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Topic 8 Acids and Bases

Total questions: 67

Worksheet time: 4hrs 20mins

Name
Class
Date
1.

What is the difference between a conjugate Brønsted–Lowry acid–base pair?

a)

Electron pair

b)

Positive charge

c)

Proton

d)

Hydrogen atom

2.

Which is an example of an amphiprotic species?

a)

Al2O3

b)

CO32−

c)

P4O10

d)

HPO42−

3.

Which two species act as Brønsted–Lowry acids in the reaction?


H2PO4− (aq) + OH− (aq) ⇌

HPO42− (aq) + H2O (l)

a)

HPO42− (aq) and OH− (aq)

b)

H2PO4− (aq) and HPO42− (aq)

c)

HPO42− (aq) and H2O (l)

d)

H2PO4− (aq) and H2O (l)

4.

Which classification is correct for the reaction?

H2PO4−(aq) + H2O(l) → HPO42−(aq) + H3O+(aq)

a)

A

b)

B

c)

C

d)

D

5.

What describes HPO42−?

a)

Amphiprotic but not amphoteric

b)

Amphoteric but not amphiprotic

c)

Amphiprotic and amphoteric

d)

Neither amphiprotic nor amphoteric

6.

Which is an acid-base conjugate pair?

a)

H3O+ / OH–

b)

H2SO4 / SO42–

c)

CH3COOH / H3O+

d)

CH3NH3+ / CH3NH2

7.

Which of the following is correct?

a)

A weak acid is a proton donor and its aqueous solution shows good conductivity.

b)

A weak acid is a proton donor and its aqueous solution shows poor conductivity.

c)

A weak acid is a proton acceptor and its aqueous solution shows good conductivity.

d)

A weak acid is a proton acceptor and its aqueous solution shows poor conductivity.

8.

Which species produced by the successive dissociations of phosphoric acid, H3PO4, are amphiprotic?

a)

HPO42− and PO43−

b)

H2PO4− and HPO42−

c)

H2PO4− and PO43−

d)

HPO42− only

9.

Which species acts as a Lewis and Brønsted–Lowry base?

a)

[Al(H2O)6]3+

b)

BF3

c)

NH4+

d)

OH−

10.

Which species behave as Brønsted–Lowry bases in the following reaction?


H2SO4 + HNO3 H2NO3+ + HSO4-

a)

HNO3 and HSO4-

b)

HNO3 and H2NO3+

c)

H2SO4 and HSO4-

d)

H2NO3+ and HSO4-

11.

Which is a conjugate Brønsted–Lowry acid-base pair?

a)

CH3COO− / H3O+

b)

H2O / CH3COO−

c)

H2O / H3O+

d)

CH3COOH / H2O

12.

Which are acid-base pairs according to the Brønsted‒Lowry theory?


I. HNO3/NO−3

II. H3O+/OH−

III. HCOOH/HCOO−

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

13.

Which of the following is an example of a Lewis acid–base reaction, but not a Brønsted–Lowry acid–base reaction?

a)

2CrO2−4(aq) + 2H+(aq) →

Cr2O2−7(aq) + H2O(l)

b)

Co(H2O)2+6(aq) + 4HCl(aq) →

CoCl2−4(aq) + 4H+(aq) + 6H2O(l)

c)

NH3(aq) + H+(aq) →

NH+4(aq)

d)

CH3COO−(aq) + H2O(l) →

CH3COOH(aq) + OH−(aq)

14.

Which row correctly describes

1.0 moldm−3 NaOH(aq)?

a)

A

b)

B

c)

C

d)

D

15.

What is the Brønsted–Lowry conjugate base of H2PO−4?

a)

H3PO4

b)

HPO2−4

c)

PO3−4

d)

HO−

16.

Which descriptions are correct for both a Brønsted–Lowry acid and a Lewis acid?

a)

A

b)

B

c)

C

d)

D

17.

Consider the equilibrium below.

CH3CH2COOH(aq) + H2O(l) ⇌ CH3CH2COO−(aq) + H3O+(aq)


Which species represent a conjugate acid-base pair?

a)

CH3CH2COOH and H2O

b)

H2O and CH3CH2COO−

c)

H3O+ and H2O

d)

CH3CH2COO− and H3O+

18.

