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Revision Final Grade 11 SABIS T1 Quiz on Acids, Bases, and Salts

Total questions: 152

Worksheet time: 1hrs 16mins

Name
Class
Date
1.

Which of the following is a strong electrolyte?

a)

CH₃COOH

b)

HCl

c)

H₂O

d)

NH₃

2.

What is the pH of a neutral solution at 25°C?

a)

0

b)

7

c)

14

d)

It depends on the temperature

3.

According to the Arrhenius definition, a base is a substance that:

a)

Donates protons.

b)

Accepts protons.

c)

Increases [OH⁻] in water.

d)

Increases [H⁺] in water.

4.

Which of the following weak electrolytes partially dissociates in aqueous solution?

a)

NaOH

b)

HCl

c)

CH₃COOH

d)

KBr

5.

What is the [H⁺] in a 0.010 M solution of HCl at 25°C?

a)

0.010 M

b)

1.00 × 10⁻⁷ M

c)

0.005 M

d)

0.020 M

6.

Which indicator turns colorless in a basic solution?

a)

Litmus

b)

Methyl orange

c)

Phenolphthalein

d)

Thymolphthalein

7.

In the reaction Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g), magnesium is:

a)

Oxidized

b)

Reduced

c)

Neither oxidized nor reduced

d)

Both oxidized and reduced

8.

What is the pH of a solution with [OH⁻] = 1.00 × 10⁻⁴ M at 25°C?

a)

4

b)

10

c)

7

d)

14

9.

Which oxide is amphoteric?

a)

MgO

b)

CO₂

c)

Al₂O₃

d)

SO₃

10.

What gas is produced when an acid reacts with a carbonate?

a)

Hydrogen

b)

Carbon dioxide

c)

Oxygen

d)

Chlorine

11.

Which of the following salts is insoluble in water?

a)

NaCl

b)

KNO₃

c)

PbSO₄

d)

NH₄NO₃

12.

What is the product when NaOH reacts with HCl?

a)

NaCl and H₂O

b)

NaCl and H₂

c)

Na₂O and HCl

d)

NaH and Cl₂

13.

Which reaction represents the dissociation of a weak acid in water?

a)

HCl → H⁺ + Cl⁻

b)

CH₃COOH ⇄ CH₃COO⁻ + H⁺

c)

NaOH → Na⁺ + OH⁻

d)

H₂O → H⁺ + OH⁻

14.

Which of the following is a characteristic property of bases?

a)

Taste sour

b)

React with metals to produce hydrogen gas

c)

Feel slippery

d)

Turn red litmus paper blue

15.

In the neutralization reaction between HCl and NaOH, what is the mole ratio of HCl to NaOH?

a)

1:2

b)

2:1

c)

1:1

d)

3:2

16.

What is the pH of pure water at 25°C?

a)

0

b)

5

c)

7

d)

14

17.

Which of the following statements is true about water being a weak electrolyte?

a)

It completely dissociates into H⁺ and OH⁻ ions.

b)

It does not conduct electricity.

c)

It partially dissociates into H⁺ and OH⁻ ions.

d)

It is a strong acid.

18.

Which salt is formed when a strong acid reacts with a weak base?

a)

Neutral salt

b)

Acidic salt

c)

Basic salt

d)

Insoluble salt

19.

Calculate the pH of a 0.010 M LiOH solution at 25°C. (Kw = 1.0 × 10⁻¹⁴)

a)

5

b)

12

c)

7

d)

14

20.

Which of the following best describes an electrolyte?

a)

A substance that does not conduct electricity in solution.

b)

A substance that conducts electricity when dissolved in water.

c)

A substance that only conducts electricity when molten.

d)

A substance that increases the conductivity of metals.

21.

What is formed when ammonia reacts with water?

a)

NH₄⁺ and OH⁻

b)

NH₃ and H⁺

c)

NH₂⁻ and H₂O

d)

NH₄OH

22.

