Question 1

Which property of barium sulfate makes it suitable for use in X-ray imaging of the digestive tract, as shown in the first image?

Accepted Answer

Its low solubility in water prevents toxicity and allows it to block X-rays.

Question 2

A saturated solution of silver iodide, AgI(s), is in equilibrium with its ions. Which equation correctly represents the solubility product constant for this equilibrium?

Accepted Answer

$$K_{sp} = [Ag^+(aq)] \cdot [I^-(aq)]$$

Question 3

Which of the following best describes a solubility equilibrium?

Accepted Answer

A dynamic equilibrium between a solute and solvent in a saturated solution.

Question 4

Given the dissolution equilibrium $$CaF_2(s$$) \rightleftharpoons $$Ca^{2+}(aq) + 2F^-(aq$$)$$, what is the correct expression for the solubility product constant?

Accepted Answer

$$K_{sp} = [Ca$$^{2+}$$(aq)] \cdot [F^-(aq)]^2$$

Question 5

A chemist mixes 100.0 mL of 0.0500 mol/L lead(II) nitrate with 200.0 mL of 0.100 mol/L sodium iodide. Will a precipitate of lead(II) iodide, PbI2(s), form? (Assume $$K_{sp}$$ for PbI2 is $$1.4 	imes 10$$^{-8}$$.)

Accepted Answer

Yes, because the ion product $$Q is $$greater than $$K_{sp}.$$

Question 6

What is the effect of adding sodium chloride to a saturated solution of silver chloride, AgCl(s)?

Accepted Answer

The solubility of AgCl decreases due to the common ion effect.

Question 7

Which equation would you use to calculate the trial ion product, $$Q$$, for the dissolution of magnesium hydroxide, Mg(OH)2(s), in water?

Accepted Answer

$$Q = [Mg$$^{2+}$$(aq)] \cdot [OH^-(aq)]^2$$

Question 8

If the trial ion product $$Q$$ for a solution is less than the solubility product constant $$K_{sp}$$, what will happen?

Accepted Answer

No precipitate will form; more solid can dissolve.

Question 9

Which of the following best explains the formation of stalactites and stalagmites in limestone caves, as shown in the third image?

Accepted Answer

They form due to the precipitation of calcium carbonate from water as a result of solubility equilibrium.

Question 10

A solution contains 0.01 mol/L calcium nitrate and 0.025 mol/L sodium phosphate. Will a precipitate form, and if so, which compound is likely to precipitate?

Accepted Answer

A precipitate of calcium phosphate, Ca3(PO4)2(s), will form.

Question 11

Which statement correctly describes the relationship between molar solubility and the solubility product constant ($$K_{sp}$$)?

Accepted Answer

Molar solubility is the maximum amount of solute that dissolves, while $$K_{sp} is $$the equilibrium constant for the solubility equilibrium.

Question 12

A student mixes 250.0 mL of 0.0025 mol/L calcium chloride with 300.0 mL of 0.0015 mol/L potassium hydroxide. Will a precipitate of calcium hydroxide, Ca(OH)2(s), form?

Accepted Answer

Yes, if the ion product $$Q$$ exceeds the $$K_{sp}$$ for Ca(OH)2.

Question 13

Which of the following is a correct application of Le Châtelier’s principle to a solubility equilibrium?

Accepted Answer

Adding a common ion shifts the equilibrium toward the solid, decreasing solubility.

Question 14

Which compound is less soluble in water: AgCl(s) with $$K_{sp} = 1.8 	imes 10$$^{-10}$$ or AgBr(s) with K$$_{sp} = 5.0 	imes $$10^{-13}$$?

Accepted Answer

AgBr(s) is less soluble because its $$K_{sp} is $$smaller.

Question 15

What is the effect of temperature on the solubility product constant ($$K_{sp}$$)?

Accepted Answer

$$K_{sp}$$ varies with temperature because solubility changes with temperature.

Question 16

Which of the following best describes the common ion effect?

Accepted Answer

The solubility of an ionic compound decreases when a common ion is added.

Question 17

A solution contains 0.015 mol/L copper(I) nitrate and 0.075 mol/L potassium iodide. Will a precipitate of copper(I) iodide, CuI(s), form if $$K_{sp}$$ for CuI is $$1.1 	imes 10$$^{-12}$$?

Accepted Answer

Yes, because the ion product $$Q is $$greater than $$K_{sp}.$$

Question 18

Which equation would you use to calculate the molar solubility of copper(II) iodate, Cu(IO3)2(s), given $$K_{sp}$$?

Accepted Answer

$$K_{sp} = [Cu$$^{2+}$$(aq)] \cdot [IO_3$^-(aq)]^2$$

Lesson 7.6-7.7: Solubility Equilibria and the Solubility Product Constant (Ksp) (12 Chem)

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