Which is not a conjugate acid-base pair?

a)

HNO3 and NO3-

b)

CH3COOH and CH3COO−

c)

H3O+ and OH−

d)

HSO4- and SO42−

19.

What is the conjugate base of H2CO3 according to the Brønsted-Lowry theory?

a)

CO32−

b)

HCO3−

c)

H3CO3+

d)

CO2

20.

Which species behave as Brønsted-Lowry acids in the following reversible reaction?


H2PO4−(aq) + CN−(aq) ⇌ HCN(aq) + HPO42−(aq)

a)

HCN and CN−

b)

HCN and HPO42−

c)

H2PO4− and

d)

HCN and H2PO4−

21.

What is the formula of the conjugate base of the hydrogenphosphate ion, HPO42−?

a)

H2PO4−

b)

H3PO4

c)

HPO4−

d)

PO43−

22.

Which are definitions of an acid according to the Brønsted-Lowry and Lewis theories?

a)

A

b)

B

c)

C

d)

D

23.

According to the Brønsted-Lowry theory, how does each species act in the equilibrium below?

CH3COOH + H2SO4 ⇌ CH3COOH2+ + HSO4−

a)

A

b)

B

c)

C

d)

D

24.

With which do most acids react?

I. sodium hydrogen carbonate

II. magnesium

III. calcium sulfate

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

25.

What are the products of the reaction between sulfuric acid and sodium hydrogen carbonate?

a)

NaSO4 + H2O + CO2

b)

Na2SO4 + CO2

c)

Na2SO4 + H2O + CO2

d)

NaSO4 + H2CO3

26.

Which react with dilute sulfuric acid?

I. Cu

II. CuO

III. CuCO3

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

27.

What occurs when solid sodium hydrogen carbonate reacts with aqueous sulfuric acid?

a)

Bubbles of sulfur dioxide form.

b)

Bubbles of both hydrogen and carbon dioxide form.

c)

Bubbles of hydrogen form.

d)

Bubbles of carbon dioxide form.

28.

A student carried out a titration to determine the concentration of an acid and found that his value had good precision but poor accuracy. Which process explains this outcome?

a)

Consistently overshooting the volume of solution from the burette into the flask.

b)

Collection of insufficient titration data.

c)

Reading the meniscus in the burette at a different angle each time.

d)

Forgetting to rinse the flask after one of the titrations.

29.

Which gas in the atmosphere causes the pH of unpolluted rain to be approximately 6?

a)

Carbon dioxide

b)

Sulfur dioxide

c)

Oxygen

d)

Nitrogen

30.

Which compound reacts with calcium oxide, CaO?

a)

K2O

b)

Na2O

c)

SO2

d)

MgO

31.

Which solutions have a pH less than 7?

I. Na2CO3 (aq)

II. [Fe(H2O)6]Cl3 (aq)

III. (NH4)2SO4 (aq)

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

32.

If 20 cm3 samples of 0.1 moldm−3 solutions of the acids below are taken, which acid would require a different volume of 0.1 moldm−3 sodium hydroxide for complete neutralization?

a)

Nitric acid

b)

Sulfuric acid

c)

Ethanoic acid

d)

Hydrochloric acid

33.

Which solution is basic at 25 °C?

Kw = 1.0 × 10−14

a)

[H+] = 1.0 × 10−3 mol dm−3

b)

[OH−] = 1.0 × 10−13 mol dm−3

c)

solution of pH = 4.00

d)

[H3O+] = 1.0 × 10−13 mol dm−3

34.

What is the pH of 0.001 mol dm−3 NaOH (aq)?

a)

1

b)

3

c)

11

d)

13

35.

What is the pH of a solution in which the hydroxide ion concentration is 1 × 10−11 mol dm−3 at 298 K?

Kw = 1 × 10−14 at 298 K

a)

3

b)

7

c)

11

d)

14

36.

What will happen if the pressure is increased in the following reaction mixture at equilibrium?

