the pH have?
a. 2
b. 3
c. 4
d. 1
e. 5
28. The [OH-] in a solution that has a pH of 5.40 is ….
a. 3.98 X 10-6M
b. 2.51 X 105M
c. 1.59 X 10-5M
d. 2.51 X 10-10M
e. 2.51 X 10-9M
29. A solution has [HC2H3O2] = 1.5 X 10-2M. The pH of this solution will be _____ the pH of a 1.5 X 10-2M solution of HCl.
a. greater than
b. the same as
c. less than
30. What concentration of HOCl (Ka = 3.5 x 10-8) has the same pH as that of 2.50 x 10-4 M HNO3?
a. 3,93M
b. 1,79M
c. 0,56M
d. 3,5 x 10-2
e. 6,8 x 10-8
31. What is the pH of a sample of gastric juice whose hydronium ion concentration is 4.5 x 10-2 M?
a. 2.35
b. 1.65
c. 1.15
d. 0.65
e. 1.35
32. The pH of the world's oceans is 8.15. The [H3O+] in the ocean is ….
a. 8.1 x 10-15
b. 7.1 x 10-8
c. 1.4 x 10-8
d. 1.4 x 10-9
e. 7.1 x 10-9
33. What is the pH of human muscle fluid in which the hydronium ion concentration is 1.6 x 10-7 M?
a. 7.16
b. 7.20
c. 7.80
d. 6.20
e. 6.80
34. A vinegar has a hydroxide ion concentration of 1.3 x 10-12 M. What is the pH of the vinegar?
a. 3.11
b. 3.88
c. 2.89
d. 2.11
e. 11.89
35. The hydroxide ion concentration of lemon juice is about 2.0 x 10-12. The pH is ….
a. 2.70
b. 12.30
c. 1.30
d. 2.30
e. 10.70
36. A detergent solution has a pH of 11.63. What is the [OH-]?
a. 2.3 x 10-12
b. 4.3 x 10-2
c. 4.3 x 10-3
d. 2.3 x 10-2
e. 6.3 x 10-3
37. The pH of a saturated solution of Mg(OH)2 is 10.50. The molarity of the magnesium ion is ….
a. 5.0 x 10-10
b. 1.6 x 10-3
c. 1.6 x 10-4
d. 3.2 x 10-4
e. 3.2 x 10-3
38. The pH of indicators.
Indicators pH Color
MO 3,2 - 4,4 red - yellow
MR 4,4 - 6,3 red - yellow
BTB 6,0 - 7,6 yellow - blue
PP 8,2 – 10,0 colorless - red

The correct color when these indicators are added to HClaq) are ....
a. MO, yellow – PP, colorless
b. MM, red – PP, red
c. BTB, blue – MJ, yellow
d. PP, red – BTB, yellow
e. MJ, red – PP, colorless
39. X(aq) is turning blue litmus to red color. If it is used MR, the color becomes red. The correct properties of this solution are ....
a. acid, pH < 4,4 b. acid, pH = 4,4 c. neutral, pH > 6,3
d. neutral, pH = 7
e. base, pH > 6,3
40. The pH of a solution is about 7. The correct statement of this solution is ….
a. PP, the solution becomes red
b. BTB, the solution becomes green
c. MR, the color changes to red
d. MO, the color changes to orange
e. red litmus becomes blue

