Solutions and Equilibria Quizzes - Comprehensive Chemistry

Question 1

Which of the following is NOT a factor that affects the solubility of a gas in a liquid?

Accepted Answer

Volume of the gas

Answer

Temperature

Answer

Pressure

Answer

Nature of the gas

Question 2

Which of the following reactions is an example of heterogeneous equilibrium?

Accepted Answer

BaSO4(s) + H2SO4(aq) ⇌ BaSO4·H2SO4(s)

Answer

2NO2(g) ⇌ N2O4(g)

Answer

CH3COOH(aq) + H2O(l) ⇌ CH3COO-(aq) + H3O+(aq)

Answer

NH3(aq) + H2O(l) ⇌ NH4+(aq) + OH-(aq)

Question 3

Which of the following is NOT a characteristic of colligative properties?

Accepted Answer

Affected by the size or shape of the solute particles

Answer

Dependent only on the concentration of the solution particles

Answer

Independent of the nature of the solute particles

Answer

Used to determine the molar mass of a solute

Question 4

The solubility of a gas in a liquid decreases with increasing:

Accepted Answer

Temperature

Answer

Pressure

Answer

Volume of the liquid

Answer

Surface area of the liquid

Question 5

Which of the following is a strong base?

Accepted Answer

Sodium hydroxide

Answer

Ammonium hydroxide

Answer

Acetic acid

Answer

Carbonic acid

Question 6

The conjugate acid of a weak base is:

Accepted Answer

A weaker acid

Answer

A stronger acid

Answer

A stronger base

Answer

A weaker base

Question 7

Which of the following is a buffer solution?

Accepted Answer

A mixture of a weak acid and its conjugate base

Answer

A mixture of a strong acid and its conjugate base

Answer

A mixture of water and a salt

Answer

A mixture of a weak base and a strong acid

Question 8

A solution is prepared by dissolving 0.1 mol of glucose (C6H12O6) in 1 kg of water. What is the molality of this solution?

Accepted Answer

0.01 m

Answer

0.1 m

Answer

1 m

Answer

10 m

Question 9

Which of the following ions is most likely to form a precipitate when added to a solution of potassium iodide?

Accepted Answer

Lead(II)

Answer

Sodium

Answer

Calcium

Answer

Magnesium

Question 10

In a saturated solution, the rate of dissolution is:

Accepted Answer

Equal to the rate of crystallization

Answer

Faster than the rate of crystallization

Answer

Slower than the rate of crystallization

Answer

Independent of the rate of crystallization

Question 11

Which of the following is a weak acid?

Accepted Answer

Ethanoic acid

Answer

Hydrochloric acid

Answer

Nitric acid

Answer

Sulfuric acid

Question 12

The pH of a solution is 3. What is the concentration of hydrogen ions (H+) in this solution?

Accepted Answer

10^-3 M

Answer

10^-4 M

Answer

10^-5 M

Answer

10^-6 M

Question 13

Which of the following reactions is an example of a heterogeneous equilibrium?

Accepted Answer

CaCO₃(s) ⇌ CaO(s) + CO₂(g)

Answer

2NO(g) ⇌ N₂(g) + O₂(g)

Answer

CH₃COOH(aq) + H₂O(l) ⇌ CH₃COO⁻(aq) + H₃O⁺(aq)

Answer

Fe³⁺(aq) + SCN⁻(aq) ⇌ [Fe(SCN)]²⁺(aq)

Question 14

Which of the following factors will shift the equilibrium of the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) to the right?

Accepted Answer

Increasing the temperature

Answer

Decreasing the pressure

Answer

Adding a catalyst

Answer

Removing NH₃(g)

Question 15

Which of the following solutions has the highest molarity?

Accepted Answer

25 g of CaCl₂ in 1000 cm³ of solution

Answer

10 g of NaCl in 250 cm³ of solution

Answer

15 g of NaOH in 500 cm³ of solution

Answer

20 g of KCl in 750 cm³ of solution

Question 16

Which factor does not affect the position of equilibrium in a chemical reaction?

Accepted Answer

Addition of an inert gas

Answer

Temperature

Answer

Concentration of reactants and products

Question 17

Which of the following is NOT classified as a colligative property of a solution?

Accepted Answer

Electrical conductivity

Answer

Boiling point elevation

Answer

Freezing point depression

Answer

Vapor pressure lowering

Question 18

Consider the dissociation of acetic acid in water: CH3COOH(aq) + H2O(l) <=> CH3COO-(aq) + H3O+(aq). Which ion in this reaction is considered a spectator ion?

