general chemistry ebbing gammon ch. 15

Chapter 15 - Acids and Bases

1.Which of the following reactions is not readily explained by the Arrhenius concept of acids and bases?

A)

HCl(g) + NH3(g) NH4Cl(s)

B)

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

C)

HClO4(aq) + H2O(l) H3O+(aq) + ClO4-(aq)

D)

HC2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2-(aq)

E)

H3O+(aq) + OH-(aq) 2H2O(l)

ANS:APTS:1DIF:easyREF:15.1

OBJ:Define acid and base according to the Arrhenius concept.

TOP:acidsandbases | acid-baseconceptsNOT:REVISED

2.Which of the following statements is/are consistent with the Arrhenius concept of acids and bases?

1.

An Arrhenius acid will increase the concentration of hydronium ion in an aqueous or nonaqueous solvent.

2.

All Arrhenius acids are strong electrolytes in water.

3.

All strong acid-strong base reactions have the same heat of reaction (DH) per mole of water formed.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 3

E)

1, 2 and 3

ANS:CPTS:1DIF:easyREF:15.1


TOP:acidsandbases | acid-baseconcepts

3.Which of the following statements does not describe a characteristic of an Arrhenius acid?

A)

An Arrhenius acid reacts with an Arrhenius base to produce a salt.

B)

An Arrhenius acid turns red litmus blue.

C)

An Arrhenius acid is an electrolyte.

D)

An Arrhenius acid reacts with CaCO3 to produce CO2.

E)

An Arrhenius acid tastes sour.

ANS:BPTS:1DIF:easyREF:15.1



KEY:ArrheniusconceptofacidsandbasesMSC:general chemistry

4.Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)

Br

B)

HF

C)

H2SO3

D)

H3O+

E)

HNO3




5.Which of the following species is not capable of acting as an Arrhenius acid in aqueous solution?

A)

CHCl3

B)

HNO3

C)

H2SO4

D)

H3O+

E)

HClO4




6.Which of the following statements is correct concerning the neutralization of sulfurous acid by a strong base?

2OH(aq) + H2SO3(aq) SO32(aq) + 2H2O(l)

A)

H2SO3 is both an Arrhenius acid and a BrnstedLowry acid.

B)

H2SO3 is a BrnstedLowry acid, but not an Arrhenius acid.

C)

H2SO3 is neither an Arrhenius acid nor a BrnstedLowry acid.

D)

H2SO3 is an Arrhenius acid, but not a BrnstedLowry acid.

E)

H2SO3 is a Lewis base.


OBJ:Define acid and base according to the BrnstedLowry concept.


KEY:Brnsted-Lowry concept of acids and basesMSC:general chemistry

7.Which of the following statements is/are consistent with the Brnsted-Lowry concept of acids and bases?

1.

A conjugate acid-base pair may differ by only one proton.

2.

A base is defined as a hydroxide ion donor.

3.

Brnsted-Lowry acid-base reactions are restricted to aqueous solutions.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 2

E)

1, 2, and 3


OBJ:Define acid and base according to the BrnstedLowry concept.


8.Which are the BrnstedLowry bases in the following equilibrium?

CH3COO(aq) + H2O(l) CH3COOH(aq) + OH(aq)

A)

CH3COO and OH

B)

H2O and OH

C)

H2O, CH3COOH, and OH

D)

CH3COO and CH3COOH

E)

H2O and CH3COOH


OBJ:Identify acid and base species. (Example 15.1)



9.Which of the following pairs of species is not a conjugate acidbase pair?

A)

HOCl, OCl

B)

HNO2, NO2+

C)

O2, OH

D)

HSO4, SO42

E)

H2CO3, HCO3





10.What is a conjugate acidbase pair for the following equilibrium?

H2O(l) + HPO42(aq) H2PO4(aq) + OH(aq)

A)

H2O is an acid and HPO42 is its conjugate base.

B)

HPO42 is an acid and OH is its conjugate base.

C)

H2O is an acid and OH is its conjugate base.

D)

HPO42 is an acid and H2PO4 is its conjugate base.

E)

HPO42 is an acid and H2O is its conjugate base.