BUFFER SOLUTION QUIZ

1. Of the following mixtures, _____ is a buffer solution.
a. 1.0 M NH3/1.0 M NH4Cl
b. 1.0 M HCl/1.0 M NaCl
c. 1.0 M NaOH/1.0 M NaCl
d. 1.0 M KCl/1.0 M KOH
e. 1.0 M H2SO4/1.0 M K2SO4
2. A buffer solution may be prepared by using a weak acid and a salt containing ….
a. anion
b. cation
c. anion and cation
d. its conjugate base
e. its conjugate acid
3. A(n) _____ solution is one that resists change in pH when an acid or base is added to it.
a. buffered
b. acid
c. salt
d. aqueous
e. base
4. Of the following mixtures, _____ is a buffer solution.
a. 1.0 M NaOH/1.0 M NaCl
b. 1.0 M HCl/1.0 M NaCl
c. 1.0 M HF/1.0 M KF
d. 1.0 M KCl/1.0 M CH3COOH
e. 1.0 M HNO3/1.0 M KNO3
5. A buffer solution must contain (at least) ….
a. An acid and a base.
b. Any acid salt.
c. Water and a metal ion.
d. A conjugate pair containing at least one weak acid or one weak base.
e. Only a base salt.
6. Which of the following combinations will produce a buffer solution?
a. HCl and Cl-
b. NaCl and NaOH
c. SO42- and SO32-
d. HC2H302 and NaC2H3O2
e. HNO3 and HCl.
7. The Ka values for HF and HNO2 are 6.8 x 10-4 and 4.5 x 10-4 respectively. Therefore it follows the HF is a _____ acid than HNO2 and F- is a _____ base than NO2-.
a. weaker, stronger
b. stronger, stronger
c. stronger, weaker
d. weaker, weaker
8. The Ka values for HSO4- and H2PO4- are 1.2 x 10-2 and 6.3 x 10-8 respectively. Therefore it follows the HSO4- is a _____ acid than H2PO4- and SO42- is a _____ base than HPO42-.
a. weaker, weaker
b. weaker, stronger
c. stronger, weaker
d. stronger, stronger
9. alues for HPO42- and HSO3- are 4.8 x 10-13 and 6.3 x 10-8 respectively. Therefore it follows the HPO42- is a _____ acid than HSO3- and PO43- is a _____ base than SO32-
a. stronger, weaker
b. weaker, weaker
c. weaker, stronger
d. stronger, stronger
10. What change will occur for the following reaction if a few drops of HCl are added?
CH3CO2H + H2O
CH3CO2- + H3O+
a. a decrease in the fraction of acid dissociated
b. an increase in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
11. What change will be observed for the following reaction if a few drops of NaOH are added?
HNO2 + H2O NO2- + H3O+
a. an increase in the fraction of acid dissociated
b. a decrease in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
12. What change will occur for the following reaction if the hypochlorous acid solution is diluted from 0.1 to 0.01 M?
HOCl + H2O OCl- + H3O+
a. an increase in the fraction of acid dissociated
b. a decrease in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
13. What is the hydronium ion concentration of a solution of 0.480 M acid and 0.680 M of its conjugate base if the ionization constant is 5.78 x 10-7?
a.2.77 x 10-7
b.3.93 x 10-6
c.8.19 x 10-9
d.4.08 x 10-7
e.8.50 x 10-7
14. What is the hydronium ion concentration of a solution of 0.700 M acid and 0.440 M of its conjugate base if the ionization constant is 3.59 x 10-8?
a. 8.98 x 10-8
b. 2.47 x 10-7
c. 1.13 x 10-7
d. 5.71 x 10-8
e. 2.26 x 10-8
15. What is the hydronium ion concentration of a solution of 0.720 M acid and 0.240 M of its conjugate base if the ionization constant is 4.38 x 10-6?
a. 6.08 x 10-6
b. 1.05 x 10-6
c. 3.15 x 10-5
d. 1.31 x 10-5
e. 1.46 x 10-6
16. What is the pH of a solution of 0.81 M acid and 0.35 M of its conjugate base if the ionization constant is 5.45 x 10-8?
a. 6.42
b. 6.70
c. 7.33
d. 6.90
e. 7.63
17. What is the hydronium ion concentration of a solution of 0.720 M acid and 0.240 M of its conjugate base if the ionization constant is 4.38 x 10-6?
a. 6.08 x 10-6
b. 1.05 x 10-6
c. 3.15 x 10-5
d. 1.31 x 10-5
e. 1.46 x 10-6
18. What is the pH of a solution of 0.81 M acid and 0.35 M of its conjugate base if the ionization constant is 5.45 x 10-8?
a.6.42
b.6.70
c.7.33
d.6.90
e.7.63
19. What is the pH of a solution of 0.28 M acid and 0.73 M of its conjugate base if the ionization constant is 3.75 x 10-9?
a.9.58
b.9.32
c.9.12
d.8.84
e.8.01
20. What is the pH of a solution of 0.49 M acid and 0.29 M of its conjugate base if the ionization constant is 5.92 x 10-8?
a.7.98
b.8.21
c.7.72
d.7.00
e.7.46
21. What is the pH of a solution of 0.17 M acid and 0.81 M of its conjugate base if the pKa = 8.62?
a.9.68
b.8.58
c.7.94
d.9.30
e.9.52
22. What is the pH of a solution of 0.28 M acid and 0.54 M of its conjugate base if the pKa = 7.93?
a.7.40
b.7.65
c.7.00
d.8.21
e.7.22
23. What is the pH of a solution of 0.65 M acid and 0.51 M of its conjugate base if the pKa = 5.30?
a.5.85 d. 5.41
b.6.05 e. 5.19
c.5.62
24. The toxic compound 2,4-dinitrophenol (used in biological research to inhibit energy production in cells) has Ka = 1.1 x 10-4 M. In an experiment, a solution of 2,4-dinitrophenol was prepared with the pH adjusted to 7.40. Calculate the ratio of the concentrations of the dissociated ion to the undissociated acid.
a. 1.2 x 102
b. 3.2 x 103
c. 1.4 x 101
d. 2.8 x 103
e. 4.7 x 103
25. Acetylsalicylic acid (aspirin) can have a serious effect on the stomach. Only the undissociated acid can cross the stomach lining. Calculate the ratio of acid to dissociated ion when the pH of the stomach is 2.00. The Ka of this acid is 2.75x10-5.
a.4.8 x 102 d. 35
b.1.2 x 102 e. 3.6 x 102
c.52
26. Uric acid is one metabolic end product and is excreted from the body in urine. The acid dissociation constant of uric acid is Ka = 4.0 x 10-6 M. The pH of a urine sample is 6.00. What is the ratio of urate ion to uric acid in the urine?
a.24
b.1.5
c.6.0
d.4.0
e.0.25
27. A buffer solution is prepared by the addition of 20.0 grams of HF and 21.0 grams of NaF to enough water to make 1.000 L of solution. The Ka of HF is 7.2 x 10-4. What is the pH of this solution?
a. 3.44
b. 3.14
c. 2.84
d. 7.0
e. 2.4
28. Which of the following pairs of compounds dissolved together in aqueous solution would NOT make a good buffer solution?
a. HNO3/NaNO3
b. H3PO4/NaH2PO4
c. H2CO3/KHCO3
d. HCN/KCN
29. We desire to make a buffer solution with a pH of 9.2. Which combination of compounds would be the best to use? Refer to the table of bases given.
a. HAc/NaAc
b. NH3/NH4Cl
c. HCl/NaCl
d. pyridine/pyridine chloride
30. A solution is prepared which is 1.0 M acetic acid. What would happen to the pH of this solution if potassium acetate were added to the solution?
a. pH would go up
b. pH would go down
c. would not affect the pH
31. An aqueous solution of NH3 is in equilibrium. Suppose a gram of NH4Cl is added to the solution, and it is allowed to come to a new equilibrium. What will happen to the pH as a result of addition of NH4Cl?
a. It will go down.
b. It will go up.
c. It will remain unaffected.
32. A buffer solution is 0.10 M HAc (acetic acid) and 0.10 M NaAc (sodium acetate) and we have 1.000 Liter of it.
What is the pH after 0.010 moles of HCl are added to this solution?
a. -2.0
b. 4.74
c. 4.82
d. 2.0
e. 4.65
33. A buffer solution has a pH = 5.5. What is the [H3O+] concentration?
a. 5.5 M
b. 3.16 x 10-6 M
c. 3.2 x 105 M
d. 0.74 M
e. 3.2 x 10-3 M
34. An indicator symbolically given as HIn can be in two different forms: as HIn (red) or as In- (yellow). The pKa of the indicator is 4.0. What will be the color of the indicator in a solution which has a pH = 7?
a. red
b. yellow
c. a color intermediate between yellow and red
35. Calculate the pH of a solution which is formally 0.50 M HAc and 0.10 M NaAc.
a. -2.5
b. 4.74
c. 5.44
d. 2.52
e. 4.04
36. A solution is prepared which is 1.0 M HOCl and 1.0 M NaOCl. What is its pH?
a. 0.0
b. 3.72
c. 7.0
d. 7.45
37. A solution is prepared which is 1.0 M HCl and 1.0 M NaCl. What is its pH?
a. -1.0
b. 1.0
c. 0.0
d. 7.0
e. 4.74
38. A 1.00 Liter buffer solution is prepared which is 1.0 M in HAc and 1.0 M in NaAc. What would be the pH after 10.0 grams of NaOH were added to the solution?
a. 7.00
b. 4.74
c. 4.52
d. 5.74
e. 4.96
39. What is the H+(aq) concentration of 0.10 M NaAc(aq)?
a. 1.34 x 10-9 M
b. 7.45 x 10-6 M
c. 1.0 x 10-7 M
d. 1.34 x 10-3 M
e. 7.45 x 10-12 M
40. The indicator bromocresol green, given symbolically as HIn, can be in two different forms: as HIn the color of the indicator is yellow, as In- the color of the indicator is blue, and an equilmolar mixture of the two species is green. The Ka of the indicator is 2.5x10-5. What will be the color of the indicator in a solution which has a pH = 3.8?
a. colorless
b. green
c. blue
d. yellow
41. A solution is prepared in which 1.0 mole of NaNO2 and 1.5 moles of HNO2 are added to a liter of aqueous solution. What is the pH of this solution?
a. 3.17
b. 3.35
c. 3.52
d. 0.176
e. 0.176
42. Suppose 3.65 grams of HCl are added to the solution in #6. What will be the new pH of the solution?
a. 2.75
b. 3.35
c. 3.60
d. 3.24
e. 3.10
43. Which salt would produce a solution with a pH significantly greater than 7.0?
a. NH4Cl
b. NaOCl
c. KCl
d. NaI
e. K2SO4
44. What is the [H+] concentration of a 0.500 M solution of NaF?
a. 2.0 x 10-13 M
b. 1.0 x 10-9 M
c. 1.0 x 10-5 M
d. 4.0 x 10-9 M
e. 2.6 x 10-6 M
45. Calculate the pH of a solution which is 2.0 M NH3 and 2.0 M NH4Cl.
a. 2.22
b. 4.74
c. 7.0
d. 9.26
e. 11.77
46. What is the Kb of the NO2- species?
a. 3.35
b. 10.6
c. 4.5 x 10-4
d. 2.2 x 10-11
e. 1.0 x 10-14
47. A flask originally contains 100.0 mL of 0.500 M aqueous HAc solution. To this solution is added 50.0 mL of 0.400 M NaOH solution. Calculate the pH of the resulting solution.
a. 4.56
b. 4.74
c. 4.96
d. 4.34
e. 2.52
48. When a weak acid is titrated with a strong base the following pH curve is obtained. What is the approximate pKa of the weak acid?
a. 1
b. 3
c. 4
d. 7
e. 14

