Question 1:

What is the expression for the equilibrium constant, \(K_c\)?

Options:

• (A) \(\dfrac{[SO_3]^2}{[O_2][SO_2]^2}\)
• (B) \(\dfrac{2[SO_3]}{[O_2]2[SO_2]}\)
• (C) \(\dfrac{[O_2][SO_2]^2}{[SO_3]^2}\)
• (D) \(\dfrac{[O_2]2[SO_2]}{2[SO_3]}\)

Correct Answer: (A)

Question 2:

Which of the following would cause the reverse reaction to speed up?

Options:

• (A) Adding more \(SO_3\)
• (B) Raising the pressure
• (C) Lowering the temperature
• (D) Removing some \(SO_2\)

Correct Answer: (A)

Question 3:

The value for \(K_c\) at 25°C is 8.1. What must happen in order for the reaction to reach equilibrium if the initial concentrations of all three species were 2.0 M?

Options:

• (A) The rate of the forward reaction would increase, and \([SO_3]\) would decrease.
• (B) The rate of the reverse reaction would increase, and \([SO_3]\) would decrease.
• (C) Both the rate of the forward and reverse reactions would increase, and the value for the equilibrium constant would also increase.
• (D) No change would occur in either the rate of reaction or the concentrations of any of the species.

Correct Answer: (A)

Question 4:

Which of the following would cause a reduction in the value for the equilibrium constant?

Options:

• (A) Increasing the amount of \(SO_3\)
• (B) Reducing the amount of \(O_2\)
• (C) Raising the temperature
• (D) Lowering the temperature

Correct Answer: (C)

Question 5:

The solubility product, \(K_{sp}\), of AgCl is \(1.8 \times 10^{-10}\). Which of the following expressions is equal to the solubility of AgCl?

Options:

• (A) \((1.8 \times 10^{-10})^2\)
• (B) \(1.8 \times 10^{-10}\)
• (C) \(\dfrac{1.8 \times 10^{-10}}{2}\)
• (D) \(\sqrt{1.8 \times 10^{-10}}\)

Correct Answer: (D)

Question 6:

Which of the following expressions is equal to the \(K_{sp}\) of \(Ag_2CO_3\)?

Options:

• (A) \(K_{sp} = [Ag^+][CO_3^{2-}]\)
• (B) \(K_{sp} = 2[Ag^+][CO_3^{2-}]\)
• (C) \(K_{sp} = [Ag^+]^2[CO_3^{2-}]\)
• (D) \(K_{sp} = [Ag^+]^2[CO_3^{2-}]^2\)

Correct Answer: (C)

Question 7:

If the solubility of \(BaF_2\) is equal to \(x\), which of the following expressions is equal to the solubility product, \(K_{sp}\), for \(BaF_2\)?

Options:

• (A) \(x^2\)
• (B) \(2x^2\)
• (C) \(2x^3\)
• (D) \(4x^3\)

Correct Answer: (D)

Question 8:

What are the concentrations of Sr²⁺ and F⁻ in the beaker?

Options:

• (A) \([Sr^{2+}] = 1.0 \times 10^{-3} M, [F^-] = 1.0 \times 10^{-3} M\)
• (B) \([Sr^{2+}] = 1.0 \times 10^{-3} M, [F^-] = 2.0 \times 10^{-3} M\)
• (C) \([Sr^{2+}] = 2.0 \times 10^{-3} M, [F^-] = 1.0 \times 10^{-3} M\)
• (D) \([Sr^{2+}] = 2.0 \times 10^{-3} M, [F^-] = 2.0 \times 10^{-3} M\)

Correct Answer: (B)

Question 9:

If some of the solution evaporates overnight, which of the following will occur?

Options:

• (A) The mass of the solid and the concentration of the ions will stay the same.
• (B) The mass of the solid and the concentration of the ions will increase.
• (C) The mass of the solid will decrease, and the concentration of the ions will stay the same.
• (D) The mass of the solid will increase, and the concentration of the ions will stay the same.

Correct Answer: (D)

Question 10:

How could the concentration of Sr²⁺ ions in solution be decreased?