ANS:CPTS:1DIF:moderateREF:15.2




11.What is the conjugate base of H2PO4(aq)?

A)

PO43

B)

H3O+

C)

HPO42-

D)

H3P

E)

H3PO4




12.What is a conjugate acidbase pair for the following equilibrium?

H2O(l) + NH4+(aq) NH3(aq) + H3O+(aq)

A)

H2O is an acid and NH3 is its conjugate base.

B)

H2O is an acid and H3O+ is its conjugate base.

C)

NH4+ is an acid and NH3 is its conjugate base.

D)

H2O is a base and NH3 is its conjugate acid.

E)

H2O is a base and NH4+ is its conjugate acid.





13.Which of the following species is amphiprotic in aqueous solution?

A)

CH3NH2

B)

H3O+

C)

NH4+

D)

F-

E)

H2O

ANS:EPTS:1DIF:moderateREF:15.2

OBJ:Define amphiprotic species.TOP:acidsandbases | acid-baseconcepts

14.Which of the following species cannot act as a Lewis base?

A)

H2S

B)

S2

C)

Al3+

D)

SH

E)

H2O


OBJ:Identify Lewis acid and Lewis base species. (Example 15.2)


KEY:LewisconceptofacidsandbasesMSC:general chemistry


A)

H2O2

B)

OH

C)

O2

D)

H2O

E)

Be2+

ANS:EPTS:1DIF:easyREF:15.3





A)

NH3

B)

NH4+

C)

N3

D)

NH2

E)

NH2





17.Which of the following species cannot act as a Lewis acid?

A)

H+

B)

H

C)

K+

D)

Mg2+

E)

Al3+





18.In the reaction

CuO(s) + SO2(g) CuSO3(s),

A)

O2 acts as a Lewis base and SO2 acts as a Lewis acid.

B)

O2 acts as a Lewis base and Cu2+ acts as a Lewis acid.

C)

CuO is the Lewis acid and CuSO3 is its conjugate base.

D)

SO2 is the Lewis acid and CuSO3 is its conjugate base.

E)

Cu2+ acts as a Lewis acid and SO32 acts as a Lewis base.





19.Consider the following reaction:

AgBr(s) + 2CN(aq) Ag(CN)2(aq) + Br(aq)

The species that are acting as a Lewis acid and Lewis base, respectively, are

A)

Br and CN.

B)

Ag+ and CN.

C)

AgBr and Ag(CN)2.

D)

Ag(CN)2 and Ag+.

E)

Ag+ and Br.





20.Which of the following is not an example of an acidbase reaction?

A)

Al(OH)3(s) + 3H+(aq) Al3+(aq) + 3H2O(l)

B)

C2H6(g) C2H4(g) + H2(g)

C)

MgO(s) + CO2(g) MgCO3(s)

D)

Al(OH)3(s) + OH(aq) Al(OH)4(aq)

E)

CN(aq) + H2O(l) HCN(aq) + OH(aq)

ANS:BPTS:1DIF:moderateREF:15.3




21.Which of the following is/are an appropriate classification of the reaction given below?

KOH(aq) + CO2(g) KHCO3(aq)

1.

The above reaction may be classified as an Arrhenius acid-base reaction.

2.

The above reaction may be classified as a Brnsted-Lowry acid-base reaction.

3.

The above reaction may be classified as a Lewis acid-base reaction.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 3

E)

none




22.Which of the following species cannot act as a Lewis acid?

A)

BeCl2

B)

H+

C)

Ag+

D)

BF3

E)

NH4+





23.Which acid has the strongest conjugate base in aqueous solution?

A)

HF

B)

HNO3

C)

HClO4

D)

HI

E)

H2SO4


OBJ:Understand the relationship between the strength of an acid and that of its conjugate base.TOP:acidsandbases | acidandbasestrength

24.Which of the following concerning the relative strength of acids and bases is/are correct?

1.

As the acidity of the acid decreases, the basicity of the conjugate base increases.

2.

The hydronium ion is the strongest acid that can be found in aqueous solution.

3.

All acids classified as strong acids in aqueous solution have the same acidity in a more acidic solvent like acetic acid.

