Write an expression for the solubility product, $K_{sp}$, of $\text{Ag}_2\text{S(s)}$.
At $298\,\text{K}$, the solubility of $\text{Ag}_2\text{S(s)}$ in water is $1.16 \times 10^{-17}\,\text{mol dm}^{-3}$. Calculate the numerical value of the solubility product, $K_{sp}$, of $\text{Ag}_2\text{S(s)}$ at $298\,\text{K}$.
Calculate the minimum volume of water required to dissolve $1.00\,\text{g}$ of $\text{Ag}_2\text{S(s)}$ under standard conditions.
Bromic(I) acid, $\text{HOBr(aq)}$, behaves as a weak acid. Its $K_a$ is $2.0 \times 10^{-9}\,\text{mol dm}^{-3}$. Calculate the pH of $0.20\,\text{mol dm}^{-3}\,\text{HOBr(aq)}$.
$5.0\,\text{cm}^3$ of $0.20\,\text{mol dm}^{-3}$ potassium hydroxide, $\text{KOH}$, are mixed with $20.0\,\text{cm}^3$ of $0.20\,\text{mol dm}^{-3}\,\text{HOBr(aq)}$. Calculate the pH of the buffer solution formed.