The solubility of $\mathrm{Hg}_2 \mathrm{I}_2$ in $\mathrm{H}_2 \mathrm{O}$ is $3.04 \times 10^{-7} \mathrm{~g} / \mathrm{L}$. The reaction $\mathrm{Hg}_2 \mathrm{I}_2 \rightleftharpoons \mathrm{Hg}_2^{2+}+2 \mathrm{~I}^{-}$represents the equilibrium. Calculate the $K_{\text {sp }}$.

The $K_{s p}$ of $\mathrm{SrSO}_4$ is $7.6 \times 10^{-7}$. Should precipitation occur when $25.0 \mathrm{~mL}$ of $1.0 \times 10^{-3} \mathrm{M} \mathrm{SrCl}_2$ solution are mixed with $15.0 \mathrm{~mL}$ of $2.0 \times 10^{-3}~M\mathrm{~Na}_2 \mathrm{SO}_4$ ? Show proof.

The $K_{\text {eq }}$ for the formation of ammonia gas from its elements is 4.0. If the equilibrium concentrations of nitrogen gas and hydrogen gas are both $2.0~M$, what is the equilibrium concentration of the ammonia gas?

Of the acids listed in Table 16.2, which ones are stronger than acetic acid and which are weaker?

If it takes $0.048 \mathrm{~g} \mathrm{~BaF}_2$ to saturate $15.0 \mathrm{~mL}$ of water, what is the $K_{s p}$ of $\mathrm{BaF}_2$ ?

For the following equations, tell in which direction, left or right, the equilibrium will shift when these changes are made: The temperature is increased, the pressure is increased by decreasing the volume of the reaction vessel, and a catalyst is added.

(a) $3\mathrm{~O}_2(\mathrm{~g})+271 \mathrm{~kJ} \rightleftharpoons 2 \mathrm{~O}_3(\mathrm{~g})$
(b) $\mathrm{CH}_4(\mathrm{~g})+\mathrm{Cl}_2(\mathrm{~g}) \rightleftharpoons \mathrm{CH}_3 \mathrm{Cl}(\mathrm{g})+\mathrm{HCl}(\mathrm{g})+110 \mathrm{~kJ}$
(c) $2 \mathrm{~NO}(\mathrm{g})+2 \mathrm{~H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{N}_2(\mathrm{~g})+2 \mathrm{~H}_2 \mathrm{O}(\mathrm{g})+665 \mathrm{~kJ}$

Calculate the $K_{\mathrm{eq}}$ for the reaction

$$\mathrm{SO}_2(g)+\mathrm{O}_2(g) \rightleftharpoons \mathrm{SO}_3(g)$$

when the equilibrium concentrations of the gases at $530^{\circ} \mathrm{C}$ are $\left[\mathrm{SO}_3\right]=11.0~M,\left[\mathrm{SO}_2\right]=4.20~M$, and $\left[\mathrm{O}_2\right]=$ $0.60 \times 10^{-3}~M$

Suppose the concentration of a solution is $0.10 ~M\mathrm{~Ba}^{2+}$ and $0.10~M\mathrm{~Sr}^{2+}$. Which sulfate, $\mathrm{BaSO}_4$ or $\mathrm{SrSO}_4$, will precipitate first when a dilute solution of $\mathrm{H}_2 \mathrm{SO}_4$ is added dropwise to the solution? Show evidence for your answer. ( $K_{\text {sp }}=1.5 \times 10^{-9}$ for $\mathrm{BaSO}_4$ and $K_{\text {sp }}=3.5 \times 10^{-7}$ for $\mathrm{SrSO}_4$ )

The $K_{\text {sp }}$ for $\mathrm{PbCl}_2$ is $2.0 \times 10^{-5}$. Will a precipitate form when $0.050 \mathrm{~mol} \mathrm{~Pb}\left(\mathrm{NO}_3\right)_2$ and $0.010 \mathrm{~mol} \mathrm{~NaCl}$ are in $1.0 \mathrm{~L}$ solution? Show evidence for your answer.

Determine the $\left[\mathrm{H}^{+}\right]$and $\left[\mathrm{OH}^{-}\right]$in

(a) $5.0 \times 10^{-5}~M\mathrm{~HNO}_3$
(b) $2.0 \times 10^{-6}~M\mathrm{~KOH}$

If $\mathrm{BaCl}_2$ is added to a saturated $\mathrm{BaSO}_4$ solution until the $\left[\mathrm{Ba}^{2+}\right]$ is $0.050~M$,

(a) what concentration of $\mathrm{SO}_4^{2-}$ remains in solution?
(b) how much $\mathrm{BaSO}_4$ remains dissolved in $100 .\mathrm{~mL}$ of the solution? $\left(K_{\text {sp }}=1.5 \times 10^{-9}\right.$ for $\left.\mathrm{BaSO}_4\right)$

Calculate whether or not a precipitate will form in the following mixed solutions:

(a) $100 \mathrm{~mL}$ of $0.010~M\mathrm{~Na}_2 \mathrm{SO}_4$ and $100 \mathrm{~mL}$ of $0.001~M\mathrm{~Pb}\left(\mathrm{NO}_3\right)_2$
(b) $50.0 \mathrm{~mL}$ of $1.0 \times 10^{-4}~M\mathrm{~AgNO}_3$ and $100 . \mathrm{mL}$ of $1.0 \times 10^{-4}~M\mathrm{~NaCl}$
(c) $1.0 \mathrm{~g} \mathrm{~Ca}\left(\mathrm{NO}_3\right)_2$ in $150 \mathrm{~mL} \mathrm{~H}_2 \mathrm{O}$ and $250 \mathrm{~mL}$ of $0.01~M\mathrm{~NaOH}$\

$$K_{\text {sp }} \mathrm{PbSO}_4=1.3 \times 10^{-8}$$

$$K_{\mathrm{sp}} \mathrm{AgCl}=1.7 \times 10^{-10}$$

$$K_{\mathrm{sp}} \mathrm{Ca}(\mathrm{OH})_2=1.3 \times 10^{-6}$$

The $K_{s p}$ of $\mathrm{CaF}_2$ is $3.9 \times 10^{-11}$. Calculate (a) the molar concentrations of $\mathrm{Ca}^{2+}$ and $\mathrm{F}^{-}$in a saturated solution and (b) the grams of $\mathrm{CaF}_2$ that will dissolve in $500 . \mathrm{mL}$ of water.

Solutions of $50.0 \mathrm{~mL}$ of $0.10~M\mathrm{~BaCl}_2$ and $50.0 \mathrm{~mL}$ of $0.15~M\mathrm{~Na}_2 \mathrm{CrO}_4$ are mixed, forming a precipitate of $\mathrm{BaCrO}_4$. Calculate the concentration of $\mathrm{Ba}^{2+}$ that remains in solution.