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

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

Q: The $K_{sp}$ for $CaF_2$ is $3.9 \times 10^{-11}$. What is the molar solubility of $CaF_2$ in pure water?

$2.1 \times 10^{-4}\ \mathrm{mol/L}$

Q: If the initial concentrations of $Ag^+$ and $Cl^-$ in a solution are such that $Q = [Ag^+][Cl^-] < K_{sp}$ for $AgCl$, what will happen?

No precipitate will form and more $AgCl$ can dissolve.

Q: Which of the following best explains why $Mg(OH)_2$ is more soluble in acidic solution?

Acid reacts with $OH^-$, shifting the equilibrium to dissolve more $Mg(OH)_2$.

Q: A student adds $0.010\ \mathrm{M}$ NaF to a saturated solution of $CaF_2$. What happens to the solubility of $CaF_2$?

The solubility of $CaF_2$ decreases due to the common ion effect.

Q: A solution contains $[Ag^+] = 1.0 \times 10^{-5}\ \mathrm{M}$ and $[Cl^-] = 2.0 \times 10^{-5}\ \mathrm{M}$. $K_{sp}$ for $AgCl$ is $1.6 \times 10^{-10}$. Will a precipitate form?

Yes, because $Q = 2.0 \times 10^{-10} > K_{sp}$

Question 1

Which of the following is the correct solubility product ($K_{sp}$) expression for $Ca_3(PO_4)_2$?

Accepted Answer

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

Question 2

A saturated solution of $CaSO_4$ has a solubility of 0.67 g/L. The molar mass of $CaSO_4$ is 136 g/mol. What is the value of $K_{sp}$ for $CaSO_4$?

Accepted Answer

$K_{sp} = 2.4 	imes 10^{-5}$

Question 3

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

Accepted Answer

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

Question 4

Which of the following best describes the effect of adding NaBr to a saturated solution of $AgBr$?

Accepted Answer

The solubility of $AgBr$ decreases due to the common ion effect.

Question 5

Which of the following compounds will be more soluble in acidic solution than in pure water?

Accepted Answer

$CaCO_3$

Question 6

A solution is prepared by mixing 0.050 L of $2.0 	imes 10^{-2}\ \mathrm{M}$ NaF with 0.010 L of $1.0 	imes 10^{-2}\ \mathrm{M}$ $Ca(NO_3)_2$. $K_{sp}$ for $CaF_2$ is $3.9 	imes 10^{-11}$. Will a precipitate of $CaF_2$ form?

Accepted Answer

Yes, because $Q > K_{sp}$

Question 7

What is the $K_{sp}$ expression for $Ag_2CO_3$?

Accepted Answer

$K_{sp} = [Ag^+]^2[CO_3^{2-}]$

Question 8

The $K_{sp}$ for $CaF_2$ is $3.9 	imes 10^{-11}$. What is the molar solubility of $CaF_2$ in pure water?

Accepted Answer

$2.1 	imes 10^{-4}\ \mathrm{mol/L}$

Question 9

Which of the following statements about $K_{sp}$ is correct?

Accepted Answer

$K_{sp}$ is constant for a given salt at a given temperature.

Question 10

Which of the following will NOT affect the solubility of $AgCl$ in water?

Accepted Answer

Adding $NaNO_3$

Question 11

If the initial concentrations of $Ag^+$ and $Cl^-$ in a solution are such that $Q = [Ag^+][Cl^-] < K_{sp}$ for $AgCl$, what will happen?

Accepted Answer

No precipitate will form and more $AgCl$ can dissolve.

Question 12

Which of the following best explains why $Mg(OH)_2$ is more soluble in acidic solution?

Accepted Answer

Acid reacts with $OH^-$, shifting the equilibrium to dissolve more $Mg(OH)_2$.

Question 13

A student adds $0.010\ \mathrm{M}$ NaF to a saturated solution of $CaF_2$. What happens to the solubility of $CaF_2$?

Accepted Answer

The solubility of $CaF_2$ decreases due to the common ion effect.

Question 14

Which of the following salts will have its solubility unaffected by a change in pH?

Accepted Answer

$NaCl$

Question 15

A solution contains $[Ag^+] = 1.0 	imes 10^{-5}\ \mathrm{M}$ and $[Cl^-] = 2.0 	imes 10^{-5}\ \mathrm{M}$. $K_{sp}$ for $AgCl$ is $1.6 	imes 10^{-10}$. Will a precipitate form?

Accepted Answer

Yes, because $Q = 2.0 	imes 10^{-10} > K_{sp}$

Question 16

Which of the following best describes the relationship between $K_{sp}$ and molar solubility for a salt $MX_2$?

Accepted Answer

$K_{sp} = 4s^3$, where $s$ is the molar solubility

Question 17

Which of the following is a correct real-life application of precipitation reactions?

Accepted Answer

Water softening by removing $Ca^{2+}$ and $Mg^{2+}$ ions as insoluble salts

Solubility and Solubility Equilibria (General Chemistry Study Notes)

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