Which of the following is a Bronsted-Lowry base?

a)

H⁺

b)

H₂O

c)

NH₄⁺

d)

CH₃COOH

23.

What is the equilibrium constant (Kw) of water at 25°C?

a)

1.0 × 10⁰

b)

1.0 × 10⁻⁷

c)

1.0 × 10⁻¹⁴

d)

1.0 × 10¹⁴

24.

Which of the following reactions represents the neutralization of sodium hydroxide with hydrochloric acid?

a)

NaOH + HCl → NaCl + H₂O

b)

NaOH + HCl → NaCl + H₂

c)

NaOH + HCl → Na + Cl + H₂O

d)

NaOH + HCl → NaCl + O₂

25.

What is the [OH⁻] in a solution with pH 5.00 at 25°C?

a)

1.00 × 10⁻⁵ M

b)

1.00 × 10⁻⁹ M

c)

1.00 × 10⁻¹⁴ M

d)

1.00 × 10⁻⁷ M

26.

Which of the following reagents can be added to HCl to prepare ZnCl₂?

a)

Zn

b)

ZnO

c)

ZnCO₃

d)

All of the above

27.

Which reagent can be added to H₂SO₄ to prepare CuSO₄?

a)

Cu

b)

CuO

c)

CuCO₃

d)

All of the above

28.

Which of the following reactions produces ammonia gas?

a)

Acid + base

b)

Ammonium salt + base

c)

Acid + metal carbonate

d)

All of the above

29.

Which reaction produces a pungent smelling gas that turns damp red litmus blue?

a)

CaO + H₂SO₄

b)

Ca(OH)₂ + H₂SO₄

c)

Ca + H₂SO₄

d)

All of the above

30.

Which of the following reactions produce gas(es)?

a)

Acid + metal carbonate

b)

Ammonium salt + base

c)

Acid + base

d)

Acid + metal

e)

Acid + metal sulfite

31.

The reaction of a strong acid with a strong base to produce salt and water is called:

a)

Combustion

b)

Precipitation

c)

Neutralization

d)

Redox

32.

Which of the following methods is used to prepare soluble salts by reacting an acid with an insoluble base?

a)

Titration method

b)

Excess method

c)

Precipitation method

d)

Crystallization method

33.

Which reagent must be added to insoluble magnesium oxide to form magnesium sulfate?

a)

HCl

b)

H₂SO₄

c)

NaOH

d)

NH₃

34.

Which of the following is an acidic oxide?

a)

MgO

b)

CO₂

c)

CaO

d)

Al₂O₃

35.

Which of the following is an acidic oxide?

a)

MgO

b)

CO₂

c)

CaO

d)

Al₂O₃

36.

What is the product when K₂O reacts with H₂O?

a)

KOH

b)

K₂CO₃

c)

KCl

d)

KHCO₃

37.

Which of the following salts is considered a neutral salt?

a)

NaCl

b)

Na₂CO₃

c)

NH₄NO₃

d)

KOH

38.

What is the product formed when an excess of NaOH reacts with NH₄NO₃?

a)

NaNO₃ and NH₄OH

b)

NaNH₂ and HNO₃

c)

NaNH₂ and NH₃

d)

NaNO₃ and NH₃

39.

During the preparation of magnesium nitrate crystals, why is excess magnesium oxide used?

a)

To ensure complete reaction with nitric acid

b)

To produce more crystals

c)

To prevent precipitation

d)

To lower the temperature

40.

What is the main purpose of using an indicator in a titration?

a)

To speed up the reaction

b)

To neutralize the solution

c)

To determine the endpoint visually

d)

To increase the acidity

41.

In the titration of HCl with NaOH, what indicates that the equivalence point has been reached when using phenolphthalein?

a)

The solution turns blue.

b)

The solution turns colorless.

c)

The solution turns pink.

d)

The solution starts to bubble.

42.