Options:

• (A) Adding some NaF to the beaker
• (B) Adding some Sr(NO₃)₂ to the beaker
• (C) Raising the temperature
• (D) Lowering the temperature

Correct Answer: (A)

Question 11:

For a reaction involving nitrogen monoxide inside a sealed flask, the value for the reaction quotient (\(Q\)) was found to be \(1.1 \times 10^2\) at a given point. If, after this point, the amount of NO gas in the flask increased, which reaction is most likely taking place in the flask?

Options:

• (A) NOBr(g) ⇌ NO(g) + ½ Br₂(g), \(K_c = 3.4 \times 10^{-2}\)
• (B) 2 NOCl(g) ⇌ 2 NO(g) + Cl₂(g), \(K_c = 1.6 \times 10^{-5}\)
• (C) 2 NO(g) + 2 H₂(g) ⇌ N₂(g) + 2 H₂O(g), \(K_c = 4.0 \times 10^6\)
• (D) N₂(g) + O₂(g) ⇌ 2 NO(g), \(K_c = 4.2 \times 10^2\)

Correct Answer: (D)

Question 12:

2 HI(g) + Cl₂(g) ⇌ 2 HCl(g) + I₂(g) + energy

A gaseous reaction occurs and comes to equilibrium, as shown above. Which of the following changes to the system will serve to increase the number of moles of I₂ present at equilibrium?

Options:

• (A) Increasing the volume at constant temperature
• (B) Decreasing the volume at constant temperature
• (C) Increasing the temperature at constant volume
• (D) Decreasing the temperature at constant volume

Correct Answer: (D)

Question 13:

2 NOBr(g) ⇌ 2 NO(g) + Br₂(g)

The reaction above came to equilibrium at a temperature of 100°C. At equilibrium, the partial pressure due to NOBr was 4 atm, the partial pressure due to NO was 4 atm, and the partial pressure due to Br₂ was 2 atm. What is the equilibrium constant, \(K_p\), for this reaction at 100°C?

Options:

• (A) \(\frac{1}{4}\)
• (B) \(\frac{1}{2}\)
• (C) 1
• (D) 2

Correct Answer: (D)

Question 14:

Br₂(g) + I₂(g) ⇌ 2 IBr(g)

At 150°C, the equilibrium constant, \(K_p\), for the reaction shown above has a value of 300. This reaction was allowed to reach equilibrium in a sealed container and the partial pressure due to IBr(g) was found to be 3 atm. Which of the following could be the partial pressures due to Br₂(g) and I₂(g) in the container?

Options:

• (A) \(P_{Br₂} = 0.1 \, atm, P_{I₂} = 0.3 \, atm\)
• (B) \(P_{Br₂} = 0.3 \, atm, P_{I₂} = 1 \, atm\)
• (C) \(P_{Br₂} = 1 \, atm, P_{I₂} = 1 \, atm\)
• (D) \(P_{Br₂} = 1 \, atm, P_{I₂} = 3 \, atm\)

Correct Answer: (A)

Question 15:

What is the identity of the excess reactant?

Options:

• (A) AgNO₃
• (B) Ag₂SO₄
• (C) KNO₃
• (D) K₂SO₄

Correct Answer: (A)

Question 16:

If the beaker above were left uncovered for several hours, what would happen?

Options:

• (A) Some of the Ag₂SO₄ would dissolve
• (B) Some of the spectator ions would evaporate into the atmosphere
• (C) The solution would become electrically imbalanced
• (D) Additional Ag₂SO₄ would precipitate

Correct Answer: (D)

Question 17:

Which ion concentrations below would have led the precipitate to form?

Options:

• (A) \([Ag^+] = 0.01 M, [SO_4^{2-}] = 0.01 M\)
• (B) \([Ag^+] = 0.10 M, [SO_4^{2-}] = 0.01 M\)
• (C) \([Ag^+] = 0.01 M, [SO_4^{2-}] = 0.10 M\)
• (D) This is impossible to determine without knowing the total volume of the solution.

Correct Answer: (B)

Question 18:

PCl₃(g) + Cl₂(g) ⇌ PCl₅(g), ΔH = -92.5 kJ/mol

In which of the following ways could the reaction above be manipulated to create more product?

