Describe how the solubility of the hydroxides of magnesium, calcium and strontium varies. Explain your answer. Arrange them from most soluble to least soluble.
Suggest how the pH of saturated solutions of the hydroxides of magnesium, calcium and strontium changes. Explain your answer.
Barium hydroxide, $\text{Ba(OH)}_2$, is a strong base. A $250.0\,\text{cm}^3$ solution of $\text{Ba(OH)}_2$ with pH $12.2$ is prepared by dissolving $\text{Ba(OH)}_2$ in distilled water. Calculate the mass of $\text{Ba(OH)}_2$ needed to prepare this solution. Show your working. [$M_r$ of $\text{Ba(OH)}_2 = 171.3$]
At $298\,\text{K}$, the solubility of iron(II) hydroxide, $\text{Fe(OH)}_2$, is $5.85 \times 10^{-6}\,\text{mol dm}^{-3}$. Write the expression for the solubility product, $K_{sp}$, of $\text{Fe(OH)}_2$.
Calculate the value of $K_{sp}$ for $\text{Fe(OH)}_2$. State its units.