Q: If the $$K_{sp} of $$AgCl is $$1.6 \times 10$$^{-10}$$, what is the molar solubility of AgCl in pure water?

$$1.3 \times 10$$^{-5}$$\ \mathrm{M}$$

Q: For the reaction $$\mathrm{$$BaSO_4$$(s) \rightleftharpoons Ba$$^{2+}$$(aq) + SO_4$^{2-}(aq)}$$, if the $$K_{sp} is$$ $$1.1 \times 10$$^{-10}$$, what is the equilibrium concentration of $$\mathrm{$$Ba^{2+}$$}$$ in pure water?

$$1.05 \times 10$$^{-5}$$\ \mathrm{M}$$

Q: If the $$K_{sp}$$ for Ag\_2CO\_3 is $$8.1 \times 10$$^{-12}$$, what is the molar solubility of Ag\_2CO\_3 in pure water?

$$1.27 \times 10$$^{-4}$$\ \mathrm{M}$$

Q: A student mixes excess PbSO\_4(s) with water and adds enough MgSO\_4 to make the SO\_$$4^{2-}$$ concentration 1.0 M. If $$K_{sp}$$ for PbSO\_4 is $$6.3 \times 10$$^{-7}$$, what is the equilibrium concentration of Pb$$^{2+}$$?

$$6.3 \times 10$$^{-7}$$\ \mathrm{M}$$

Q: If the solubility of Ca\_3(PO\_4)\_2 is $$3.92 \times 10$$^{-5}$$ M, what is the concentration of Ca$$^{2+}$$ ions in a saturated solution?

$$1.18 \times 10$$^{-4}$$\ \mathrm{M}$$

Question 1

Which of the following statements best describes a solubility equilibrium?

Accepted Answer

It is a heterogeneous reaction involving the dissolution and precipitation of ionic compounds.

Question 2

Which of the following salts is always soluble in water?

Accepted Answer

NH\_4Cl

Question 3

Given the dissolution reaction $$\mathrm{Ca_3$(PO_4$)_2(s) \rightleftharpoons 3\ Ca$$^{2+}$$(aq) + 2\ PO_4$^{3-}(aq)}$$, which is the correct expression for the solubility product constant $$K_{sp}$$?

Accepted Answer

$$K_{sp} = [Ca$$^{2+}$$]^3[PO_4$^{3-}]^2$$

Question 4

If the $$K_{sp} of $$AgCl is $$1.6 	imes 10$$^{-10}$$, what is the molar solubility of AgCl in pure water?

Accepted Answer

$$1.3 	imes 10$$^{-5}$$\ \mathrm{M}$$

Question 5

Which factor does NOT affect the solubility of a salt in water?

Accepted Answer

The color of the salt

Question 6

A saturated solution of Mg(OH)\_2 is in equilibrium. What happens to the solubility of Mg(OH)\_2 if NaOH is added to the solution?

Accepted Answer

The solubility decreases due to the common ion effect.

Question 7

For the reaction $$\mathrm{$$BaSO_4$$(s) ightleftharpoons Ba$$^{2+}$$(aq) + SO_4$^{2-}(aq)}$$, if the $$K_{sp} is$$ $$1.1 	imes 10$$^{-10}$$, what is the equilibrium concentration of $$\mathrm{$$Ba^{2+}$$}$$ in pure water?

Accepted Answer

$$1.05 	imes 10$$^{-5}$$\ \mathrm{M}$$

Question 8

Which of the following best explains the common ion effect?

Accepted Answer

Adding a common ion decreases the solubility of a salt by shifting the equilibrium toward the solid.

Question 9

If the $$K_{sp}$$ for Ag\_2CO\_3 is $$8.1 	imes 10$$^{-12}$$, what is the molar solubility of Ag\_2CO\_3 in pure water?

Accepted Answer

$$1.27 	imes 10$$^{-4}$$\ \mathrm{M}$$

Question 10

A student mixes excess PbSO\_4(s) with water and adds enough MgSO\_4 to make the SO\_$$4^{2-}$$ concentration 1.0 M. If $$K_{sp}$$ for PbSO\_4 is $$6.3 	imes 10$$^{-7}$$, what is the equilibrium concentration of Pb$$^{2+}$$?

Accepted Answer

$$6.3 	imes 10$$^{-7}$$\ \mathrm{M}$$

Question 11

Which compound will produce the highest concentration of $$Ag^{+}$$ ions in a saturated solution: AgCl ($$K_{sp}=1.8\$$times10^{-10}$$), AgBr (K$$_{sp}=5.0\$$times10^{-13}$$), or AgI ($$K_{sp}=8.3\$$times10^{-17}$$)?

Accepted Answer

AgCl

Question 12

Which of the following is the correct $$K_{sp}$$ expression for the dissolution of SrF\_2(s)?

Accepted Answer

$$K_{sp} = [Sr$$^{2+}$$][F^-]^2$$

Question 13

If the solubility of Ca\_3(PO\_4)\_2 is $$3.92 	imes 10$$^{-5}$$ M, what is the concentration of Ca$$^{2+}$$ ions in a saturated solution?

Accepted Answer

$$1.18 	imes 10$$^{-4}$$\ \mathrm{M}$$

Question 14

Which of the following best describes the difference between solubility and $$K_{sp}$$?

Accepted Answer

Solubility is the amount of solute that dissolves to form a saturated solution, while $$K_{sp} is $$the equilibrium constant for the dissolution reaction.

Question 15

A solution is saturated with respect to Mg(OH)\_2. Which of the following must be true?

Accepted Answer

Both solid Mg(OH)\_2 and its ions are present, with dissolution and precipitation occurring at equal rates.

Question 16

If the $$K_{sp}$$ for CaF\_2 is $$4.0 	imes 10$$^{-11}$$, what is the molar solubility of CaF\_2 in pure water?

Accepted Answer

$$1.0 	imes 10$$^{-4}$$\ \mathrm{M}$$

Question 17

Which of the following will increase the solubility of a salt whose anion is a weak base?

Accepted Answer

Decreasing the pH of the solution

Question 18

Which of the following is true about the $$K_{sp}$$ value for a given salt?

Accepted Answer

It is constant for a given salt at a specific temperature.

Solubility Equilibria and the Solubility Product Constant ($K_{sp}$)

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