Which salt is prepared using the precipitation method?

a)

NaCl

b)

PbCl₂

c)

KNO₃

d)

NH₄OH

43.

What is the net ionic equation for the reaction between HCl and NaOH?

a)

H⁺ + Cl⁻ + Na⁺ + OH⁻ → Na⁺ + Cl⁻ + H₂O

b)

H⁺ + OH⁻ → H₂O

c)

Na⁺ + Cl⁻ → NaCl

d)

HCl + NaOH → NaCl + H₂O

44.

Which of the following is a method to prepare insoluble salts?

a)

Titration method

b)

Excess method

c)

Precipitation method

d)

Crystallization method

45.

What happens to the pH of a solution when a strong acid is added to it?

a)

It increases.

b)

It decreases.

c)

It remains the same.

d)

It first increases then decreases.

46.

When molten NaOH is electrolyzed, which ion is discharged at the cathode?

a)

Na⁺

b)

OH⁻

c)

H₂O

d)

O²⁻

47.

Which of the following salts is formed from a weak acid and a strong base?

a)

NaCl

b)

Na₂CO₃

c)

NH₄Cl

d)

KOH

48.

What type of salt is formed when H₂SO₄ reacts with NH₃?

a)

Neutral salt

b)

Acidic salt

c)

Basic salt

d)

Amphoteric salt

49.

Which of the following is true about the solubility of salts?

a)

All chlorides are insoluble.

b)

Sulfates are always soluble.

c)

Nitrates are generally soluble.

d)

Carbonates are always insoluble.

50.

What is the product when ammonium nitrate reacts with potassium hydroxide?

a)

Ammonia and potassium nitrate

b)

Ammonium hydroxide and potassium nitrate

c)

Ammonia and potassium hydroxide

d)

Ammonium hydroxide and potassium nitrate

51.

Which of the following is NOT a characteristic property of acids?

a)

Sour taste

b)

Slippery feel

c)

React with metals to produce hydrogen gas

d)

Turn blue litmus paper red

52.

In the reaction 2Cu + O₂ → 2CuO, which element is oxidized?

a)

Copper

b)

Oxygen

c)

Both Copper and Oxygen

d)

Neither

53.

What is the oxidizing agent in the reaction Zn + Cu²⁺ → Zn²⁺ + Cu?

a)

Zn

b)

Cu²⁺

c)

Zn²⁺

d)

Cu

54.

What is the oxidation number of Cr in Cr₂O₇²⁻?

a)

+6

b)

+3

c)

+2

d)

+7

55.

Which of the following is a reducing agent?

a)

H₂O₂

b)

KMnO₄

c)

Fe

d)

Cr₂O₇²⁻

56.

In the half-reaction Zn → Zn²⁺ + 2e⁻, what process is zinc undergoing?

a)

Reduction

b)

Oxidation

c)

Neither

d)

Both

57.

Which of the following best defines a redox reaction?

a)

A reaction involving acids and bases.

b)

A reaction involving precipitation.

c)

A reaction involving the transfer of electrons.

d)

A reaction involving gas formation.

58.

What is the product formed at the cathode during the electrolysis of molten lead bromide (PbBr₂)?

a)

Lead metal

b)

Bromine gas

c)

Lead(II) bromide

d)

Hydrogen gas

59.

During electrolysis, electrons flow from:

a)

Anode to Cathode

b)

Cathode to Anode

c)

Electrolyte to Anode

d)

Electrolyte to Cathode

60.

Which species is reduced in the reaction: Cu²⁺ + Zn → Cu + Zn²⁺?

a)

Cu²⁺

b)

Zn

c)

Both Cu²⁺ and Zn

d)

Neither

61.

What is the oxidizing agent in the reaction 2Fe³⁺ + Zn → 2Fe²⁺ + Zn²⁺?

a)

Fe³⁺

b)

Zn

c)

Fe²⁺

d)

Zn²⁺

62.

