Determine the $\mathrm{pH}$ for the following solutions:

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

One day in a laboratory, some water spilled on a table. In just a few minutes the water had evaporated. Some days later, a similar amount of water spilled again. This time, the water remained on the table after 7 or 8 hours. Name three conditions that could have changed in the lab to cause this difference.

Under certain circumstances, when oxygen gas is heated, it can be converted into ozone according to the following reaction equation:

$$3 \mathrm{O}_2(g)+\text { heat } \rightleftharpoons 2 \mathrm{~O}_3(g)$$

Name three different ways that you could increase the production of the ozone.

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?

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 $\mathrm{BaF}_2$ ?

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) $2.0 \times 10^{-6}~M\mathrm{~KOH}$

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

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) $2 \mathrm{~NO}(\mathrm{g})+2 \mathrm{~H}_2(\mathrm{~g}) \rightleftharpoons \mathrm{N}_2(\mathrm{~g})+2 \mathrm{~H}_2 \mathrm{O}(\mathrm{g})+665 \mathrm{~kJ}$

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 $\left.\mathrm{BaSO}_4\right)$