Describe how the solubilities of the hydroxides of magnesium, calcium and strontium change. Explain your answer. Put them in order from most soluble to least soluble.
Suggest how the pH of saturated solutions of the hydroxides of magnesium, calcium and strontium varies. 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 a pH of $12.2$ is prepared by dissolving $\text{Ba(OH)}_2$ in distilled water. Calculate the mass of $\text{Ba(OH)}_2$ required to make this solution. Show your working. $[M_r\!:\,\text{Ba(OH)}_2 = 171.3]$
The solubility of iron(II) hydroxide, $\text{Fe(OH)}_2$, is $5.85 \times 10^{-6}\,\text{mol dm}^{-3}$ at $298\,\text{K}$. Write the expression for the solubility product, $K_{sp}$, of $\text{Fe(OH)}_2$.
Calculate the value of $K_{sp}$ of $\text{Fe(OH)}_2$. Include its units.