In an electrochemical cell, oxidation occurs at the:

a)

Cathode

b)

Anode

c)

Both electrodes

d)

Neither electrode

63.

What is the oxidation number of C in CH₃OH?

a)

+1

b)

-2

c)

0

d)

+2

64.

Which of the following is an example of a redox reaction?

a)

NaOH + HCl → NaCl + H₂O

b)

H₂SO₄ + Ba(OH)₂ → BaSO₄ + 2H₂O

c)

2Cu + O₂ → 2CuO

d)

AgNO₃ + NaCl → AgCl + NaNO₃

65.

In the reaction ZnO + C → Zn + CO, which element is reduced?

a)

Zinc

b)

Carbon

c)

Oxygen

d)

Both Zinc and Carbon

66.

What is the overall reaction in an electrolysis cell where water is decomposed?

a)

2H₂O(l) → 2H₂(g) + O₂(g)

b)

2H₂O(l) → 4H⁺(aq) + 2OH⁻(aq)

c)

H₂O(l) → H₂(g) + O₂(g)

d)

2H₂O(l) → 2H₂O₂(aq)

67.

What gas is produced at the anode during the electrolysis of concentrated aqueous NaCl?

a)

Hydrogen

b)

Chlorine

c)

Oxygen

d)

Sodium

68.

Which of the following half-reactions represents reduction?

a)

Zn → Zn²⁺ + 2e⁻

b)

Cu²⁺ + 2e⁻ → Cu

c)

O₂ + 4H⁺ + 4e⁻ → 2H₂O

d)

Both B and C

69.

During the electrolysis of dilute sulfuric acid, what gas is produced at the cathode?

a)

Oxygen

b)

Hydrogen

c)

Sulfur dioxide

d)

Chlorine

70.

What is the product at the cathode when molten NaOH is electrolyzed?

a)

Sodium metal

b)

Oxygen gas

c)

Hydrogen gas

d)

Water

71.

In the electroplating process, the object to be plated is connected to the:

a)

Positive terminal

b)

Negative terminal

c)

Anode

d)

Both A and C

72.

Which of the following best describes a reducing agent?

a)

A substance that gains electrons.

b)

A substance that loses electrons.

c)

A substance that is oxidized.

d)

Both B and C

73.

What is the product formed at the anode during the electrolysis of aqueous CuSO₄ using inert electrodes?

a)

Copper metal

b)

Oxygen gas

c)

Hydrogen gas

d)

Copper ions

74.

In a voltaic cell, electrons flow from:

a)

Cathode to Anode

b)

Anode to Cathode

c)

Electrolyte to Anode

d)

Electrolyte to Cathode

75.

Which metal has the highest tendency to lose electrons (be oxidized)?

a)

Silver

b)

Copper

c)

Zinc

d)

Gold

76.

What is produced at the cathode during the electrolysis of molten PbBr₂?

a)

Lead metal

b)

Bromine gas

c)

Lead(II) bromide

d)

Hydrogen gas

77.

Which of the following represents an oxidation half-reaction?

a)

MnO₄⁻ + 8H⁺ + 5e⁻ → Mn²⁺ + 4H₂O

b)

Fe²⁺ → Fe³⁺ + e⁻

c)

Cl₂ + 2e⁻ → 2Cl⁻

d)

Cu²⁺ + 2e⁻ → Cu

78.

During the electrolysis of CuSO₄ using copper electrodes, what happens to the mass of the anode?

a)

Increases

b)

Decreases

c)

Remains the same

d)

Fluctuates

79.

What gas is produced at the cathode during the electrolysis of concentrated aqueous NaCl?

a)

Chlorine

b)

Hydrogen

c)

Oxygen

d)

Sodium

80.

In the electrolysis of water, how many molecules of water are required to produce one molecule of oxygen gas?

a)

1

b)

2

c)

3

d)

4

81.

Which of the following species is an oxidizing agent?

a)

Zn

b)

H₂

c)

Cu²⁺

d)

Cl⁻

82.

