Module 5.4 Solution Equilibria

Which of the following metal carbonates has the highest molar solubility?

• Calcium carbonate

• Copper(II) carbonate

• Iron(II) carbonate

• Lead(II) carbonate

Consider the following equilibrium.

HF(aq) + CF₃COO⁻(aq) ↔ F⁻(aq) + CF₃COOH(aq) Keq = 3.80 × 10⁻⁴

Which of the following correctly identifies the strongest acid and the strongest base in this system?

• Strongest acid: CF₃COOH(aq), strongest base: F⁻(aq)

• Strongest acid: CF₃COOH(aq), strongest base: CF₃COO⁻(aq)

• Strongest acid: HF(aq), strongest base: F⁻(aq)

• Strongest acid: HF(aq), strongest base: CF₃COO⁻(aq)

Equal volumes of two 0.04 mol L⁻¹ solutions were mixed together.

Which pair of solutions would give the greatest mass of precipitate?

• Ba(OH)₂ and MgCl₂

• Ba(OH)₂ and MgSO₄

• Ba(OH)₂ and NaCl

• Ba(OH)₂ and Na₂SO₄

The following apparatus was set up in a temperature-controlled laboratory.

Excess solid sodium hydroxide is added to the beaker.

Which of the following correctly identifies the change in the CuSO₄(s) mass and the colour of the solution after several days?

• No change in CuSO₄ mass, no change in colour

• No change in CuSO₄ mass, blue colour fades

• CuSO₄ mass decreases, blue colour intensifies

• CuSO₄ mass decreases, blue colour fades

The graph shows the concentration of silver and chromate ions which can exist in a saturated solution of silver chromate.

Based on the information provided, what is the Ksp for silver chromate?

• 1.1 × 10⁻⁸

• 2.2 × 10⁻⁸

• 1.1 × 10⁻¹²

• 4.4 × 10⁻¹²

A 2.0 g sample of silver carbonate (MM = 275.81 g mol⁻¹) was added to 100.0 mL of water in a beaker. The solubility of silver carbonate at this temperature is 1.2 × 10⁻⁴ mol L⁻¹. It was then diluted by adding another 100.0 mL of water.

What is the ratio of the concentration of silver ions in solution before and after dilution?

• 1 : 1

• 1 : 2

• 2 : 1

• 4 : 1

What is the molar solubility of iron(II) hydroxide?

• 2.3 × 10⁻⁶ mol L⁻¹

• 2.9 × 10⁻⁶ mol L⁻¹

• 3.7 × 10⁻⁶ mol L⁻¹

• 4.9 × 10⁻⁹ mol L⁻¹

Sodium chloride dissolves in water according to the following equation.

NaCl(s) ↔ Na⁺(aq) + Cl⁻(aq)

A saturated solution of NaCl in water contains sodium and chloride ions at the concentrations pictured in the table.

What is the Ksp of sodium chloride?

• 2.65 × 10⁻²

• 8.16 × 10⁻²

• 12.26

• 37.6

What mass of lead(II) iodide (MM = 461 g mol⁻¹) will dissolve in 375 mL of water?

• 0.233 g

• 0.293 g

• 0.369 g

• 0.621 g

What will happen when sulfuric acid is added to a saturated solution of sparingly soluble calcium sulfate?

• The concentration of calcium and sulfate ions will increase over time due to the presence of H⁺ ions.

• The concentration of calcium and sulfate ions will decrease over time due to the presence of H⁺ ions.

• The concentration of calcium and sulfate ions will increase over time due to the presence of SO₄^2– ions.

• The concentration of calcium and sulfate ions will decrease over time due to the presence of SO₄^2– ions.