A)

1 only

B)

2 only

C)

3 only

D)

1 and 2

E)

1, 2, and 3

ANS:DPTS:1DIF:easyREF:15.4


25.Which of the following acids has the weakest conjugate base in aqueous solution?

A)

CH3COOH

B)

HOCl

C)

HF

D)

HNO2

E)

HClO4



26.Which of the following acids has the strongest conjugate base?

A)

HClO

B)

HClO4

C)

HClO2

D)

HClO3

E)

HCl



KEY:relativestrengthsofacidsandbasesMSC:general chemistry

27.The acid strength decreases in the series HBr > HSO4 > CH3COOH > HCN > HCO3. Which of the following is the strongest base?

A)

SO42

B)

CO32

C)

CH3COO

D)

Br

E)

CN




28.What is the leveling effect?

A)

All bases are 100% ionized in water.

B)

All acids are 100% ionized in solvents other than water.

C)

All strong acids are 100% ionized in water.

D)

An acid with a higher concentration in water has a lower pH than an acid with a lower concentration in water.

E)

A base with a higher concentration in water has a lower pH than a base with a lower concentration in water.




29.Which of the following reactions is not product-favored?

A)

NaOH(aq) Na+(aq) + OH(aq)

B)

NH3(aq) + H2O(l) NH4+(aq) + OH(aq)

C)

HClO4(aq) + H2O(l) H3O+(aq) + ClO4(aq)

D)

HCl(aq) + H2O(l) H3O+(aq) + Cl(aq)

E)

H2SO4(aq) + H2O(l) H3O+(aq) + HSO4(aq)


OBJ:Decide whether reactants or products are favored in an acidbase reaction. (Example 15.3)TOP:acidsandbases | acidandbasestrength


30.Given equal concentrations of the following acids, which exhibits the greatest amount of ionization in water?

A)

nitrous acid

B)

chlorous acid

C)

ascorbic acid

D)

hydrobromic acid

E)

citric acid



31.Which of the following statements is true concerning an aqueous solution of the weak base NH3?

A)

OH is a stronger base than NH3.

B)

OH is a stronger acid than NH4+.

C)

NH4+ is a stronger acid than H3O+.

D)

NH3 is a weaker base than H2O.

E)

H2O is a stronger acid than H3O+.




32.Which of the following statements is true concerning an aqueous solution of the strong acid HBr?

A)

Br is a stronger acid than H2O.

B)

Br is a stronger base than OH.

C)

H3O+ is a stronger acid than HBr.

D)

H2O is a stronger acid than HBr.

E)

H2O is a stronger base than Br.




33.Rank the following in order of decreasing acid strength in aqueous solution: HCl, HOCl, HOBr, HOI.

A)

HCl > HClO > HBrO > HIO

B)

HIO > HBrO > HClO > HCl

C)

HCl > HIO > HBrO > HClO

D)

HClO > HCl > HBrO > HIO

E)

HClO > HBrO > HCl > HIO


OBJ:Understand the periodic trends in the strengths of the binary acids HX.

TOP:acidsandbases | acidandbasestrength

34.Which of the following statements is incorrect?

A)

One reason why HCl is a stronger acid than HF is that the HCl bond is weaker than the HF bond.

B)

F is a stronger base than Cl.

C)

One reason why HCl is a stronger acid than HF is that Cl is more electronegative than F.

D)

The acids HBr and HI both appear equally strong in water.

E)

One reason why HCl is a stronger acid than HF is that Cl has a larger atomic radius than F.




KEY:molecularstructureandacidstrength

MSC:general chemistry

35.Which solution has the highest pH?

A)

0.10 M HBr(aq)

B)

0.10 M HI(aq)

C)

0.10 M HF(aq)

D)

0.10 M HCl(aq)

E)

0.10 M HClO4(aq)






36.Which of the following is the strongest acid in aqueous solution?

A)

H3AsO4

B)

H3PO4

C)

H3PO3

D)

H3SbO4

E)

H3AsO3


OBJ:Understand the rules for determining the relative strengths of oxoacids.