CO2 (g) + H2O (l) ⇌ H+ (aq) + HCO3− (aq)

a)

The equilibrium will shift to the right and pH will decrease.

b)

The equilibrium will shift to the right and pH will increase.

c)

The equilibrium will shift to the left and pH will increase.

d)

The equilibrium will shift to the left and pH will decrease.

37.

10.0 cm3 of an aqueous solution of sodium hydroxide of pH = 10 is mixed with 990.0 cm3 of distilled water. What is the pH of the resulting solution?

a)

8

b)

9

c)

11

d)

12

38.

Which statement is incorrect for a 0.10 mol dm–3 HCOOH solution?

a)

pH = 1

b)

[H+] << 0.10 mol dm–3

c)

[HCOO–] is approximately equal to [H+]

d)

HCOOH is partially ionized

39.

What is the pH of 1.0 × 10−3 mol dm−3 sodium hydroxide, NaOH(aq)?

Kw = 1.0 × 10−14

a)

3

b)

4

c)

10

d)

11

40.

10.0 cm3 of a solution of a strong acid with a pH of 3 is added to a volumetric flask and the total volume is made up to 1.00 dm3 by adding distilled water. The resulting solution is then thoroughly mixed.

What is the pH of the diluted solution?

a)

1

b)

2

c)

4

d)

5

41.

A solution of 50 cm3 hydrochloric acid has a pH of 4. What is the final pH if 450 cm3 of water is added?

a)

3

b)

4

c)

5

d)

6

42.

A solution of acid HX has a pH = 1 and a solution of acid HY has a pH = 3. Which statement must be correct?

a)

HX is a stronger acid than HY.

b)

HY is a stronger acid than HX.

c)

The [H+] in the solution of HY is 100 times greater than the [H+] in the solution of HX.

d)

The [H+] in the solution of HY is 100 times greater than the [H+] in the solution of HX.

43.

What is the pH of the solution formed when 10 cm3 of HCl (aq) with pH 1.0 is added to 990 cm3

of water?

a)

1.5

b)

2.0

c)

2.5

d)

3.0

44.

The pH of a solution changes from pH=2 to pH=5. What happens to the concentration of the hydrogen ions during this pH change?

a)

It decreases by a factor of 1000

b)

It increases by a factor of 1000

c)

It decreases by a factor of 100

d)

It increases by a factor of 100

45.

An example of a strong acid solution is perchloric acid, HClO4, in water. Which statement is correct for this solution?

a)

HClO4 is completely dissociated in the solution.

b)

HClO4 exists mainly as molecules in the solution.

c)

The solution reacts only with strong bases.

d)

The solution has a pH value greater than 7.

46.

What is the correct expression for the ionic product constant of water, Kw?

a)

Kw=[H+][OH−]K_w=\frac{\left[H^+\right]}{\left[OH^-\right]}

b)

Kw=[H2O][H+][OH−]K_w=\frac{\left[H_2O\right]}{\left[H^+\right]\left[OH^-\right]}

c)

Kw=[H+]+[OH−]K_w=\left[H^+\right]+\left[OH^-\right]

d)

Kw=[H+][OH−]K_w=\left[H^+\right]\left[OH^-\right]

47.

What is the order of increasing pH for the following solutions of the same concentration?

a)

HCl (aq) < NH3 (aq) < NaOH (aq) < CH3COOH (aq)

b)

CH3COOH (aq) < HCl (aq) < NH3 (aq) < NaOH (aq)

c)

HCl (aq) < CH3COOH (aq) < NH3 (aq) < NaOH (aq)

d)

NaOH (aq) < NH3 (aq) < CH3COOH (aq) < HCl (aq)

48.

Which statement is correct?

a)

A strong acid is a good proton donor and has a strong conjugate base.

b)

A weak acid is a poor proton acceptor and has a strong conjugate base.

c)

A strong acid is a good proton donor and has a weak conjugate base.

d)

A strong base is a good proton donor and has a weak conjugate acid.

49.

Which 1.0 moldm–3 solution has the highest pH?

a)

Ammonium chloride

b)

Sulfuric acid

c)

Sodium chloride

d)

Ammonia

50.