ACID AND BASE QUIZ

1. There are three different theories of acid and base. According to the Arrhenius theory, the correct strong acids are ….
a. HBr and HF
b. HNO3 and HI
c. HOCl and HOCl2
d. HCOOH and HF
e. CH3COOH and H2SO4
2. Organic acids contain a carboxyl group— a group that contains an acidic hydrogen that can ionize. The formula for the carboxyl group is ….`
a. –NH2
b. –OH
c. –CH3
d. –OCH3
e. –COOH
3. From the following acids, the correct weak acids are ….
a. H2SO4, HI
b. HCl, HBr
c. HNO2, HF
d. HNO3,H2SO3
e. HClO4, HClO
4. Which of the following is the weakest acid?
a. HCl
b. HClO
c. HBr
d. HBrO
e. HI
5. Which of the following acids is a diprotic, weak acid?
a. carbonic acid
b. hydrochloric acid
c. perchloric acid
d. acetic acid
e. sulphuric acid
6. A base used in the manufacture of soap is ….
a. calcium hydroxide
b. sodium hydroxide
c. ammonia
d. zinc hydroxide
e. barium hydroxide
7. Of the following solution, … is turning blue litmus red.
a. orange juice
b. lemon juice
c. vinegar
d. ammonia
e. table salt
8. A common substance that contains acetic acid is ….
a. vinegar
b. ammonia water
c. salad oil
d. soap
e. table salt
9. Of the following, _____ is not a characteristic of an acid.
a. tasting sour
b. turning red litmus blue
c. turning blue litmus red
d. contain H atom in its formulae
e. producing hydrogen ions in solution
10. Of the following, _____ is not characteristic of a base.
a. turning red litmus blue
b. tasting bitter
c. producing hydroxide ions in solution
d. producing a solution with a pH < 7 11. When dissolved in water, salts …. a. are nonelectrolytes b. have a bitter taste c. are electrolytes d. release hydrogen ions e.release hydroxide ions 12. A base can be prepared by the reaction between …. a. an active nonmetal with water b. a gas with water c. a sulfide with water d. an active metal with water 13. Of the following, the property that most closely relates to acids is …. a. bitter taste b. contains hydroxide polyatomic ion c. sour taste d. salty taste 14. When an acid is dissolved in water, it usually forms …. a. hydrogen ions b. hydroxide ions c. no ions d. chloride ions e. simple molecules 15. The acid used in the storage battery in your car is …. a. nitric acid b. hydrochloric acid c. tartaric acid d. sulfuric acid e. acetic acid 16. The sour taste of lemons and limes is due to a substance called …. a. acetic acid b. citric acid c. hydrochloric acid d. carbonic acid e. oxalate acid 17. In the following reaction, … is a base. HClO4(aq)+KOH(aq) --> KClO4(aq)+H2O(l)
a. KOH
b. H2O
c. HClO4
d. KClO4
e. KClO4 and H2O
18. The conjugate base of acetic acid (CH3COOH) is ….
a. CH3COO-
b. CH3COOH2+
c. CH2COO2-
d. CHCOO3-
e. CCOOH2-
19. The conjugate acid of the weak base methylamine (CH3NH2) is ….
a. CH3N2-b. CH3NH-c. CH3NH3+d. CH3NH3-e. CH3NH42+
20. Hydrazine (N2H4), formerly used as a rocket fuel, is a base. What is its conjugate acid?
a. N2H4- d. N2H5+ b. N2H3+ e. N2H5 c. N2H5-
21. In terms of base strength, OH- is … CH3COO-.
a. stronger than
b. weaker than
c. the same as
d. different with
e. similar with
22. Which definition of an acid is more restrictive? In other words, which definition includes fewer substances in its definition of an acid?
a. Lewis
b. Arrhenius
c. Brønsted-Lowry
d. Arrhenius and Lewis
e. Arrhenius and Bronsted-Lowry
23. Conjugate acid-base pair is ….
a. an acid and base that react to form water
b. a pair of acids with similar structures
c. two substances related by the donation/acceptance of a proton
d. two substances that have the same acid-base effect in water.
24. Which of the following pairs does not represent a conjugate acid-base pair?
a. HClO4 / ClO4-
b. HCl / Cl-
c. H2SO4 / SO42-
d. H2O / OH-
e. NH3 / NH4+
25. Identify the Brønsted-Lowry acids and bases (conjugate pairs) in the following equation. (A= B-L acid; B= B-L base)
HC2H3O2 + CN- = HCN + C2H3O2–
a. B A B A
b. B B A A
c. A B A B
d. A B B A
e. B A A B
26. The conjugate of a weak base is …
a. a strong base
b. a weak base
c. a strong acid
d. a weak acid
e. None of these
27. Which of these is the weakest conjugate base?
a. NH2–
b. Cl-
c. C2H3O2–
d. CN-
e. SO42–
28. NH3 + H2O Û NH4+ + OH-
The correct statement is ….
a. NH3 is acid
b. NH4+ is conjugate acid of NH3
c. H2O is base
d. OH- is conjugate base of NH4+
e. NH3- and H2O are conjugate acid and conjugate base
29. H2O + HCO3- Û H2CO3 + OH- The bases are ….
a. H2O and HCO3-
b. H2CO3 and H2O
c. H2CO3 and OH-
d. H2O and OH-
e. HCO3- and OH-
30. From the above equation, the correct statement is ….
a. H2O is a weak acid
b. HCO3- is neutral
c. OH- is a weak base
d. H2CO3 is a weak acid
31. H2O + HCN ↔ CN- + H3O+
In this equation ….
a. HCN is a base
b. H2O and HCN are a weak base and a weak acid
c. H3O+ is a base
d. CN- is a conjugate acid of HCN
32. H2O + HSO4- ↔ SO42- + H3O+
The wrong statement is ….
a. as an acid, HSO4- is weaker than H3O+
b. as a base, HSO4- is stronger than H3O+
c. as an acid, H2O is weaker than H3O+
d. H2O is stronger than SO42-
33. Known 5 equations below:
1. H2O + NH3 ↔ NH4+ + OH-
2. H2O + HF ↔ H3O+ + F-
3. H2O + NH3 ↔ NH2- + H3O+
4. H2O + HCN ↔ CN- + H3O+
5. H2O + HSO4- ↔ SO42- + H3O+
Occording to Bronsted–Lowry, H2O as an acid and a base are in number ....
a. 1 and 2
b. 2 and 3
c. 2 and 4
d. 2 and 5
e. 4 and 5
34. The difference between acid and conjugate base is ….
a. a proton
b. a neutron
c. an electron
d. a nucleus
e. none of these
35. A substance that may act as both an acid and a base is ….
a. a hydride
b. a hydroxide
c. disproportionate
d. amphoteric
e. a salt
36. Which of the following would be the most basic substance in aqueous solution?
a. HSO4-
b. F-
c. I-
d. Cl-
e. NO3-
37. Which of the following would be the most acidic substance in aqueous solution?
a. Na+
b. SO42-
c. H2O
d. NH2-
e. NH4+
38. According to the Lewis theory, a base ….
a. is a proton acceptor.
b. is a proton donor.
c. makes available a share in a pair of electrons.
d. is any compound that contains electron pairs.
e. accepts a share in a pair of electrons.
39. Which statement concerning the autoionization (self-ionization) of water is FALSE?
2 H2O(l) <==> H3O+ + OH-(aq)