What is the role of the electrolyte in an electrolytic cell?

a)

To conduct electricity by transferring electrons.

b)

To provide ions for the redox reactions.

c)

To serve as electrodes.

d)

Both A and B

83.

Which half-reaction represents the reduction of Cr₂O₇²⁻ to Cr³⁺?

a)

Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O

b)

Cr₂O₇²⁻ → 2Cr³⁺ + 7O²⁻

c)

Cr₂O₇²⁻ + 6e⁻ → 2Cr³⁺ + 7O₂

d)

Cr₂O₇²⁻ + 14H⁺ → 2Cr³⁺ + 7H₂O

84.

What is the product formed at the anode during the electrolysis of dilute sulfuric acid?

a)

Sulfur dioxide

b)

Oxygen gas

c)

Hydrogen gas

d)

Sulfuric acid remains unchanged

85.

In the reaction 8H₂O + Cr₂O₇²⁻ + 3CH₃OH → 3CH₂O + 2Cr³⁺ + 7H₂O + 8OH⁻, which species is oxidized?

a)

H₂O

b)

Cr₂O₇²⁻

c)

CH₃OH

d)

OH⁻

86.

Which of the following is NOT a property of reducing agents?

a)

They lose electrons.

b)

They are oxidized in reactions.

c)

They increase the oxidation state of other substances.

d)

They themselves get reduced.

87.

What is the main product when aqueous Cu²⁺ ions are reduced at the cathode during electrolysis?

a)

Copper(II) oxide

b)

Copper metal

c)

Copper(I) chloride

d)

Copper hydroxide

88.

In the electroplating process, what happens at the anode?

a)

Metal is deposited

b)

Metal ions are dissolved

c)

Oxygen gas is produced

d)

Hydrogen gas is produced

89.

Which of the following metals is least likely to be deposited at the cathode during electrolysis of an aqueous solution containing both Na⁺ and Ag⁺ ions?

a)

Sodium

b)

Silver

c)

Both are equally likely

d)

Neither is likely

90.

What is the role of an inert electrode in electrolysis?

a)

To participate in the reaction

b)

To act as a catalyst

c)

To conduct electricity without reacting

d)

To donate electrons

91.

During the electrolysis of molten PbBr₂, which species is reduced at the cathode?

a)

Pb²⁺

b)

Br⁻

c)

PbBr₂

d)

Pb

92.

What is produced at the cathode during the electrolysis of dilute CuSO₄ using inert electrodes?

a)

Copper metal

b)

Oxygen gas

c)

Hydrogen gas

d)

Sulfur dioxide

93.

Which of the following best describes an oxidizing agent?

a)

A substance that donates electrons

b)

A substance that accepts electrons

c)

A substance that is oxidized

d)

A substance that is a reducing agent

94.

In an electrolytic cell, which electrode is connected to the positive terminal of the power source?

a)

Cathode

b)

Anode

c)

Both

d)

Neither

95.

What gas is produced at the cathode during the electrolysis of dilute NaCl solution?

a)

Chlorine

b)

Hydrogen

c)

Oxygen

d)

Sodium

96.

What is produced at the cathode during the electrolysis of dilute NaCl solution?

a)

Chlorine

b)

Hydrogen

c)

Oxygen

d)

Sodium

97.

During the electrolysis of dilute CuSO₄, why does the solution's color fade?

a)

Cu²⁺ ions are being deposited as copper metal.

b)

Cu²⁺ ions are being oxidized.

c)

SO₄²⁻ ions are being reduced.

d)

Water is being decomposed.

98.

Which of the following metals can be plated onto an object using electroplating?

a)

Silver

b)

Nickel

c)

Copper

d)

All of the above

99.

What is the product formed at the anode during the electrolysis of aqueous AgNO₃ using inert electrodes?

a)

Silver metal

b)

Nitrogen dioxide

c)

Oxygen gas

d)

No reaction

100.

