Describe and explain how the solubilities of the sulfates of the Group II elements change down the group.
Use the data above to determine values of $\u0006H^\u000b_\text{solution}$ for $\text{Mg(OH)}_2$ and for $\text{Sr(OH)}_2$.
Use your results in (i) to suggest whether $\text{Sr(OH)}_2$ is more or less soluble in water than $\text{Mg(OH)}_2$. State any assumptions you make.
Suggest whether $\text{Sr(OH)}_2$ would be more or less soluble in hot water than in cold water. Explain your answer.
The table below gives some enthalpy changes for magnesium and strontium compounds.
Calcium hydroxide, $\text{Ca(OH)}_2$, has only slight solubility in water.
Write an expression for $K_{sp}$ for calcium hydroxide, and state its units.
A $25.0\,\text{cm}^3$ portion of a saturated solution of $\text{Ca(OH)}_2$ needed $21.0\,\text{cm}^3$ of $0.0500\,\text{mol dm}^{-3}$ $\text{HCl}$ for complete neutralisation. Calculate $[\text{OH}^-(aq)]$ and $[\text{Ca}^{2+}(aq)]$ in the saturated solution, and hence determine a value for $K_{sp}$.
Compare the solubility of $\text{Ca(OH)}_2$ in $0.1\,\text{mol dm}^{-3}$ $\text{NaOH}$ with its solubility in water. Explain your answer.