Options:

• (A) Decreasing the concentration of PCl₃
• (B) Increasing the pressure
• (C) Increasing the temperature
• (D) None of the above

Correct Answer: (B)

Question 19:

A sample of solid MgCl₂ would be most soluble in which of the following solutions?

Options:

• (A) LiOH (aq)
• (B) CBr₄ (aq)
• (C) Mg(NO₃)₂ (aq)
• (D) AlCl₃ (aq)

Correct Answer: (A)

Question 20:

For a reaction involving sulfur dioxide and oxygen inside a sealed flask, the value for the reaction quotient \(Q\) was found to be \(2.5 \times 10^1\) at a given point. If, after this point, the amount of SO₂ gas in the flask increased, which reaction is most likely taking place in the flask?

Options:

• (A) SO₂(g) + O₂(g) ⇌ 2 SO₃(g), \(K_c = 1.2 \times 10^2\)
• (B) 2 SO₃(g) ⇌ 2 SO₂(g) + O₂(g), \(K_c = 3.4 \times 10^{-3}\)
• (C) SO₃(g) ⇌ SO₂(g) + ½ O₂(g), \(K_c = 5.6 \times 10^{-1}\)
• (D) 2 SO₂(g) + O₂(g) ⇌ 2 SO₃(g), \(K_c = 2.0 \times 10^1\)

Correct Answer: (B)

Question 21:

In a reaction between nitrogen and hydrogen to produce ammonia, the equilibrium constant \(K_c\) is \(4.5 \times 10^2\) at 450°C. If the reaction quotient \(Q\) is \(5.0 \times 10^2\), which direction will the reaction proceed?

Options:

• (A) The reaction will proceed towards the products.
• (B) The reaction will proceed towards the reactants.
• (C) The reaction is already at equilibrium.
• (D) The reaction will stop immediately.

Correct Answer: (B)

Question 22:

At a certain temperature, the equilibrium constant \(K_c\) for the following reaction is \(3.2 \times 10^{-4}\):

2 H₂(g) + O₂(g) ⇌ 2 H₂O(g)

If the concentrations of H₂ and O₂ are both increased, how will the equilibrium shift?

Options:

• (A) The equilibrium will shift towards the products.
• (B) The equilibrium will shift towards the reactants.
• (C) The equilibrium will remain unchanged.
• (D) The reaction will stop.

Correct Answer: (A)

Question 23:

A reaction has the following equilibrium expression:

\(K_c = \frac{[CO_2][H_2O]}{[CH_4][O_2]^2}\)

Which of the following reactions corresponds to this equilibrium expression?

Options:

• (A) CH₄(g) + 2 O₂(g) ⇌ CO₂(g) + 2 H₂O(g)
• (B) CH₄(g) + O₂(g) ⇌ CO(g) + 2 H₂O(g)
• (C) CO₂(g) + 2 H₂O(g) ⇌ CH₄(g) + O₂(g)
• (D) CO(g) + H₂ ⇌ CH₄(g) + O₂(g)

Correct Answer: (A)

Question 24:

The solubility product \(K_{sp}\) of silver chloride (AgCl) is \(1.8 \times 10^{-10}\). What is the molar solubility of AgCl in pure water?

Options:

• (A) \(1.8 \times 10^{-5}\) M
• (B) \(1.3 \times 10^{-5}\) M
• (C) \(1.8 \times 10^{-10}\) M
• (D) \(1.3 \times 10^{-10}\) M

Correct Answer: (B)

Question 25:

The solubility product \(K_{sp}\) of lead(II) fluoride (PbF₂) is \(4.0 \times 10^{-8}\). What is the molar solubility of PbF₂ in pure water?

Options:

• (A) \(1.0 \times 10^{-4}\) M
• (B) \(2.0 \times 10^{-4}\) M
• (C) \(1.6 \times 10^{-3}\) M
• (D) \(1.0 \times 10^{-3}\) M

Correct Answer: (C)

Question 26:

The solubility product \(K_{sp}\) of calcium hydroxide (Ca(OH)₂) is \(5.5 \times 10^{-6}\). What is the molar solubility of Ca(OH)₂ in pure water?