In a redox reaction, the substance that gets oxidized is:

a)

The oxidizing agent

b)

The reducing agent

c)

The catalyst

d)

The spectator ion

101.

What is the product formed at the cathode during the electrolysis of molten ZnCl₂?

a)

Zinc metal

b)

Chlorine gas

c)

Hydrogen gas

d)

Zinc chloride

102.

Which of the following statements is true about fuel cells compared to batteries?

a)

Fuel cells can continuously produce electricity as long as reactants are supplied.

b)

Batteries never need to be recharged.

c)

Fuel cells are less efficient than batteries.

d)

Batteries require a constant supply of fuel to operate.

103.

Calculate the [H⁺] and [OH⁻] in a 0.010 M solution of LiOH at 25°C. (Kw = 1.0 × 10⁻¹⁴)

a)

[H⁺] = 1.0 × 10⁻¹² M, [OH⁻] = 0.010 M

b)

[H⁺] = 1.0 × 10⁻¹⁰ M, [OH⁻] = 0.010 M

c)

[H⁺] = 1.0 × 10⁻¹² M, [OH⁻] = 1.0 × 10⁻² M

d)

[H⁺] = 1.0 × 10⁻⁸ M, [OH⁻] = 1.0 × 10⁻⁶ M

104.

Which of the following reactions represents the partial dissociation of a weak acid in water?

a)

HCl → H⁺ + Cl⁻

b)

H₂SO₄ → 2H⁺ + SO₄²⁻

c)

CH₃COOH ⇄ CH₃COO⁻ + H⁺

d)

NaOH → Na⁺ + OH⁻

105.

What is the pH of a 0.010 M solution of HCl at 25°C?

a)

2

b)

4

c)

7

d)

12

106.

Identify the acidic oxide from the following:

a)

MgO

b)

ZnO

c)

SO₃

d)

Al₂O₃

107.

Which of the following salts is basic in aqueous solution?

a)

NH₄Cl

b)

NaCl

c)

Na₂CO₃

d)

KNO₃

108.

When excess NaOH is added to NH₄NO₃, which gas is evolved?

a)

Hydrogen

b)

Ammonia

c)

Nitrogen

d)

Carbon dioxide

109.

What is the product formed when CaO reacts with H₂O?

a)

Ca(OH)₂

b)

CaCO₃

c)

CaCl₂

d)

CaSO₄

110.

Which of the following reactions represents the complete dissociation of a strong base?

a)

NH₃ + H₂O ⇄ NH₄⁺ + OH⁻

b)

NaOH → Na⁺ + OH⁻

c)

CH₃COOH ⇄ CH₃COO⁻ + H⁺

d)

H₂O ⇄ H⁺ + OH⁻

111.

Determine whether the salt Na₂SO₄ is acidic, basic, or neutral.

a)

Acidic

b)

Basic

c)

Neutral

d)

Amphoteric

112.

In the reaction NH₄NO₃ + KOH → KNO₃ + NH₃ + H₂O, what type of reaction is occurring?

a)

Neutralization

b)

Redox

c)

Precipitation

d)

Decomposition

113.

Which of the following is a neutral salt?

a)

Na₂CO₃

b)

NH₄Cl

c)

NaCl

d)

KOH

114.

What is the pH of a 0.10 M solution of CH₃COOH? (Ka = 1.8 × 10⁻⁵)

a)

2.9

b)

4.7

c)

7.0

d)

9.2

115.

Which of the following best explains why water is considered a weak electrolyte?

a)

It does not dissociate into ions.

b)

It completely dissociates into ions.

c)

It partially dissociates into ions.

d)

It only conducts electricity when molten.

116.

What is the product when NH₄NO₃ reacts with KOH?

a)

NH₃ and KNO₃

b)

NH₄OH and KNO₃

c)

NH₄OH and KNO₃ and H₂O

d)

NH₃ and KNO₃ and H₂O

117.