37.Rank the following in order of decreasing acid strength: H2O, H2S, H2Se, H2Te

A)

H2Te > H2Se > H2S > H2O

B)

H2O > H2S > H2Se > H2Te

C)

H2Se > H2Te > H2S > H2O

D)

H2S > H2Te > H2Se > H2O

E)

H2Se > H2S > H2Te > H2O




38.Which of the following is the strongest acid?

A)

HClO2

B)

HCl

C)

HClO4

D)

HClO

E)

HClO3






39.Which of the following solutes, dissolved in 1.0 kg of water, would be expected to provide the fewest particles and to freeze at the highest temperature?

A)

0.10 mol HClO

B)

0.10 mol HClO3

C)

0.10 mol HClO2

D)

0.10 mol HClO4

E)

0.10 mol HCl

ANS:APTS:1DIF:difficultREF:15.5





40.Rank H3PO4, H2PO4, and HPO42 in order of increasing acid strength.

A)

HPO42 < H2PO4 < H3PO4

B)

H2PO4 < HPO42 < H3PO4

C)

H2PO4 < H3PO4 < HPO42

D)

HPO42 < H3PO4 < H2PO4

E)

H3PO4 < H2PO4 < HPO42


OBJ:Understand the relative acid strengths of a polyprotic acid and its anions.




41.The ionization constant of water at a temperature above 25C is 1.71014. What is the pH of pure water at this temperature?

2H2O(l) H3O+(aq) + OH(aq)

A)

7.88

B)

5.68

C)

6.88

D)

13.85

E)

7.00


OBJ:Define self-ionization (or autoionization).

TOP:acidsandbases | self-ionizationofwaterandpH

KEY:self-ionizationofwaterMSC:general chemistry

42.The autoionization of water, as represented by the equation below, is known to be endothermic. Which of the following correctly states what occurs as the temperature of water is raised?

H2O(l) + H2O(l) H3O+(aq) + OH(aq)

A)

The pH of the water decreases, and the water becomes more acidic.

B)

The pH of the water decreases, and the water remains neutral.

C)

The pH of the water increases, and the water remains neutral.

D)

The pH of the water does not change, and the water remains neutral.

E)

The pH of the water increases, and the water becomes more acidic.

ANS:BPTS:1DIF:difficultREF:15.6




43.The equilibrium constant for the autonionization of water (shown below) increases with increasing temperature, from 1.01 x10-14 at 25C to 5.31 x10-14 at 50C.

H2O(l) + H2O(l) H3O+(aq) + OH(aq)

Which of the following statements is consistent with this behaviour?

A)

The autoionization of water is an endothermic reaction.

B)

The autoionization of water is an exothermic reaction.

C)

The hydronium ion concentration at equilibrium increases with increasing temperature.

D)

The hydronium ion concentration at equilibrium decreases with increasing temperature.

E)

Both A and C.

ANS:EPTS:1DIF:difficultREF:15.6



44.What is the equilibrium concentration of amide ion (NH2) in liquid ammonia at 25C? ("am"=dissolvedinammonia)

2NH3(l) NH4+(am) + NH2(am); Kc = 1.8 1024 at 25C

A)

2.6 1012 M

B)

3.6 1024 M

C)

1.3 1012 M

D)

1.8 1024 M

E)

9.0 1025 M


OBJ:Define the ion-product constant for water.

TOP:acidsandbases | self-ionizationofwaterandpHMSC:general chemistry

45.What is the hydronium-ion concentration in a solution formed by combining 750mL of 0.10MNaOH with 250mL of 0.30MHCl?

NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)

A)

0.075 M

B)

1.7 1013 M

C)

1.0 107 M

D)

0.30 M

E)

0.10 M

ANS:CPTS:1DIF:difficultREF:15.6




46.At 20C, the ion-product constant of water, Kw, is

6.8810

15

. What is the pH of pure water at 20C?

A)

7.000

B)

6.501

C)

7.181

D)

7.081

E)

none of these

ANS:DPTS:1DIF:moderateREF:15.8



47.The concentration of H3O+ in a solution is 7104 M at 25C. What is its hydroxide-ion concentration?