a. This reaction is an acid-base reaction according to the Bronsted-Lowry theory.
b. ater is amphiprotic.
c. A H2O molecule may react as an acid by donating a proton.
d. In this reaction H3O+ and OH- are a conjugate acid-base pair
e. A H2O molecule may react as a base by accepting a proton.
40. To prepare 1.0 L of a 0.100 M solution of phosphoric acid, the volume (mL) of the concentrated solution (15 M) which needed is ….
a. 6.7 b. 6.67 c. 20.0 d. 2.2 e. 2.0
41. Barium hydroxide is a strong base. Compute [Ba2+] and [OH-] for a solution that is prepared by dissolving 6.0 x 10-2 mole of barium hydroxide in 500.0 mL of water. (Ar Ba = 137.33, O = 16.00, H = 1.008)
a. 1.2 x 10-2, 2.4 x 10-2
b. 1.2 x 10-1, 1.2 x 10-1
c. 1.2 x 10-1, 2.4 x 10-1
d. 1.2 x 10-2, 1.2 x 10-2
e. 2.5 x 10-1, 1.2 x 10-1
42. Calculate the [ClO4-], and [H3O+] in an aqueous solution containing 0.025 moles of HClO4 in 500.0 mL of water.
a. 2.0 x 10-12, 5.0 x 10-2
b. 5.0 x 10-2, 2.0 x 10-12
c. 5.0 x 10-2, 5.0 x 10-2
d. 2.0 x 10-13, 5.0 x 10-1
e. 5.0 x 10-2, 2.0 x 10-2
43. The normality of a solution of sulfuric acid that is 0.200 M is ….
a. 0.200N b.0.400N c. 0.100N d. 0.196N e. 0.980N
44. A bottle of wine vinegar contains 6.5HC2H3O2 by mass. If vinegar has a density of 1.03 g/ml, how many grams of HC2H3O2 are in a 400 ml bottle?
a. 13g b. 35g c. 27g d. 260g e. 6g
45. Glacial acetic acid has a density of 1.05 g/ml. If 46.2 of HC2H3O2 will dissolve in 1.0g of water, the molarity of the solution is ….
a. 14M b. 17M c. 4M d. 5M e. 36M
46. Glacial acetic acid is a saturated solution. If 46.2 g of HC2H3O2 will dissolve in 1.0g of water, the mass percent acetic acid is ….
a. 90 b. 98 c. 102 d. 47 e. 2
47. When 25.00 mL of 0.250 M potassium hydroxide solution reacts with 20.00 mL of 0.500 M sulfuric acid solution, _____ moles of water will be produced.
a. 5.00 x 10-3
b. 13.0 x 10-3
c. 100 x 10-3
d. 6.25 x 10-3
e. 3.75 x 10-3
48. How many mL of water must be added to 50 mL of 0.100M HCl to dilute it to 0.033M?
a. 151 b. 75 c. 101 d. 61 e. 201
49. What is the normality of 100g of H2SO4 dissolved in 1L of H2O?
a. 1.0 b. 2.1 c. 0.55 d. 10.5 e. 3.6
50. How many millimoles of H+ are there in 50.0 mL of 0.10 M HCl?
a. 50.0 mol
b. 20.0 mol
c. 5.0 mol
d. 2.0 mol
e. 0.5 mol
51. How many mmol OH- are there in 20.0 mL of 0.010 M Ba(OH)2?
a. 0.40 mmol
b. 0.20 mmol
c. 0.02 mmol
d. 0.04 mmol
e. 0.08 mmol
52. What is the molarity of 250.0 mL of a solution which contains 25.0 mmol of H+?
a. 2.5 M d. 1.0 M
b. 0.5 M e. 0.25 M
c. 0.1 M
53. Given the following Ka values, determine which species is the strongest base.
H2SO3 1.2 x 10-2 HNO2 4.5 x 10-4 HCNO 3.5 x 10-4
a. H2SO3
b. NO2-
c. HNO2
d. HSO3-
e. CNO-
54. The Ka values for HCNO and HNO2 are 2.2 x 10-4 and 4.5 x 10-4 respectively. Therefore it follows the HCNO is a acid than HNO2 and CNO- is a _____ base than NO2-.
a. stronger, stronger
b. stronger, weaker
c. weaker, weaker
d. weaker, stronger
55 The Ka values for HS- and HPO42- are 1.2 x 10-13 and 4.8 x 10-13 respectively. Therefore it follows the HS- is a _____ acid than HPO42- and S2- is a _____ base than PO43-.
a. stronger, stronger
b. stronger, weaker
c. weaker, weaker
d. weaker, stronger
56. Based upon the following values of Ka, place the acids in order from weakest to strongest ….
HCN (Ka = 6.2 x 10-10)
HCOOH (Ka =1.78 x 10-4)
HC2H3O2 (Ka = 1.8 x 10-5)
HNO2 (Ka = 4.6x10-4)
a. HC2H3O2-HCN-HNO2-HCOOH
b. HCN-HC2H3O2-HCOOH-HNO2
c. HCN-HNO2-HC2H3O2-HCOOH
d. HCOOH-HNO2-HCN-HC2H3O2
e. HNO2-HCOOH-HC2H3O2-HCN
57. Which of the following is not true for the dissociation of a strong acid?
a. The equilibrium lies far to the right
b. equilibrium lies far to the left
c. [H+] >> [HA]
d. Ka is large
e. The conjugate base will be weak
58. What change will be observed for the following reaction if a few drops of NaOH are added?
HNO2+H2O NO2-+H3O+
a. an increase in the fraction of acid dissociated
b. a decrease in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
59. What change will occur for the following reaction if a few drops of HCl are added?
CH3CO2H + H2O --> CH3CO2- + H3O+
a. a decrease in the fraction of acid dissociated
b. an increase in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
60. Given Ka values of 1.8 x 10-4 and 6.8 x 10-4 for HCO2H and HNO2 respectively, the equilibrium constant for the following reaction is ….
HCO2- + HNO2 --> HCO2H + NO2-
a.0.26
b.8.6 x 10-4
c.5.0 x 10-4
d.1.2 x 10-7
e.3.8
61. Given Ka values of 1.0 x 10-10 and 6.8 x 10-8 for C6H5OH and C5H5NH+ respectively, the equilibrium constant for the following reaction is ….
C6H5O- + C5H5NH+
C6H5OH + C5H5N
a. 0.15
b. 6.8 x 10-8
c. 6.8 x 10-2
d. 1.5 x 10-3
e. 6.8 x 102
62. Given Ka values of 5.6 x 10-10 and 1.7 x 10-5 for NH4+ and CH3CO2H respectively, calculate the equilibrium constant for the following reaction.
NH4+ + CH3CO2- --> NH3 + CH3CO2H
a. 3.3
b. 0.30
c. 1.7 x 10-5
d. 3.0 x 104
e. 3.3 x 10-5
63. What is the hydronium ion concentration of a 0.380 M acid solution of an acid whose ionization constant is 1.58x10-9
a. 4.16 x 10-9
b. 2.45 x 10-5
c. 1.26 x 10-5
d. 6.00 x 10-10
e. 6.45 x 10-5
64. What is the hydronium ion concentration of a 0.1 M solution of Zn2+ solution of zinc perchlorate? The acidity constant of the following reaction is 3 x 10-10.
Zn2+(aq) + 2 H2O --> Zn(OH)+(aq) + H3O+
a. 5 x 10-6
b. 2 x 10-4
c. 2 x 10-6
d. 2 x 10-5
e. 5 x 10-5
65. What is the hydronium ion concentration of a 0.02 M solution of Cu2+ solution of copper(II) perchlorate? The acidity constant of the following reaction is 5x10-9
Cu2+(aq) + 2 H2O --> Cu(OH)+(aq) + H3O+
a. 1 x 10-5
b. 5 x 10-4
c. 7 x 10-5
d. 7 x 10-4
e. 1 x 10-4
66. What is the ionization constant of an acid if the hydronium ion concentration of a 0.400 M solution is 1.40 x 10-4 M?
a. 1.22 x 10-9
b. 4.90 x 10-8
c. 1.96 x 10-8
d. 1.40 x 10-3
e. 1.40 x 10-6
67. What is the acidity constant for the following reaction given that the hydronium ion concentration of a 0.04 M solution of Ni2+ solution of nickel(II) perchlorate is 4.5x10-6?
Ni2+(aq) + 2 H2O --> Ni(OH)+(aq) + H3O+
a. 4 x 10-6
b. 2 x 10-10
c. 2 x 10-12
d. 5 x 10-10
e. 5 x 10-12