Accepted Answer

H2O

Answer

CH3COOH

Answer

CH3COO-

Answer

H3O+

Question 19

Consider the equilibrium reaction: 2SO2(g) + O2(g) <=> 2SO3(g) + heat. According to Le Chatelier's principle, which change will shift the equilibrium to the right (favoring the formation of products)?

Accepted Answer

Increase in pressure

Answer

Decrease in temperature

Answer

Removal of SO2

Answer

Addition of a catalyst

Question 20

Which of the following is classified as a strong base?

Accepted Answer

Sodium hydroxide (NaOH)

Answer

Ammonia (NH3)

Answer

Acetic acid (CH3COOH)

Answer

Carbonic acid (H2CO3)

Question 21

Which of the following is NOT a colligative property of solutions?

Accepted Answer

Molarity

Answer

Boiling point elevation

Answer

Freezing point depression

Answer

Osmotic pressure

Question 22

A 0.1 mol/dm3 solution of sodium chloride has a freezing point of -0.37 °C. What is the van't Hoff factor for sodium chloride?

Accepted Answer

2

Answer

1

Answer

2.5

Answer

Cannot be determined from the provided information

Question 23

Which of the following reactions is NOT in equilibrium?

Accepted Answer

N2(g) + 3H2(g) → 2NH3(g)

Answer

H2(g) + I2(g) ⇌ 2HI(g)

Answer

CO(g) + 2H2(g) ⇌ CH3OH(g)

Answer

Fe3+(aq) + SCN-(aq) ⇌ [Fe(SCN)]2+(aq)

Question 24

Which of the following is a way to predict the direction of a shift in equilibrium?

Accepted Answer

Le Chatelier's principle

Answer

The Gibbs free energy equation

Answer

The Arrhenius equation

Answer

The ideal gas law

Question 25

Which of the following is a strong electrolyte?

Accepted Answer

Sodium chloride

Answer

Sucrose

Answer

Ammonia

Answer

Ethanol

Question 26

What is the approximate pH of a 0.01 mol/dm3 solution of hydrochloric acid?

Accepted Answer

1

Answer

2

Answer

3

Answer

4

Question 27

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

Accepted Answer

Dependent on the nature of the solute particles

Answer

Independent of the identity of the solute

Answer

Proportional to the concentration of the solute

Answer

Related to the intermolecular forces between solvent and solute particles

Question 28

In a chemical equilibrium, the rate of the forward reaction is:

Accepted Answer

Equal to the rate of the reverse reaction

Answer

Greater than the rate of the reverse reaction

Answer

Less than the rate of the reverse reaction

Answer

Zero

Question 29

A buffer solution is characterized by:

Accepted Answer

Resistance to changes in pH when small amounts of acid or base are added

Answer

A pH of exactly 7

Answer

High electrical conductivity

Answer

A high concentration of hydrogen ions

Question 30

Which of the following is classified as a weak base?

Accepted Answer

Ammonia

Answer

Sodium hydroxide

Answer

Potassium hydroxide

Answer

Hydrochloric acid

Question 31

The pH of a solution is measured to be 4. What is the molar concentration of hydrogen ions in the solution?

Accepted Answer

10^-4 M

Answer

10^-5 M

Answer

10^-6 M

Answer

10^-7 M

Question 32

Which of the following statements describes the common ion effect?

Accepted Answer

The solubility of a precipitate increases in the presence of a common ion

Answer

The pH of a solution decreases in the presence of a strong acid

Answer

The rate of a reaction decreases in the presence of a catalyst

Answer

The boiling point of a solution increases in the presence of a non-volatile solute

Question 33

A solution has a pH of 9. Which of the following indicators would be most appropriate to use to determine the equivalence point of an acid-base titration?

Accepted Answer

Phenolphthalein

Answer

Methyl orange

Answer

Litmus

Answer

Methyl red

Question 34

Which of the following is NOT a colligative property of solutions?

Accepted Answer

Electrical conductivity

Answer

Boiling point elevation

Answer

Freezing point depression

Question 35

Which of the following is a strong electrolyte?

Accepted Answer

NaCl

Answer

NH₃

Answer

CH₃COOH

Answer

C₆H₁₂O₆

Question 36

What is the equilibrium constant expression for the following reaction?

Accepted Answer

K = [NH⁺⁻⁽⁺⁹][OH⁻⁽]/[NH₃]

Answer

K = [OH⁻⁽]/[NH₃]

Answer

K = [NH⁺⁻⁽⁺⁹]/[NH₃]

Question 37

What is the conjugate acid of NH₃?