Options:

• (A) \(1.5 \times 10^{-2}\) M
• (B) \(2.0 \times 10^{-2}\) M
• (C) \(1.2 \times 10^{-2}\) M
• (D) \(1.0 \times 10^{-2}\) M

Correct Answer: (C)

Question 27:

What is the \(K_{sp}\) expression for the compound barium sulfate (BaSO₄)?

Options:

• (A) \(K_{sp} = [Ba^{2+}] [SO_4^{2-}]\)
• (B) \(K_{sp} = [Ba^{2+}]^2 [SO_4^{2-}]^2\)
• (C) \(K_{sp} = [Ba^{2+}]^2 [SO_4^{2-}]\)
• (D) \(K_{sp} = [Ba^{2+}] [SO_4^{2-}]^2\)

Correct Answer: (A)

Question 28:

If the solubility product \(K_{sp}\) of magnesium carbonate (MgCO₃) is \(3.5 \times 10^{-8}\), what is the concentration of carbonate ions \([CO_3^{2-}]\) in a saturated solution?

Options:

• (A) \(5.9 \times 10^{-4}\) M
• (B) \(1.9 \times 10^{-4}\) M
• (C) \(3.5 \times 10^{-8}\) M
• (D) \(1.0 \times 10^{-5}\) M

Correct Answer: (B)

Question 29:

Which of the following will decrease the solubility of calcium phosphate \((Ca_3(PO_4)_2)\) in water?

Options:

• (A) Adding HCl
• (B) Adding Ca(NO₃)₂
• (C) Increasing temperature
• (D) Adding Na₃PO₄

Correct Answer: (B)

Question 30:

The \(K_{sp}\) of copper(II) hydroxide \((Cu(OH)_2)\) is \(2.2 \times 10^{-20}\). If the concentration of \(OH^{-}\) ions in a solution is \(1.0 \times 10^{-6}\) M, what is the concentration of \(Cu^{2+}\) ions?

Options:

• (A) \(2.2 \times 10^{-8}\) M
• (B) \(2.2 \times 10^{-14}\) M
• (C) \(1.1 \times 10^{-7}\) M
• (D) \(4.4 \times 10^{-20}\) M

Correct Answer: (A)

Question 31:

The solubility product \(K_{sp}\) of barium sulfate (BaSO₄) is \(1.1 \times 10^{-10}\). If the ion product \(Q\) for a given solution is \(2.5 \times 10^{-10}\), what will happen when barium chloride (BaCl₂) is added to the solution?

Options:

• (A) BaSO₄ will precipitate out of the solution
• (B) The solution will remain unsaturated
• (C) BaSO₄ will dissolve completely
• (D) No change will occur

Correct Answer: (A)

Question 32:

The \(K_{sp}\) of calcium carbonate (CaCO₃) is \(4.5 \times 10^{-9}\). If the concentration of calcium ions is \(3.0 \times 10^{-3}\) M and the concentration of carbonate ions is \(2.0 \times 10^{-3}\) M, what is the value of the ion product \(Q\), and will precipitation occur?

Options:

• (A) \(Q = 6.0 \times 10^{-6}\), precipitation will occur
• (B) \(Q = 6.0 \times 10^{-9}\), precipitation will not occur
• (C) \(Q = 6.0 \times 10^{-6}\), precipitation will not occur
• (D) \(Q = 6.0 \times 10^{-9}\), precipitation will occur

Correct Answer: (A)

Question 33:

The solubility product \(K_{sp}\) of magnesium hydroxide (Mg(OH)₂) is \(8.9 \times 10^{-12}\). What is the molar solubility of Mg(OH)₂ in a solution where the concentration of hydroxide ions is fixed at \(1.0 \times 10^{-4}\) M?

Options:

• (A) \(8.9 \times 10^{-12}\) M
• (B) \(8.9 \times 10^{-8}\) M
• (C) \(8.9 \times 10^{-4}\) M
• (D) \(8.9 \times 10^{-6}\) M

Correct Answer: (B)

Question 34:

The ion product \(Q\) for a solution of iron(III) hydroxide (Fe(OH)₃) is \(4.0 \times 10^{-36}\). If the \(K_{sp}\) of Fe(OH)₃ is \(2.5 \times 10^{-39}\), what can be concluded about the solution?