In the reaction Mg(s) + 2HCl(aq) → MgCl₂(aq) + H₂(g), what is the oxidizing agent?

a)

Mg

b)

HCl

c)

H₂

d)

MgCl₂

118.

Which method is best suited for preparing an insoluble salt?

a)

Titration method

b)

Precipitation method

c)

Excess method

d)

Crystallization method

119.

What is the main reason for using a pipette in a titration experiment?

a)

To measure large volumes accurately

b)

To transfer a precise volume of solution

c)

To hold the flask securely

d)

To indicate the endpoint visually

120.

Which of the following salts will hydrolyze in water to form a basic solution?

a)

NH₄Cl

b)

Na₂CO₃

c)

KNO₃

d)

HCl

121.

What is the net ionic equation for the reaction between MgO and H₂SO₄?

a)

MgO + H₂SO₄ → MgSO₄ + H₂O

b)

Mg²⁺ + SO₄²⁻ → MgSO₄

c)

O²⁻ + 2H⁺ → H₂O

d)

Mg + SO₄²⁻ → MgSO₄

122.

During the titration of 0.010 M HCl with 0.010 M NaOH, how much NaOH is needed to reach the equivalence point for 25.0 cm³ of HCl?

a)

25.0 cm³

b)

12.5 cm³

c)

50.0 cm³

d)

6.25 cm³

123.

Which of the following is NOT a characteristic property of acids?

a)

Sour taste

b)

Corrosive to metals

c)

Slippery feel

d)

Turn blue litmus paper red

124.

What is the primary reason for excess reagent in the excess method of salt preparation?

a)

To ensure complete precipitation

b)

To drive the reaction to completion

c)

To facilitate filtration

d)

To prevent side reactions

125.

Which of the following statements correctly describes the reaction between a strong acid and a weak base?

a)

The resulting solution is neutral.

b)

The resulting solution is acidic.

c)

The resulting solution is basic.

d)

No reaction occurs.

126.

Calculate the [H⁺] in a solution where pH = 5.00.

a)

1.00 × 10⁻⁵ M

b)

1.00 × 10⁻⁷ M

c)

1.00 × 10⁻⁹ M

d)

1.00 × 10⁻¹⁴ M

127.

Which of the following salts is formed from a weak acid and a weak base?

a)

NaCl

b)

NH₄NO₃

c)

K₂CO₃

d)

Na₂SO₄

128.

In the reaction Zn + Cu²⁺ → Zn²⁺ + Cu, which species is the oxidizing agent?

a)

Zn

b)

Cu²⁺

c)

Zn²⁺

d)

Cu

129.

What is the oxidation number of Mn in MnO₄⁻?

a)

+7

b)

+6

c)

+4

d)

+3

130.

Identify the reducing agent in the reaction 2Fe³⁺ + Zn → 2Fe²⁺ + Zn²⁺.

a)

Fe³⁺

b)

Zn

c)

Fe²⁺

d)

Zn²⁺

131.

Which of the following is an example of a non-combustion redox reaction?

a)

CH₄ + 2O₂ → CO₂ + 2H₂O

b)

Zn + CuSO₄ → ZnSO₄ + Cu

c)

C + O₂ → CO₂

d)

2H₂ + O₂ → 2H₂O

132.

In the half-reaction Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O, how many electrons are gained by each Cr atom?

a)

1

b)

2

c)

3

d)

6

133.

What is the product when CuO reacts with H₂?

a)

Cu and H₂O

b)

Cu and H₂O₂

c)

Cu²⁺ and H₂O

d)

Cu and O₂

134.

During the electrolysis of molten ZnCl₂, which species is oxidized?

a)

Zn²⁺

b)

Cl⁻

c)

Zn

d)

Cl₂

135.

What is the standard electrode potential for the reduction of Cu²⁺ to Cu?

a)

+0.34 V

b)

-0.34 V

c)

+0.77 V

d)

-0.77 V

136.