Accepted Answer

NH⁺⁻⁽⁺⁹

Answer

H⁻⁽

Answer

OH⁻⁽

Answer

H₂O

Question 38

What is the molar solubility of a salt with a solubility product of 2 × 10⁻-10⁽?

Accepted Answer

1.4 × 10⁻-5⁽ M

Answer

3.2 × 10⁻-5⁽ M

Answer

2.8 × 10⁻-5⁽ M

Answer

2.0 × 10⁻-5⁽ M

Question 39

A colligative property that measures the lowering of the freezing point of a solvent caused by a solute is known as the:

Accepted Answer

Cryoscopic constant

Answer

Ebullioscopic constant

Answer

Osmotic pressure

Answer

Vapor pressure lowering

Question 40

For the reaction A + 2B <=> C, the equilibrium constant expression is:

Accepted Answer

Kc = [C]/[A][B]^2

Answer

Kc = [C]^2/[A][B]

Answer

Kc = [A][B]/[C]

Question 41

Which of the following is a characteristic of a buffer solution?

Accepted Answer

Contains a weak acid and its conjugate base

Answer

Has a pH of exactly 7

Answer

Contains only a strong acid

Question 42

The common ion effect refers to:

Accepted Answer

The suppression of ionization of a weak acid or base when a common ion is added.

Answer

The enhancement of ionization of a weak acid or base when a common ion is added.

Question 43

Which of the following reactions is an example of a precipitation reaction?

Accepted Answer

CaCl2(aq) + Na2SO4(aq) → CaSO4(s) + 2NaCl(aq)

Answer

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

Answer

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g)

Answer

2H2(g) + O2(g) → 2H2O(g)

Question 44

Identify the net ionic equation for the reaction between aqueous solutions of sodium carbonate and calcium chloride.

Accepted Answer

Ca2+(aq) + CO32-(aq) → CaCO3(s)

Answer

2Na+(aq) + CO32-(aq) → Na2CO3(aq)

Answer

Ca2+(aq) + 2Cl-(aq) → CaCl2(aq)

Answer

Na+(aq) + Cl-(aq) → NaCl(aq)

Question 45

Which substance is classified as a strong electrolyte?

Accepted Answer

Sodium chloride

Answer

Ammonia

Answer

Water

Answer

Acetic acid

Question 46

A 0.1 M solution of NaCl has a freezing point of -0.37 °C. Calculate the van't Hoff factor (i) for NaCl.

Accepted Answer

2

Answer

3

Answer

1

Answer

1.5

Question 47

Identify the heterogeneous equilibrium reaction among the following.

Accepted Answer

CaCO3 (s) ⇌ CaO (s) + CO2 (g)

Answer

H2O (l) ⇌ H+ (aq) + OH- (aq)

Answer

Fe3+ (aq) + SCN- (aq) ⇌ Fe(SCN)2+ (aq)

Answer

2NO2 (g) ⇌ 2NO (g) + O2 (g)

Question 48

For the reaction: A + B ⇌ C + D, the equilibrium constant (Kc) is 4. If the initial concentrations of A, B, C, and D are 1 M, 2 M, 0 M, and 0 M, respectively, determine the equilibrium concentration of C.

Accepted Answer

0.8 M

Answer

1.6 M

Answer

3.2 M

Answer

0.4 M

Question 49

Predict the change in equilibrium position of the following reaction, N2 (g) + 3H2 (g) ⇌ 2NH3 (g), when the pressure is increased.

Accepted Answer

Shifts to the product side

Answer

Remains unchanged

Answer

Shifts to the reactant side

Answer

Cannot be predicted

Question 50

Determine the pH of a 0.01 M solution of a weak acid with a Ka of 1 x 10-5.

Accepted Answer

4

Answer

5

Answer

6

Answer

3

Question 51

Which of the following salts is most likely to undergo hydrolysis in water?

Accepted Answer

NaF

Answer

NH4Cl

Answer

CaCl2

Answer

NaCl

Question 52

Identify the conjugate base of H2O.

Accepted Answer

OH-

Answer

H3O+

Answer

H+

Answer

H2O2

Question 53

Which of the following is a buffer solution?

Accepted Answer

A mixture of a weak acid and its conjugate base

Answer

A solution of a salt

Answer

A solution of a weak base

Answer

A mixture of a strong acid and a strong base

Question 54

Calculate the molar solubility of CaCO3 in a solution with [CO32-] = 0.01 M.

Accepted Answer

1 x 10-9 M

Answer

1 x 10-5 M

Answer

1 x 10-1 M

Answer

1 x 10-3 M