Which compound is a strong acid?

a)

NH3

b)

HNO3

c)

H2CO3

d)

CH3COOH

51.

A student adds 0.3 g of magnesium metal to equal volumes of hydrochloric acid and ethanoic acid of the same concentrations in separate flasks. Which statement is correct?

a)

Hydrochloric acid reacts more rapidly as it has a higher pH than ethanoic acid.

b)

A greater total volume of H2 gas is produced with hydrochloric acid than with ethanoic acid.

c)

The same total volume of H2 gas is produced with both hydrochloric acid and ethanoic acid.

d)

Ethanoic acid reacts more slowly because it has a lower pH than hydrochloric acid.

52.

Which group of three compounds contains only weak acids and bases?

a)

A

b)

B

c)

C

d)

D

53.

Which list contains only strong bases?

a)

ammonia, sodium hydroxide, ethylamine

b)

potassium hydroxide, ammonia, sodium hydroxide

c)

lithium hydroxide, potassium hydroxide, barium hydroxide

d)

ammonia, ethylamine, barium hydroxide

54.

Which products would be formed when hydrochloric acid reacts with magnesium oxide?

a)

magnesium chloride and carbon dioxide

b)

magnesium chloride, hydrogen gas and water

c)

magnesium, hydrogen gas and water

d)

magnesium chloride and water

55.

Which group of three compounds contains only weak acids and bases?

a)

A

b)

B

c)

C

d)

D

56.

The table below shows data for the Ka and pKb values for some acids and bases at 298 K. Which two formulas represent the weakest acid and the weakest base in the table?

a)

HClO and C6H5NH2

b)

C6H5CH2COOH and NH3

c)

C6H5CH2COOH and C6H5NH2

d)

HClO and NH3

57.

Which salts will dissolve in water to give solutions with a pH above 7?

I. Na2CO3

II. CH3COONa

III. Na2SO4

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

58.

Which 0.10 moldm−3 solution would have the highest conductivity?

a)

HCl

b)

NH3

c)

CH3COOH

d)

H2CO

59.

A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?

a)

Acid A is stronger than acid B.

b)

[A] > [B].

c)

The concentration of H+ ions in A is higher than in B.

d)

The concentration of H+ ions in B is twice the concentration of H+ ions in A.

60.

Which of the following are weak acids in aqueous solution?

I. CH3COOH

II. H2CO3

III. HCl

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

61.

For equal volumes of 1.0 moldm−3 solutions of hydrochloric acid, HCl(aq), and methanoic acid, HCOOH(aq), which statements are correct?

I. HCl dissociates more than HCOOH

II. HCl is a better electrical conductor than HCOOH

III. HCl will neutralize more NaOH than HCOOH

a)

I and II only

b)

I and III only

c)

II and III only

d)

I, II and III

62.

When equal volumes of four 0.1 moldm−3 solutions are arranged in order of increasing pH (lowest pH first), what is the correct order?

a)

CH3COOH < HNO3 < CH3CH2NH2 < KOH

b)

HNO3 < CH3COOH < CH3CH2NH2 < KOH

c)

CH3CH2NH2 < HNO3 < CH3COOH < KOH

d)

KOH < CH3CH2NH2 < CH3COOH < HNO3

63.

Which list contains only strong acids?

a)

CH3COOH, H2CO3, H3PO4

b)

HCl, HNO3, H2CO3

c)

CH3COOH, HNO3, H2SO4

d)

HCl, HNO3, H2SO

64.

Which is not a source of oxides of sulfur and nitrogen?

a)

burning coal

b)

internal combustion engines

c)

burning methane

d)

volcanic eruptions

65.

What is the major reason why the pH of unpolluted rain is less than 7?

a)

methane

b)

carbon dioxide

c)

nitrogen oxides

d)

sulfur dioxide

66.

Which of the following gases does not result in acid deposition?

a)

CO2

b)

NO2

c)

NO

d)

SO2

67.

Which pH value is that of an aqueous solution of carbon dioxide?

a)

2.1

b)

5.6

c)

9.8

d)

12.2

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