A)

7 104 M

B)

1 1010 M

C)

2 1010 M

D)

3 1010 M

E)

1 1011 M


OBJ:Calculate the concentrations of H3O+ and OH in solutions of a strong acid or base. (Example 15.4)TOP:acidsandbases | solutionsofastrongacidorbase


48.At 25C a solution has a hydroxide-ion concentration of 4.94105 M. What is its hydronium-ion concentration?

A)

4.94 1019 M

B)

1.00 107 M

C)

1.00 1014 M

D)

4.94 105 M

E)

2.02 1010 M




49.What is the hydronium-ion concentration of a 0.0087MLiOH solution?

A)

1.1 1012 M

B)

8.7 103 M

C)

1.0 1014 M

D)

1.0 107 M

E)

8.7 1017 M




50.What is the hydronium-ion concentration of a 0.0038MBa(OH)2 solution?

A)

7.6 103 M

B)

3.8 103 M

C)

1.3 1012 M

D)

2.6 1012 M

E)

1.0 107 M




51.Which of the following expressions is not equivalent to pH?

A)

log [H+(aq)]

B)

C)

14.0 pOH

D)

E)

log Kw


OBJ:Define pH.TOP:acidsandbases | solutionsofastrongacidorbase

KEY:pHofasolutionMSC:general chemistry

52.A solution in which the pH is 1.5 would be described as

A)

neutral.

B)

very acidic.

C)

slightly basic.

D)

slightly acidic.

E)

very basic.


OBJ:Define pH.TOP:acidsandbases | solutionsofastrongacidorbase

KEY:pHofasolutionMSC:general chemistry

53.A solution has a hydroxide-ion concentration of 0.0030M. What is the pOH of the solution?

A)

11.48

B)

2.52

C)

7.00

D)

8.19

E)

5.81


OBJ:Calculate the pH from the hydronium-ion concentration. (Example 15.5)

TOP:acidsandbases | solutionsofastrongacidorbaseKEY:pHofasolution


54.What is the pH of a 0.051 M HClO4 solution?

A)

15.29

B)

2.98

C)

12.71

D)

1.29

E)

11.02





55.What is the pOH of a 0.044 M HI solution?

A)

3.12

B)

12.64

C)

10.88

D)

15.36

E)

1.36





56.What is the pH of the final solution when 25 mL of 0.025 M HCl has been added to 35mL of 0.040MHCl at 25C?

A)

3.22

B)

1.78

C)

1.47

D)

2.69

E)

3.39





57.What is the pH of a 0.0042 M hydrochloric acid solution?

A)

5.47

B)

11.62

C)

7.00

D)

8.53

E)

2.38





58.The hydronium-ion concentration of a solution is 2.5106 M. What is the pH of the solution?

A)

6.81

B)

3.77

C)

2.00

D)

5.60

E)

10.60





59.At 25C, what is the pH of a 10.0 M HBr solution?

A)

1.000

B)

0.000

C)

10.000

D)

1.000

E)

14.000





60.Which aqueous solution has the lowest pH?

A)

0.30 M HCl

B)

0.30 M NaOH

C)

0.30 M NH3

D)

0.30 M Ba(OH)2

E)

0.30 M H2SO4



TOP:acidsandbases | solutionsofaweakacidorbase

61.What pH should a solution have if its pH is about the same as that of vinegar?

A)

about 8

B)

about 11

C)

about 1

D)

about 6

E)

about 3



TOP:acidsandbases | solutionsofaweakacidorbaseMSC:general chemistry

62.A solution has a pH value of 3.76. What is the pOH for this solution?

A)

7.00

B)

3.72

C)

3.76

D)

1.74

E)

10.24





63.Which solution has the highest pH?

A)

0.1 M Ba(OH)2

B)

0.1 M CH3COOH

C)

0.1 M HCl

D)

0.1 M NH3

E)

0.1 M NaOH

ANS:APTS:1DIF:moderateREF:15.8




64.The pOH of a solution is 5.22. What is the pH of the solution?

A)

5.22

B)

8.78

C)

6.03

D)

7.00

E)

2.68





65.What is the pH of a 0.0035 M Ba(OH)2 solution?

