(Solved): Why does the addition of acid increase the solubility of calcium phosphate? View Available Hint(s) ...

Why does the addition of acid increase the solubility of calcium phosphate? View Available Hint(s) It decreases the phosphate ion concentration, forcing the equilibrium to the right. It increases the phosphate ion concentration, forcing the equilibrium to the right. It decreases the phosphate ion concentration, forcing the equilibrium to the left. It increases the phosphate ion concentration, forcing equilibrium to the left. It decreases the calcium ion concentration, forcing the equilibrium to the right. It increases the calcium ion concentration, forcing the equilibrium to the right. It decreases the calcium ion concentration, forcing the equilibrium to the left. It increases the calcium ion concentration, forcing equilibrium to the left. The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, ${\mathrm{F}}^{?}$, can react with ${\mathrm{H}}_3{\mathrm{O}}^{+}$. Now consider the solubility of insoluble salts: $\begin{array}{rl}\mathrm{AgCl}(\mathrm{s})& ?{\mathrm{Ag}}^{+}(\mathrm{aq})+{\mathrm{Cl}}^{?}(\mathrm{aq})\\ \mathrm{AgF}(\mathrm{s})& ?{\mathrm{Ag}}^{+}(\mathrm{aq})+{\mathrm{F}}^{?}(\mathrm{aq})\end{array}$ The addition of acid has no affect on silver chloride. But for the second reaction, ${\mathrm{H}}_3{\mathrm{O}}^{+}$will react with ${\mathrm{F}}^{?}$, decreasing its concentration and driving the equilibrium to the right. Thus, salts that contain the conjugate of a weak acid become more soluble as the acidity of the solution increases. It decreases the calcium ion concentration, forcing the equilibrium to the left. It increases the calcium ion concentration, forcing equilibrium to the left. Part C What is the net ionic equation for ${\mathrm{AlPO}}_4$ (s) dissolving in ${\mathrm{H}}_3{\mathrm{O}}^{+}(\mathrm{aq})$ ? Express your answer as a chemical equation. ? J A cnemical reaction does not occur tor inis question.