Chapter 10, Problem 89E

What mass in grams of magnesium nitrate, $\text{Mg}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}$, must be used to precipitate as magnesium hydroxide all of the hydroxide ion in $\text{50}\text{.0}\text{ml}$ of $17.0\%$ by mass $\text{NaOH}$, the density of which is $\text{1}\text{.19}\text{g}/\text{mL}$? The precipitation reaction is $\text{2NaOH}+\text{Mg}{\left({\text{NO}}_{\text{3}}\right)}_{\text{2}}\to \text{Mg}{\left(\text{OH}\right)}_{\text{2}}+{\text{2NaNO}}_{\text{3}}$.