A)

9.04

B)

11.54

C)

2.46

D)

11.85

E)

2.15





66.What is the pOH of a 0.0055 M Ba(OH)2 solution?

A)

9.49

B)

11.74

C)

12.04

D)

1.96

E)

2.26





67.A solution has a hydronium-ion concentration of 0.0082 M. What is its pOH?

A)

2.09

B)

16.09

C)

9.20

D)

4.80

E)

11.91





68.A solution has a hydroxide-ion concentration of 0.043 M. What is its pH?

A)

15.37

B)

12.63

C)

17.15

D)

7.00

E)

1.37





69.What is the pOH of a 0.065 M HNO3 solution?

A)

12.81

B)

11.27

C)

15.19

D)

1.19

E)

2.73

ANS:APTS:1DIF:moderateREF:15.8




70.What is the pH of a 0.0086 M LiOH solution?

A)

9.24

B)

11.93

C)

2.07

D)

4.76

E)

16.07





71.What is the pOH of a 0.0092 M CsOH solution?

A)

2.04

B)

16.04

C)

9.31

D)

4.69

E)

11.96





72.What is the pH of a solution prepared by dissolving 0.739 g of NaOH(s) in 4.50L of water?

A)

1.733

B)

12.267

C)

7.000

D)

11.613

E)

2.387





73.What is the pOH of a solution prepared by dissolving 0.287 g of KOH(s) in 7.00L of water?

A)

10.864

B)

3.136

C)

2.291

D)

11.709

E)

7.000





74.What is the pH of a solution prepared by dissolving 0.365 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 6.00L? (R=0.0821Latm/(Kmol))

A)

2.566

B)

11.434

C)

1.788

D)

7.000

E)

12.212

ANS:APTS:1DIF:difficultREF:15.8




75.What is the pOH of a solution prepared by dissolving 0.465 L of HCl(g), measured at STP, in enough water such that the total volume of the solution is 4.50 L? (R=0.0821Latm/(Kmol))

A)

12.317

B)

7.000

C)

1.683

D)

11.664

E)

2.336

ANS:DPTS:1DIF:difficultREF:15.8




76.Which of the following solutions has the highest hydroxide-ion concentration?

A)

0.1 M HCl

B)

a solution with pH = 5

C)

0.1 M H2SO4

D)

pure water

E)

a solution with pOH = 12


OBJ:Calculate the hydronium-ion concentration from the pH. (Example 15.6)

TOP:acidsandbases | solutionsofastrongacidorbase

77.A solution has a pH of 10.20 at 25C. What is the hydroxide-ion concentration at 25C?

A)

3.8 M

B)

2.2 102 M

C)

1.6 104 M

D)

6.3 1011 M

E)

1.0 107 M





78.A solution has a pOH of 5.36. What is its hydroxide-ion concentration?

A)

1.8 104 M

B)

5.4 M

C)

2.3 109 M

D)

4.4 106 M

E)

4.7 103 M





79.The pOH of a solution is 5.06. What is its hydronium-ion concentration?

A)

1.1 105 M

B)

1.1 109 M

C)

8.7 106 M

D)

5.06 M

E)

6.3 103 M





80.The pH of a solution of a strong base is 10.27 at 25C. What is its hydronium-ion concentration?

A)

2.9 103 M

B)

1.9 104 M

C)

1.4 104 M

D)

5.4 1011 M

E)

1.4 102 M





81.What is the hydroxide-ion concentration in a solution formed by combining 200.mL of 0.15MHCl with 300.mL of 0.090MNaOH at 25C?

HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

A)

1.7 1013 M

B)

0.090 M

C)

1.7 1012 M

D)

0.054 M

E)

1.0 107 M





82.Which solution would cause blue litmus to turn red?

A)

a solution of pH 10

B)

a solution of 0.01 M NH3

C)

a solution of pOH 4

D)

a solution of 0.005 M CH3COOH

E)

a solution of 0.10 M NaOH


OBJ:Describe the determination of pH by a pH meter and by acidbase indicators.



general chemistry ebbing gammon ch. 15

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