Q: If the $$K_{sp} of$$ $$\mathrm{AgCl} is$$ $$1.8 \times 10$$^{-10}$$ at 25$$^\circ$$C, what is the molar solubility of $$\mathrm{AgCl}$$ in pure water?

$$1.3 \times 10$$^{-5}$$\ \mathrm{mol/L}$$

Q: A student adds enough $$\mathrm{NaF} to a $$saturated solution of $$\mathrm{$$CaF_2$$} to $$make $$[\mathrm{F^-}] = 0.10\ \mathrm{M}. If$$ $$K_{sp}$$ for $$\mathrm{$$CaF_2$$} is$$ $$4.0 \times 10$$^{-11}$$, what is the new equilibrium concentration of $$\mathrm{$$Ca^{2+}$$}$$?

$$4.0 \times 10$$^{-9}$$\ \mathrm{M}$$

Q: The $$K_{sp}$$ for $$\mathrm{$$PbSO_4$$} is$$ $$6.3 \times 10$$^{-7}$$ at 25$$^\circ$$C. If $$[\mathrm{$$SO_4$$^{2-}}]$$ is increased to 1.0$$\ \mathrm{M}$$ by adding $$\mathrm{$$MgSO_4$$}$$, what is the equilibrium concentration of $$\mathrm{$$Pb^{2+}$$}$$?

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

Q: For the dissolution of $$\mathrm{Ca_3$(PO_4$)_2}$$: $$\mathrm{Ca_3$(PO_4$)_2(s) \rightleftharpoons 3Ca$$^{2+}$$(aq) + 2PO_4$$^{3-}$$(aq)}$$, if $$K_{sp} = 1.0 \times 10$$^{-25}$$, what is the molar solubility s$?

$$s = (1.0 \times 10$$^{-25}$$/108)^{1/5}$

Question 1

Which of the following statements best describes a saturated solution at equilibrium for an ionic solid in water?

Accepted Answer

No more solid can dissolve, and the rates of dissolution and precipitation are equal.

Question 2

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

Accepted Answer

$$K_{sp} = [\mathrm{Ca$$^{2+}$$}][\mathrm{F^-}]^2$$

Question 3

If the $$K_{sp} of$$ $$\mathrm{AgCl} is$$ $$1.8 	imes 10$$^{-10}$$ at 25$$^\circ$$C, what is the molar solubility of $$\mathrm{AgCl}$$ in pure water?

Accepted Answer

$$1.3 	imes 10$$^{-5}$$\ \mathrm{mol/L}$$

Question 4

Which of the following will decrease the solubility of $$\mathrm{AgCl} in $$water?

Accepted Answer

Adding $$\mathrm{NaCl} to $$the solution

Question 5

A student adds enough $$\mathrm{NaF} to a $$saturated solution of $$\mathrm{$$CaF_2$$} to $$make $$[\mathrm{F^-}] = 0.10\ \mathrm{M}. If$$ $$K_{sp}$$ for $$\mathrm{$$CaF_2$$} is$$ $$4.0 	imes 10$$^{-11}$$, what is the new equilibrium concentration of $$\mathrm{$$Ca^{2+}$$}$$?

Accepted Answer

$$4.0 	imes 10$$^{-9}$$\ \mathrm{M}$$

Question 6

Which of the following compounds will have the highest molar solubility in water, given their $$K_{sp}$$ values? $$\mathrm{AgCl}$$ ($$K_{sp} = 1.8 	imes 10$$^{-10}$$), $$\mathrm{AgBr}$$ (K$$_{sp} = 5.0 	imes $$10^{-13}$$), $$\mathrm{AgI}$$ ($$K_{sp} = 8.3 	imes 10$$^{-17}$$)

Accepted Answer

$$\mathrm{AgCl}$$

Question 7

The $$K_{sp}$$ for $$\mathrm{$$PbSO_4$$} is$$ $$6.3 	imes 10$$^{-7}$$ at 25$$^\circ$$C. If $$[\mathrm{$$SO_4$$^{2-}}]$$ is increased to 1.0$$\ \mathrm{M}$$ by adding $$\mathrm{$$MgSO_4$$}$$, what is the equilibrium concentration of $$\mathrm{$$Pb^{2+}$$}$$?

Accepted Answer

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

Question 8

Which of the following best explains the common ion effect?

Accepted Answer

The solubility of a salt decreases when a solution already contains one of its ions.

Question 9

For the dissolution of $$\mathrm{Ca_3$(PO_4$)_2}$$: $$\mathrm{Ca_3$(PO_4$)_2(s) ightleftharpoons 3Ca$$^{2+}$$(aq) + 2PO_4$$^{3-}$$(aq)}$$, if $$K_{sp} = 1.0 	imes 10$$^{-25}$$, what is the molar solubility s$?

Accepted Answer

$$s = (1.0 	imes 10$$^{-25}$$/108)^{1/5}$

Question 10

A saturated solution of $$\mathrm{$$BaSO_4$$} is $$prepared. Which of the following will NOT appear in the equilibrium expression for $$K_{sp}$$?

Accepted Answer

$$[\mathrm{$$BaSO_4$$(s)}]$$

Question 11

Which of the following changes will increase the solubility of $$\mathrm{Mg(OH)_2} in $$water?

Accepted Answer

Decreasing the pH of the solution

Question 12

If $$K_{sp}$$ for $$\mathrm{Ag_2CO_3} is$$ $$8.1 	imes 10$$^{-12}$$, what is the molar solubility s$ of $$\mathrm{Ag_2CO_3}$$?

Accepted Answer

$$s = (K_{sp}/4$$)^{1/3}$$

Question 13

A solution contains $$[\mathrm{Ag^+}] = 1.0 	imes 10$$^{-5}$$\ \mathrm{M}$$ and $$[\mathrm{Cl^-}] = 1.0 	imes 10$$^{-5}$$\ \mathrm{M}. If$$ $$K_{sp}$$ for $$\mathrm{AgCl} is$$ $$1.8 	imes 10$$^{-10}$$, what will happen?

Accepted Answer

The solution is saturated and no change will occur.

Question 14

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

Accepted Answer

Solubility is the amount that dissolves (g/L or mol/L), while $$K_{sp} is $$the equilibrium constant for the dissolution reaction.

Question 15

Which of the following factors does NOT affect the value of $$K_{sp}$$ for a given salt?

Accepted Answer

The presence of a common ion

Question 16

A patient is treated for lead poisoning. To reduce $$\mathrm{Pb$$^{2+}$$} in $$the blood, a doctor administers a solution containing $$\mathrm{SO_4$^{2-}}. $$What is the chemical principle behind this treatment?

Accepted Answer

The addition of $$\mathrm{SO_4$^{2-}}$$ causes $$\mathrm{$$PbSO_4$$} to $$precipitate, lowering $$\mathrm{Pb$$^{2+}$$}$$ concentration via the common ion effect.

Question 17

Which of the following is true about the dissolution of $$\mathrm{$$BaSO_4$$} in $$water?

Accepted Answer

At equilibrium, the rate of dissolution equals the rate of precipitation.

Question 18

A chemist wants to increase the solubility of $$\mathrm{Fe(OH)_3} in $$water. Which of the following would be most effective?

Accepted Answer

Adding acid to lower the pH

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

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