ACID BASE TITRATION QUIZ

1. 50 mL of HCl(aq) is titrated with 0,10 M NaOH(aq). If the volume of NaOH needed is 60 mL, the [HCl] is ….

a. 0,08 M
b. 0,01 M
c. 0,12 M
d. 0,15 M
e. 0,20 M

2. The pH of the equivalent point is ….

a. 2
b. 5
c. < 7
d. 7
e. > 7

3. When the volume of NaOH which added to HCl(aq) is 25 mL, the pH of solution is ….

a. 1 – log 3
b. 1 + log 3
c. > 1
d. < 7
e. 7 + log 3

4. The pH after the addition of 50 mL of NaOH(aq) is ….

a. > 2
b. 2
c. 5
d. 7
e. < 7

5. The pH after the addition of 70 mL of NaOH(aq) is ….

a. 3 – 3log2
b. 3 + 3log2
c. 7
d. 11 – 3log2
e. 11 + 3log2

6. Which indicator would probably not work for detecting the endpoint, when strong acid is titrated with a strong base?

a. bromocresol purple, with a color change in the range pH = 5.2 to
b. thymol blue, with a color change in the range pH = 8.0 to 9.6
c. bromophenol blue, with a color change in the range pH = 3.0 to 4.
d. bromothymol blue, with a color change in the range pH = 6.0 to 7.6

7. If the above titration uses other indicators, which indicator would be worked?

a. MO, with a color change in the range pH = 3,1 to 4,4
b. MR, with a color change in the range pH = 4,2 to 6,2
c. PP, with a color change in the range pH = 8.3 to 10.0
d. MO or PP

Consider the following indicator ranges.
MO 3,1 – 4,4 (red – yellow)
MR 4,4 – 6,2 (red – yellow)
BTB 6,2 – 7,6 (yellow – blue)
PP 8,0–10,0 (colorless–red)
8. Which indicator(s) would be the best choice for the titration of strong acid that is titrated with strong base?

a. Methyl orange and methyl red would work best.
b. Bromothymol blue and phenolphthalein would work.
c. Methyl red would be best.
d. litmus
e. Phenolphthalein would work best.

9. Which indicator(s) would be the best choice for the titration of strong base that is titrated with strong acid?

a. MO
b. MR
c. BTB
d. PP
e. litmus

10. Which indicator(s) would be the best choice for the titration of weak acid that is titrated with strong base?

a. MO
b. MR
c. BTB
d. PP
e. litmus

11. It would require ... mL of 0.30 M hydrochloric acid solution to neutralize 20.0 mL of 0.30 M sodium hydroxide solution.

a. 15.0
b. 10.0
c. 40.0
d. 30.0
e. 20.0

12. 200.0 mL of 0.200 M HCl is titrated with 0.050 M NaOH. What is the pH after the addition of 100.0 mL of the NaOH solution?

a. 1,45
b. 1,03
c. 0,93
d. 0,82
e. 0,76

13. What is the molarity of a potassium hydroxide solution if 50.0 mL of it neutralizes 25.0 mL of a 0.250 M solution of sulfuric acid?

a. 0.10 M
b. 0.15 M
c. 0.20 M
d. 0.25 M
e. 0.30 M

14. It would require ... mL of 0.300 N sulfuric acid solution to neutralize 20.0 mL of 0.300 N sodium hydroxide solution.

a. 40.0
b. 10.0
c. 20.0
d. 30.0
e. 15.0

15. How many grams of solid sodium hydroxide may be neutralized by 150 mL of 0.150 HCl?

a. 90g
b. 1.11g
c. 9g
d. 11.2g
e. 0.9g

16. Calculate the concentration of a 25.0 mL sample of mono-protic acid if it took 31.6mL of 0.110 M NaOH to neutralize it completely.

a. 0.139
b. 0.159
c. 0.087
d. 0.87
e. 11.5

17. The stoichiometric point in an acid-base titration ….

a. will always have a pH of 7.00
b. will have a pH of 7.00 when it involves a strong acid and strong base
c. will have a pH of 7.00 when a weak acid and a weak base are used
d. will have a pH above 7.00 when a weak base and a strong acid are used
e. will have a pH below 7.00 when a weak acid and a strong base are used

18. A 25.00 mL sample of 0.100 M HCl is titrated with 0.100 M NaOH. What is the pH of the solution at the points where 24.5 and 25.5 mL of NaOH have been added.

a. 3.30, 10.70
b. 3.30, 10.00
c. 3.30, 11.00
d. 3.00, 11.00
e. 3.00, 10.00

19. What is the pH of 100.0 mL of 0.100 M HCl after 20.0 mL of 0.100 M NaOH have been added?

a. 0.98
b. 1.17
c. 1.86
d. 2.02
e. 2.42

20. What is the pH of 100.0 mL of 0.100 M HCl after 100.0 mL of 0.100 M NaOH have been added?

a.0.00
b.1.00
c.6.86
d.7.00
e.7.25

21.What is the pH of 100.0 mL of 0.100 M HCl after 150.0 mL of 0.100 M NaOH have been added?

a. 1.70
b. 5.89
c. 8.98
d. 10.78
e. 12.30

22.The pH of a titration of 0.10M HCl by 0.150M NaOH at equivalence point is ....

a. 6.85
b. 7.00
c. 7.15
d. 7.36
e. 8.20

23. What is the pH of a solution in which 25.0 mL of 0.010 M Sr(OH)2 are added to 20.0 mL of 0.020 M H2SO4?

a. 11.82
b. 11.52
c. 2.52
d. 2.48
e. 1.76

24. A 1.20 g sample of fumaric acid is dissolved in 100.0 mL of water and titrated with 0.300 M NaOH to the second equivalence point. The volume of base used is 69.0 mL. What is the molecular mass of fumaric acid which contains two dissociable protons?

a. 84
b. 116
c. 142
d. 58
e. 232

25. A 1.50 g sample of Vitamin C is dissolved in 100.0 mL of water and titrated with 0.250 M NaOH to the methyl orange equivalence point. The volume of the base used is 34.1 mL. What is the molecular mass of Vitamin C assuming one dissociable proton per molecule?

a. 139
b. 176
c. 146
d. 164
e. 152

26. 0.550 g sample of butyric acid is dissolved in 100.0 mL of water and titrated with 0.100 M NaOH to the phenolphthalein equivalence point. The volume of the base used is 62.4 mL. What is the molecular mass of butyric acid assuming one dissociable proton per molecule?