Options:

• (A) The solution is supersaturated, and Fe(OH)₃ will precipitate
• (B) The solution is saturated, and no precipitation will occur
• (C) The solution is unsaturated, and Fe(OH)₃ will dissolve
• (D) The solution is supersaturated, but no precipitation will occur

Correct Answer: (A)

Question 35:

If the solubility product \(K_{sp}\) of silver sulfate (Ag₂SO₄) is \(1.2 \times 10^{-5}\), what is the molar solubility of silver sulfate in water?

Options:

• (A) \(1.0 \times 10^{-2}\) M
• (B) \(1.2 \times 10^{-2}\) M
• (C) \(1.6 \times 10^{-3}\) M
• (D) \(4.0 \times 10^{-2}\) M

Correct Answer: (C)

Question 36:

For a solution of calcium fluoride (CaF₂), the ion product \(Q\) is \(1.0 \times 10^{-10}\) and the \(K_{sp}\) is \(3.9 \times 10^{-11}\). What will happen in the solution?

Options:

• (A) CaF₂ will precipitate
• (B) CaF₂ will dissolve
• (C) No change will occur
• (D) The solution will remain supersaturated

Correct Answer: (A)

Question 37:

The solubility product \(K_{sp}\) of lead(II) chloride (PbCl₂) is \(1.7 \times 10^{-5}\). What will happen when more chloride ions are added to the solution?

Options:

• (A) PbCl₂ will precipitate
• (B) PbCl₂ will dissolve further
• (C) The solution will become unsaturated
• (D) No change will occur

Correct Answer: (A)

Question 38:

The solubility product \(K_{sp}\) of silver bromide (AgBr) is \(5.0 \times 10^{-13}\). If a solution has an ion product \(Q\) of \(3.0 \times 10^{-13}\), what can be concluded about the solution?

Options:

• (A) The solution is supersaturated, and AgBr will precipitate
• (B) The solution is saturated, and no precipitation will occur
• (C) The solution is unsaturated, and AgBr will dissolve
• (D) The solution is supersaturated, but no precipitation will occur

Correct Answer: (C)

Question 39:

A solution contains \(5.0 \times 10^{-3}\) M of Ba²⁺ and \(1.0 \times 10^{-2}\) M of SO₄^2-. The \(K_{sp}\) of barium sulfate (BaSO₄) is \(1.1 \times 10^{-10}\). What is the value of the ion product \(Q\), and will precipitation occur?

Options:

• (A) \(Q = 5.0 \times 10^{-5}\), precipitation will not occur
• (B) \(Q = 5.0 \times 10^{-5}\), precipitation will occur
• (C) \(Q = 5.0 \times 10^{-3}\), precipitation will occur
• (D) \(Q = 5.0 \times 10^{-3}\), precipitation will not occur

Correct Answer: (B)

Question 40:

The \(K_{sp}\) of calcium hydroxide (Ca(OH)₂) is \(6.5 \times 10^{-6}\). If the concentration of hydroxide ions in a solution is \(2.0 \times 10^{-3}\) M, what is the molar solubility of Ca(OH)₂ in this solution?

Options:

• (A) \(1.6 \times 10^{-4}\) M
• (B) \(1.6 \times 10^{-2}\) M
• (C) \(6.5 \times 10^{-2}\) M
• (D) \(3.2 \times 10^{-4}\) M

Correct Answer: (A)

Question 41:

A solution is prepared by mixing \(1.0 \times 10^{-3}\) M NaCl and \(1.0 \times 10^{-3}\) M AgNO₃. If the solubility product \(K_{sp}\) of silver chloride (AgCl) is \(1.8 \times 10^{-10}\), what will happen in this solution?

Options:

• (A) No reaction will occur
• (B) AgCl will dissolve
• (C) AgCl will precipitate
• (D) The solution will become supersaturated

Correct Answer: (C)

Question 42:

The solubility product \(K_{sp}\) of lead(II) bromide (PbBr₂) is \(6.6 \times 10^{-6}\). What is the molar solubility of PbBr₂ in pure water?