In the reaction 2Fe²⁺ + H₂O₂ + 2H⁺ → 2Fe³⁺ + 2H₂O, which species is reduced?

a)

Fe²⁺

b)

H₂O₂

c)

H⁺

d)

Fe³⁺

137.

Which of the following best describes a reducing agent?

a)

A substance that gains electrons.

b)

A substance that loses electrons.

c)

A substance that remains unchanged.

d)

A substance that is reduced.

138.

In the reaction 3CH₃OH + 2Cr₂O₇²⁻ + 16H⁺ → 6CH₂O + 4Cr³⁺ + 11H₂O, which element undergoes oxidation?

a)

Carbon in CH₃OH

b)

Chromium in Cr₂O₇²⁻

c)

Hydrogen in H⁺

d)

Oxygen in H₂O

139.

Which of the following statements is true about oxidizing agents?

a)

They donate electrons.

b)

They become oxidized in reactions.

c)

They accept electrons.

d)

They reduce other substances.

140.

What is the product formed at the cathode during the electrolysis of aqueous CuSO₄ using inert electrodes?

a)

Cu²⁺

b)

Cu metal

c)

O₂ gas

d)

H₂ gas

141.

Which of the following half-reactions represents oxidation?

a)

Cu²⁺ + 2e⁻ → Cu

b)

Zn → Zn²⁺ + 2e⁻

c)

O₂ + 4H⁺ + 4e⁻ → 2H₂O

d)

Fe³⁺ + e⁻ → Fe²⁺

142.

In an electrolytic cell, what occurs at the cathode?

a)

Oxidation

b)

Reduction

c)

Both oxidation and reduction

d)

Neither oxidation nor reduction

143.

Which of the following metals is least reactive and thus least likely to be oxidized in a redox reaction?

a)

Sodium

b)

Magnesium

c)

Copper

d)

Zinc

144.

During the electrolysis of dilute NaCl solution using inert electrodes, which gas is produced at the anode?

a)

Hydrogen

b)

Chlorine

c)

Oxygen

d)

Sodium

145.

What is the oxidizing agent in the reaction 2H₂ + O₂ → 2H₂O?

a)

H₂

b)

O₂

c)

H₂O

d)

None

146.

In the displacement reaction Zn + Cu²⁺ → Zn²⁺ + Cu, what is the role of zinc?

a)

Oxidizing agent

b)

Reducing agent

c)

Catalyst

d)

Both A and B

147.

Which of the following is true about fuel cells compared to batteries?

a)

Fuel cells can continuously produce electricity as long as reactants are supplied.

b)

Batteries can be recharged indefinitely without any loss.

c)

Fuel cells require periodic refueling like batteries.

d)

Batteries produce more energy per unit mass than fuel cells.

148.

What is the primary product at the anode during the electrolysis of molten NaCl?

a)

Sodium metal

b)

Chlorine gas

c)

Oxygen gas

d)

Hydrogen gas

149.

In an electrochemical cell, which electrode serves as the site of reduction?

a)

Anode

b)

Cathode

c)

Both electrodes

d)

Neither electrode

150.

During the electroplating of a spoon with silver, what occurs at the anode?

a)

Silver ions are reduced to silver metal.

b)

Silver metal is oxidized to silver ions.

c)

Electrons are gained by silver ions.

d)

No reaction occurs at the anode.

151.

Which of the following statements correctly describes the role of electrons in redox reactions?

a)

Electrons are created during oxidation.

b)

Electrons are consumed during reduction.

c)

Electrons are neither consumed nor produced.

d)

Electrons are transferred from oxidizing to reducing agents.

152.

In the reaction 2Fe²⁺ + H₂O₂ + 2H⁺ → 2Fe³⁺ + 2H₂O, what is the change in oxidation state for iron?

a)

+2 to +3

b)

+3 to +2

c)

+2 to +0

d)

No change

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