a. 140
b. 88
c. 122
d. 160
e. 46

27. A 25.00 mL sample of 0.100 M CH3CO2H is titrated with 0.100 M NaOH. What is the pH of the solution at the points where 24.0 and 24.5 mL of NaOH have been added. (Ka = 1.8x10-5)

a. 5.32, 6.13
b. 5.61, 6.44
c. 5.61, 6.13
d. 6.13, 7.00
e. 6.13, 6.43

28. A 25.00 mL sample of 0.100 M CH3CO2H is titrated with 0.100 M NaOH. What is the pH of the solution at the points where 24.0 and 26.5 mL of NaOH have been added. (Ka=1.8 x 10-5)

a. 5.61, 10.30
b. 5.61, 11.30
c. 6.44, 10.7
d. 6.13, 11.46
e. 6.13, 10.3

HYDROCARBON QUIZ

1. You encounter many organic compounds everyday. Some organic compounds are ethanol (grain alcohol) and acetone (nail polish remover). Another organic compound which can be found in the daily life is ….
a. Salt b. water c. sugar d. bone e. mineral
2. Hydrocarbon is one of the organic compound that mainly contains ….
a. Carbon d. hydrogen
b. Oxygen e. carbon and hydrogen
c. carbon and oxygen
3. Which one of the following compounds is not classified as hydrocarbons?
a. CH3CH2CH2CH3 d. CH3CH2OH
b. C10H22 e.C6H6
c. C2H2
4. Hydrocarbons are classified into two main types, aliphatic and aromatic. The following substances which can not be classified as an aliphatic hydrocarbon is ….
a. alkane are all hydrocarbons that do not contain ….
a. benzene rings d. branched chains
b. cyclic chains e. closed chains
c. opened chains
5. One example of organic compounds that have a long chain is ....
a. petroleum
b. methane
c. glucose
d.sucrose
e. alcohol
6. Closed chains of carbon atoms can be explained as ….
a. a chain which only has carbon atoms
b. a cyclic bond among carbon atoms
c. a bond among carbon atoms that form a branched chains
d. a cyclic chain which has a double bond
e. a special chain which contains carbon and hydrogen atoms
7. Cyclic chains of carbon atoms can be explained as follow, except ….
a. a bond among carbon atoms which form a ring
b. have different formulae with saturated hydrocarbons
c. a chain which is classified as closed chain
d. have the same formulae with opened chains
e. a branch-closed chain is also a cyclic chain
8. Branched chain can be ….
(1) alkane
(2) alkene
(3) alkadiene
(4) alkyne
(1) and (2)
(2) and (3)
(3) and (4)
(1), (2), and (3)
(1), (2), (3), and (4)
9. The special features of carbon below are correct, except ….
a. has tetravalence
b. forms covalence of four
c. can bond one of another
d. the atomic number is 6
e. makes possible branched chains
10. Other kinds of atoms, such as oxygen, nitrogen, and sulfur, may be attached to the carbon atoms by ….
a. single or multiple covalent bond
b. single covalent bonds
c. double covalent bonds
d. triple covalent bonds
e. multiple covalent bonds
11. The simplest organic compounds are hydrocarbons, compounds containing only carbon and hydrogen. The wrong hydrocarbon compounds is ….
a. alcohol
b. benzene
c. butane
d. gasoline
e. cyclopropane
12. A hydrocarbon in which all carbon atoms are bonded to the maximum number of hydrogen atoms is classified as … hydrocarbon
a. saturated
b. aromatic
c. alkene
d. alkyne
e. cyclic
13. The saturated hydrocarbon can be classified as ….
a. alkene
b. alkane
c. alkyne
d. alkane and alkene
e. alkene and alkyne
14. Unsaturated hydrocarbons are ….
a. alkane and alkene
b. alkane and alkyne
c. alkene and alkyne
d. alkane, alkene, and alkyne
15. A hydrocarbon that has no carbon-carbon double or triple bonds ….
a. is saturated
b. is unsaturated
c. is not branched
d. must be straight-chain
16. Which hydrocarbon contains six carbon atoms?
a. heptane
b. 2,2-dimethylbutane
c. 2-methylhexane
d. cyclopentane
17. Methane is one of the saturated hydrocarbons, because it
a. has a tetrahedral structure
b. has 4 single covalent bond
c. is bonded only to the hydrogen atoms
d. is bonded to the maximum number of hydrogen atoms
e. can bond to the maximum number of other carbon atoms
18.Methane is one of the saturated hydrocarbons, because it
a. has a tetrahedral structure
b. has 4 single covalent bond
c. is bonded only to the hydrogen atoms
d. is bonded to the maximum number of hydrogen atoms
e. can bond to the maximum number of other carbon atoms
19. The statements below are correct about carbon atom, except ….
a. group IVA in the periodic table
b. can forms single covalent bonds
c. its compounds are molecules
d. is contained in the diamond
e. has 6 electrons’ valence
20. Methane is the simplest hydrocarbon. The wrong statement about methane is ….
a. consists of one carbon atom
b. there are 8 electron’s pairs
c. four hydrogen atoms are bonded
d. has four C—H bonds
e. forms a tetrahedral structure
21. The total number of valence electrons involved in the electron dot (or Lewis) formula of methane is:
a. 4
b. 6
c. 8
d. 10
e. 12
22. The examples of saturated hydrocarbon compounds are ….
a. C2H2, C8H14
b. C5H12, C7H16
c. C5H8, C6H14
d. C3H6, C6H12
e. CH4, C4H8
23. Aromatic hydrocarbons are hydrocarbons that contain benzene rings. Benzene consists of a ring of six carbon atoms with alternating single and double carbon–carbon bonds. The molecular formula of benzene is ….
a. CH
b. C2H2
c. C3H3
d. C6H6
e. C12H12
24. To know how the atoms are bonded to one another in the hydrocarbon compounds is by looking at ….
a. molecular formula
b. structural formula
c. general formula
d. condenced formula
e. specific formula
25. A structural formula does not convey information about the three-dimensional arrangement of atoms, because this formula only shows ….
a. the kind of elements
b. the type of atoms
c. molecular formula
d. condenced formula
e. general formula
26. To look at the three-dimensional arrangement of atoms in the hydrocar-bon compounds, you would draw a three dimensional formula by ….
a. make a diagram
b. make a picture
c. make a three-dimensional picture
d. construct a model of the atoms
e. construct a model of the molecule
27. Which of the following is both the correct bond angle and molecular geometry around a carbon atom with four single bonds?
a. 120°, tetrahedral
b. 120°, planar
c. 109.5°, tetrahedral
d. 109.5°, planar
e. 104.5°, tetrahedral
28. When two carbon atoms are bonded to one another, the possible number of hydrogen atoms that form an alkane are ….
a. 2
b. 4
c. 6
d. 8
e. 10
29. The general molecular formula of alkanes is ….
a. CnHn
b. CnH2n
c. CnH3n
d. CnH2n+2
e. –CnH2n+1–
30. The general formula of alkyl is ….
a. –CH
b. –CH2
c. –CH3
d. –CnH2n
e. –CnH2n+1
31. What is the common name for the following alkyl group? - CH(CH3)2
a. Isobutyl
b. Isopropyl
c. tert-butyl
d. sec-butyl
32. A homologous series of alkanes is a series of alkane compounds in which
one compound differs from a preceding one by ….
a. –CH–
b. -CH2–
c. –CH3
d. –CnH2n–
e. –CnH2n+1–
33. Members of a homologous series have similar … properties.
a. chemical
b. physical
c. general
d. natural
e. special
34. Structures of organic compounds are often given by condensed structural formula, where condensed formula of the fourth alkane is ….
a. (CH)4
b. (CH2)4
c. CH3CHCHCH3
d. (CH3)2CHCH
e. CH3(CH2)2CH3
35. The number of C atoms primer, secunder, tertier of CH3(CH2)2CH(CH3)CH2C(CH3)3 are ….
a. 5, 1,1, 1
b. 4, 2, 1, 1
c. 5, 2, 1, 1
d. 4, 2, 2, 1
e. 4, 1, 2, 1
36. The number of hydrogens in n-nonane is
a. 6
b. 9
c. 16
d. 18
e. 20
37. Which compound is likely to have the highest boiling point?
a. n-butane
b. n-hexane
c. decane
d. C13H18
e. C8H18
38. The empirical formula of ethane is …
a. CH
b. CH2
c. CH3
d. CH4
e. C2H6
39. When organic compounds without multiple bonds are named, the carbons are numbered so that the substituents have the … possible numbers.
(1) highest
(2) lowest
(3) same
a. (1)
b. (2)
c. (3)
d. (1) and (2)
e. (1) and (3)
40. The compound 2,4-dimethylpentane has the molecular formula ….
a. C5H12
b. C8H18
c. C6H14
d. C9H18
e. C7H16
41. What is the molecular formula for a straight chain alkane having 22 carbons?
a. C22H40
b. C22H46
c. C22H42
d. C22H48
e. C22H44
42. Which one of the following hydrocarbons is a gas at room temperature and pressure?
a. Propane
b. Hexane
c. Octane
d. Nonane
e. Decane
43. Cycloalkanes are saturated hydrocarbons in which the carbon atoms form a ring; the general formula is ….
a. CnHn-2­
b. CnHn
c. CnH2n-2
d. CnH2n
e. CnH2n+2
44. When naming hydrocarbons, we look first for the … chain of carbon atoms that contains multiple bonds.
a. shortest continuous
b. longest continuous
c. shortest branch
d. longest branch
45. The compound 2,4-dimethylpentane has the molecular formula …
a. C5H12
b. C7H16
c. C6H14
d. C8H18
e. C6H12
46. CH3CH2CH3 represents the … for propane.
a. geometric isomer
b. structural isomer
c. molecular formula
d. empirical formula
e. condensed structural formula
47. What is the IUPAC name of the molecule whose carbon skeleton is shown below?
C - C - C - C - C - C - C - C - C
a. n-hexane
b. n–heptane
c. n–decane
d. n-nonane
e. n-octane
48. CH3CH2CH2CH2CH3 is named ….
a. pentane
b. hexane
c. propane
d. butane
e. heptane
49.The condensed structural formula of 4-ethyl-3-methylheptane is ….
a. CH3CH2CH(CH3)CH(C2H5)(CH2)2CH3
b. CH3CH2CH(CH3)CH(C2H5)(CH2)2CH3V
c. CH3CH2CH(CH3)CH(C2H5 )(CH2)2CH3
d. CH3CH2CH(CH3)CH(C2H5)(CH2)2CH3
e. CH3CH2CH(CH3)CH(C2H5)(CH2)2CH3
50. The best name for :
CH3CH(CH3) CH(CH2CH3)CH2CH2CH3 is ….
a. 1,1-dimethyl-2-ethylpentane.
b. 2-methyl-3-ethylhexane.
c. 4-ethyl-5-methylhexane.
d. 2-methyl-3-propylpentane.
e. 4-ethyl-5-methylhexane.
51. The IUPAC name of CH3CH2C(CH3)2(CH2)4CH3 is ….
a. 3-methyloctane
b. 3-dimethyloctane
c. 3,3-dimethyloctane
d. 3-dimethylheptane
e. 3,4-dimethyloctane
52. The unique aspect of a saturated hydrocarbon is that it must contain ….
a. only single bonds
b. single and double bonds
c. double and triple bonds
d. only carbon and hydrogen
e. single, double and triple bonds
53. The chemical formula of 2-methyl pentane is ….
a. C5H6
b. C4H8
c. C5H10
d. C6H12
e. C6H14
54. This compound is named ….
a. 3-methylpentane
b. 4-methylpentane
c. 2-methylpentane
d. methylpentane
e. dimethylbutane
55. The name of CH3CH2CHClCH3 is ….
a. chlorobutane d. 1-chlorobutane
b. 2-chlorobutane e. 3-chlorobutane
c. chloro-2-butane
56. What is the simplest cyclic alkane?
a. cycloethane d. cyclopropane
b. cyclobutane e. cyclopentane
c. cyclohexane
57. When 6 carbon atoms form a ring chain and have a single covalent bond, the possible number of hydrogen atoms are ….
a. 6 d. 12
b. 8 e. 14
c.10
58. The chemical formula of cyclohexane is ….
a. C6H6 d. C6H12
b. C6H8 e. C6H14
c. C6H10
59. The empirical formula of cyclohexane is ....
a. CH d. CH2
b. C2H e. CH3
c. C2H5
60. The name of this compound is ….
a. methylhexane
b. methylbenzene
c. hexylmethane
d. 1-methylcyclohexane
e. Methylcyclohexane
61. This compound is named ….
a. cyclohextyldimethane
b. methylcyclohexane
c. 1,3-methylcyclohexane
d. 1,3-dimethylcyclohexane
e. 1,3-dimethylbenzene
62. The above compound is named ….
a. 1,4-dichlorocyclohexane
b. 2,5-dichlorocyclohexane
c. p-dichlorobenzene
d. dichlorocyclohexane
e. 1,4-dichlorobenzene
63. How many primary carbons are in the following hydrocarbon?
a. 3 d. 8
b. 4 e. 15
c. 5
64. In the condensed structural formulas of cycloalkanes, a carbon atom and its attached hydrogen atoms are assumed to be at each ….
a. side d. chain
b. corner e. ring
c. branch
65. Benzene has the molecular formula … and the empirical formula ….
a. C6H6 and CH
b. C6H12 and CH2
c. C6H14 and C3H7
d. C6H10 and C3H5
e. C6H8 and C3H4