Options:

• (A) \(1.2 \times 10^{-2}\) M
• (B) \(1.6 \times 10^{-2}\) M
• (C) \(2.0 \times 10^{-2}\) M
• (D) \(2.2 \times 10^{-2}\) M

Correct Answer: (A)

Question 43:

A solution contains \(2.0 \times 10^{-3}\) M \(Ca^{2+}\) and \(1.0 \times 10^{-3}\) M \(C_2O_4^{2-}\). The solubility product \(K_{sp}\) of calcium oxalate (\(CaC_2O_4\)) is \(2.3 \times 10^{-9}\). Will precipitation occur?

Options:

• (A) Yes, because \(Q > K_{sp}\)
• (B) No, because \(Q < K_{sp}\)
• (C) No, because \(Q = K_{sp}\)
• (D) Yes, because \(Q = K_{sp}\)

Correct Answer: (A)

Question 44:

Which of the following will increase the solubility of barium sulfate (BaSO₄)?

Options:

• (A) Adding \(H_2SO_4\)
• (B) Adding \(Na_2SO_4\)
• (C) Adding \(HCl\)
• (D) Adding a complexing agent

Correct Answer: (D)

Question 45:

The solubility product \(K_{sp}\) of magnesium hydroxide (Mg(OH)₂) is \(1.8 \times 10^{-11}\). If the concentration of hydroxide ions is fixed at \(1.0 \times 10^{-3}\) M, what is the concentration of \(Mg^{2+}\) ions in the solution?

Options:

• (A) \(1.8 \times 10^{-11}\) M
• (B) \(1.8 \times 10^{-8}\) M
• (C) \(1.8 \times 10^{-5}\) M
• (D) \(1.8 \times 10^{-4}\) M

Correct Answer: (B)

Question 46:

A solution contains \(3.0 \times 10^{-4}\) M \(Pb^{2+}\) and \(1.0 \times 10^{-3}\) M \(Cl^{-}\). The solubility product \(K_{sp}\) of lead(II) chloride (\(PbCl_2\)) is \(1.6 \times 10^{-5}\). Will precipitation occur?

Options:

• (A) Yes, because \(Q > K_{sp}\)
• (B) No, because \(Q < K_{sp}\)
• (C) No, because \(Q = K_{sp}\)
• (D) Yes, because \(Q = K_{sp}\)

Correct Answer: (A)

Question 47:

Which of the following changes would increase the solubility of iron(III) hydroxide (\(Fe(OH)_3\))?

Options:

• (A) Adding \(HCl\)
• (B) Adding \(NaOH\)
• (C) Increasing the concentration of \(Fe^{3+}\)
• (D) Adding \(FeCl_3\)

Correct Answer: (A)

Question 48:

The solubility product \(K_{sp}\) of barium fluoride (\(BaF_2\)) is \(1.0 \times 10^{-6}\). What is the molar solubility of \(BaF_2\) in a solution already containing \(0.1\) M \(F^{-}\)?

Options:

• (A) \(1.0 \times 10^{-6}\) M
• (B) \(1.0 \times 10^{-4}\) M
• (C) \(1.0 \times 10^{-5}\) M
• (D) \(1.0 \times 10^{-3}\) M

Correct Answer: (B)

Question 49:

If the ion product \(Q\) for a solution of calcium phosphate (\(Ca_3(PO_4)_2\)) is \(2.5 \times 10^{-30}\) and the \(K_{sp}\) of calcium phosphate is \(1.3 \times 10^{-29}\), what can be concluded?

Options:

• (A) The solution is unsaturated, and no precipitation will occur
• (B) The solution is saturated, and precipitation will occur
• (C) The solution is supersaturated, and precipitation will occur
• (D) The solution is unsaturated, and precipitation will occur

Correct Answer: (A)

Question 50:

The solubility product \(K_{sp}\) of silver carbonate (\(Ag_2CO_3\)) is \(8.1 \times 10^{-12}\). What is the molar solubility of \(Ag_2CO_3\) in pure water?

Options:

• (A) \(1.3 \times 10^{-4}\) M
• (B) \(9.0 \times 10^{-5}\) M
• (C) \(1.0 \times 10^{-5}\) M
• (D) \(8.1 \times 10^{-6}\) M

Correct Answer: (A)