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 ($K_{sp}=1.8	imes10^{-10}$), AgBr ($K_{sp}=5.0	imes10^{-13}$), or AgI ($K_{sp}=8.3	imes10^{-17}$)?

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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