CHEM QUIZ THIRTH SEMESTER

Choose the correct answer!

1. Which of the following sets of quantum numbers describes the most easily removed electron in an aluminum atom in its ground state?
a. n = 3, l = 1, ml = -1, ms = -1/2
b. n = 1, l = 0, ml = 0, ms = -1/2
c. n = 4, l = 1, ml = 1, ms = +1/2
d. n = 3, l = 0, ml = 0, ms = +1/2
e. n = 2, l = 1, ml = 0, ms = -1/2

2. The electronic configuration which represents an atom in the excited state is...
a. 1s2 2s2 2p5
b. 1s2 2s2 2p6
c. 1s2 2s2 2p6 3s2
d. 1s2 2s2 2p5 3s1
e. 1s2 2s2 2p6 3s1

3. The position of an element with the electron configuration (Ar) 4s2 3d10 4p3 in the Periodic Table is in the … (…) group, … period, and … block.
a. 5 (VA), 4, s
b. 5 (VB), 4, p
c. 8 (VIIIA), 4, s
d. 15 (VA), 4, p
e. 15 (VB), 4, d

4. If F3 and NH3 molecules are compared one of another, the correct answer about these molecules is ....
a. BF3 is polar
b. NH3 is non polar
c. NH3 has lone pair electron
d. BF3 doesn’t have lone pair electron
e. the hybridization state of NH3 is sp2

5. If you compare the molecules of methane, ammonia, and water, the wrong answer about those molecules is ....
a. each molecule has certain shape
b. the geometry of methane is tetrahedral
c. the hybridization state of H2O is sp3
d. all molecules have the same geometry
e. the molecule shape of ammonia is pyramid

6. One of the following chemical bonds is very weak and is independent of the type of element involved. This chemical bond is ….
a. ionic
b. covalent
c. hydrogen
d. dipole-dipole
e. Van der Waals

7. Which phase change is exothermic? 1. H2O(s) -->H2O(l) 2. H2O(l) -->H2O(s) 3. H2O(s) -->H2O(g) 4. H2O(l) -->H2O(g)

a. 1
b. 2
c. 1 and 2
d. 1 and 3
e. 3 and 4

8. Given the following equations and delta H values, determine the heat of reaction (kJ) at 298 K for the reaction: N2(g) + O2(g) --> 2 NO(g)
4NH3(g)+5O2(g)-->6H2O(l)+4NO(g) H/kJ = -613 4NH3(g) + 3O2(g)-->2N2(g)+6H2O(l) H/kJ = -790
a. +177
b. +89
c. -89
d. -177
e. -1403

