Approximately $0.14 \mathrm{~g}$ of nickel(II) hydroxide, $\mathrm{Ni}(\mathrm{OH})_2(s)$, dissolves per liter of water at $20^{\circ} \mathrm{C}$. Calculate the $K_{s p}$ for $\mathrm{Ni}(\mathrm{OH})_2(s)$ at this temperature.

A solution of hydrofluoric acid, HF, has a $\mathrm{pH}$ of $2.30$. Calculate the equilibrium concentrations of $\mathrm{HF}^2 \mathrm{~F}^{-}$, and $\mathrm{H}_9 \mathrm{O}^{+}$, and calculate the amount of HF originally dissolved per liter.

How much water must Poison Ivy add to a $4$-liter solution that contains $5 \%$ extract of baneberry to get a solution that contains $3 \%$ extract of baneberry?

Using what you know from these meaningful parts, answer the following question:

Do you think a kiloliter has more or less liquid than a liter?

Calculate the solubility in grams per liter of silver sulfate, $\mathrm{Ag}_2 \mathrm{SO}_4(s)$, in a $0.55-\mathrm{M}$ silver nitrate, $\mathrm{AgNO}_3(a q)$, solution at $25^{\circ} \mathrm{C}$.

Calculate the pH at 25 degree Celsius of a solution that is prepared by dissolving 25.0 grams of barium acetate, $\mathrm{Ba}\left(\mathrm{CH}_3 \mathrm{COO}\right)_2(s)$, in enough water to make exactly 1.00 liter of solution.

Calculate the hydrogen ion concentration, in moles per liter, for solutions with each of the following $\mathrm{pOH}$ values. a. $\mathrm{POH}=3.91$ b. $\mathrm{pOH}=12.56$ c. $\mathrm{POH}=1.15$ d. $\mathrm{pOH}=8.77$

A bottle of soda contains 360 ml. (a) How many mililiters are contained in a six-bottle carton? (b) How many liters does the amount in part (a) equal? (c) At $2.45 for the carton of soda, what is its cost per liter?

Calculate the solubility in grams per liter of $\mathrm{Pb}\left(\mathrm{IO}_3\right)_2(s)$ in $0.10 \mathrm{M} \mathrm{KIO}_3(a q)$ at $25^{\circ} \mathrm{C}$.

Using what you know from these meaningful parts, answer the following question:

Do you think a milliliter has more or less liquid than a liter?

A water molecule has mass $3.0 \times 10^{-26} \mathrm{~kg}$. How many molecules are in 1 liter $\left(1000 \mathrm{~cm}^3\right)$ of water?

The solubility-product constant for $\mathrm{Mg}(\mathrm{OH})_2(s)$ in equilibrium with water at $25^{\circ} \mathrm{C}$ is $5.6 \times 10^{-12} \mathrm{M}^3$. Calculate the solubility in grams per liter of $\mathrm{Mg}(\mathrm{OH})_2(s)$ in water at $25^{\circ} \mathrm{C}$.

Calculate the solubility in grams per liter of $\mathrm{Ag}_2 \mathrm{SO}_4(s)$ in $0.15 \mathrm{M} \mathrm{K}_2 \mathrm{SO}_4(a q)$ at $25^{\circ} \mathrm{C}$.

Calculate the solubility of $\mathrm{Mg}(\mathrm{OH})_2(s)$ in grams per liter in an aqueous solution buffered at $\mathrm{pH}=8.50$ at $25^{\circ} \mathrm{C}$.