9. Which of the following equations represents a reaction that provides the heat of formation of hydrogen peroxide (H2O2)?
a. 2 H2O(l) --> H2O2(l) + H2(g)
b. H2(g) + O2(g) -->H2O2(l)
c. 2 H(g) + 2 O(g) --> H2O2(l)
d. H2O(l) + 1/2 O2(g) --> H2O2(l)
e. 2 H(g) + O2(g) -->H2O2(l)

10. The heats of formation of CO2(g) and H2O(l) are -394 kJ/mole and -285.8 kJ/mole respectively. Using the data for the following combustion
reaction,calculate the heat of formation ofC4H10(g) 2 C4H10(g) + 13 O2(g) --> 8 CO2(g) + 10 H2O(l) H=-5756.1 kJ
a. -149
b. -138
c. -127
d. -115
e. -106

11. A catalyst alters the rate of a chemical
reaction by ....
a. stability the reaction
b. always providing a surface
on which molecules react
c. changing the products formed in the reaction
d. inducing an alternate pathway for the reaction with generally lower
activation energy
e. changing the frequency of collisions between molecules

12. Which of the following is the rate law (differential) of the reaction aA --> B, if reactant A is second order?
a. Rate = k
b. Rate = k[A]
c. Rate = [A]
d. Rate = k[A]2
e. Rate = [A]2

13. If the concentration of a reactant is doubled and the rate of the reaction quadruples, with all other factors which would affect the rate of the reaction
held constant, the order of the reactant is ....
a. zero
b. first
c. second
d. third
e. forth

14. The following rate data were obtained at 25oC for the indicated reaction. What is the rate-law expression for the reaction: 2 A + B --> 4 C?
[A] mol/L [B] mol/L v of C (M/min)
0.10 0.10 2.0 x 10-4
0.20 0.10 8.0 x 10-4
0.40 0.20 2.6 x 10-2

a. rate = k[A]2 [B]2
b. rate = k[A] [B]
c. rate = k[A]2[B]3
d. rate = k[A] [B]2
e. rate = k[A]2[B]

15. What is the rate law
for a reaction mechanism which consists of the following steps : (1) A + B --> C + D (slow) (2) A + C --> E (fast) (3) E + F --> G (fast)
a. Rate = k[A][C]
b. Rate = k[A][B]
c. Rate = k[B][C]
d. Rate = k[A][E]
e. Rate = k[E][F]

16. The collision theory of reaction rates:
I. helps to expose how temperature affects the rate.
II. assumes that the rate depends on the frequency at which reactants collide.
III. assumes that reactants must be in correct orientation to react.
IV. assumes that only collisions with energy above the activation energy are successful.
a. I, II, and III are correct. IV is incorrect.
b. I, III, and IV are correct. II is incorrect.
c. II, III, and IV are correct, I is incorrect.
d. II and IV are correct, I is incorrect.
e. All are correct statements.

17. Identify the INCORRECT statement below regarding chemical equilibrium ….
a. All chemical reactions are, in principle, reversible.
b. Equilibrium is achieved when the forward reaction rate equals the reverse reaction rate.
c. Equilibrium is achieved when the concentration of species become constant.
d. Equilibrium is achieved when the reaction quotient Q equals the equilibrium constant.
e. Equilibrium is achieved when the reactant and product concentrations become equal.

18. Given the reaction: A2B(s) --> A+(aq) + B2-(aq) What is the equilibrium constant expression for the reaction?
a. 2[A+][B2-]
b. 2[A+] + [B2-]
c. [A+]2[B2-]
d. [A+] [B2-]2
e. [A+]2 + [B2-]
19. The reaction A(g) --> B(g) has a K value of 3.2 x 102. At equilibrium, which of the following would be true?
a. [A] = [B] b. [A] < [B] c. [A] > [B] d. [A] > 0 e. [B] = 0

20. If the reaction :
2A(g) + B(g) --> 3C(g) was changed to 3C(g) --> 2A(g) + B(g) at the same conditions, what would the value of KP be? Kc=X
a. X
b. X2
c. 2X
d. 1/X
e. square root of X
21. What will happen to the value of the equilibrium constant for the following reaction if Cl2 is added after equilibrium is established?
4HCl(g)+O2(g) --> 2H2O(g)+Cl2(g) + heat
a. it will decrease b. no change will occur c. it will increase
d. it will decrease 2 x
e. it will increase 2 x
22. Given the reaction at equilibrium:
2 SO2(g) + O2(g) --> 2SO3(g) + heat
The concentration of SO3(g) may be increased by ....
a. decreasing [SO2]
b. decreasing [O2]
c. adding catalyst
d. increasing the pressure
e. increasing the temperature
23. Consider the following equilibrium: 2O2(g) + N2(g) ⇄ N2O4(g)
When 2.0 mol of O2 and 3.0 mol of N2 were placed in a 10.0 L container at 25oC, the value of Kc=0.90. If the same number of moles of reactant were placed in a 5.0 L container at 25oC, the equilibrium constant would be ….
a. 0.011
b. 0.45
c. 0.90
d. 1.20
e. 1.80
24. One mole of gaseous AB is placed in a one liter container. At equilibrium it is 50% dissociated according to the equation shown here: 2AB --> 2A + B2. The equilibrium constant is ….
a. 0.0125
b. 0.025
c. 0.04
d. 0.125
e. 0.25
25. The equilibrium constant Kc for the following reaction at 800oC is 7.14 x 10-2. What is Kp at this temperature? (R = 0.082 L atm/mol K)
2 CO(g) --> C(s) + CO2(g)
a. 5.92 x 102 b. 9.22 x 10-6 c. 7.14 x 10-2 d. 6.29 e. 8.10 x 10-4

Ikatan Ion

• Ikatan yang terjadi antara ion positif dan ion negatif karena gaya elektrostatis
• Ion positif terjadi karena melepaskan elektron
• Ion negatif terjadi karena mengikat elektron
• Ion positif berasal dari unsur logam terutama dari Gol IA dan IIA
• Ion negatif berasal dari unsur non logam terutama Gol VI A dan VIIA
• Terjadi antara unsur logam dan non logam
Contoh 1 :
Ikatan antara Na dengan Cl
Konfigurasi elektronnya



Atom Na melepaskan 1 elektron valensinya sehingga konfigurasi elektronnya sama dengan gas mulia.



Atom Cl menerima 1 elektron pada kulit terluarnya sehingga konfigurasi elektronnya sama dengan gas mulia


Contoh 2.
Ikatan antara 11Na dan 8O


melepas 1 elektron


mengikat 2 elektron



Contoh 3:
12Mg dengan 8O


melepas 2 elekron

mengikat 2 elektron



Sifat umum senyawa ionik :

• Titik didih dan titik lelehnya tinggi
• Keras, tetapi mudah patah
• Penghantar panas yang baik
• Lelehan maupun larutannya dapat menghantarkan listrik (elektrolit)
• Larut dalam air
• Tidak larut dalam pelarut/senyawa organik (misal : alkohol, eter, benzena)

Animasi ikatan ion
Tags:

Ikatan Kimia
Ikatan Ion
Ikatan Kovalen
Ikatan Kovalen Koordinasi
Polarisasi Ikatan Kovalen
Animasi flash Proses Pembentukan Ikatan Kovalen
Pengecualian dan Kegagalan Aturan Oktet