Consider the dissociation of strong versus weak acids: HCl(aq)+H2O(l)H3O+(aq)+Cl
ID: 970600 • Letter: C
Question
Consider the dissociation of strong versus weak acids:
HCl(aq)+H2O(l)H3O+(aq)+Cl(aq)
HF(aq)+H2O(l)H3O+(aq)+F(aq)
The first reaction is not reversible, but the second one is. So, only the conjugate of the weak acid, F, can react with H3O+. Now consider the solubility of insoluble salts:
AgCl(s)Ag+(aq)+Cl(aq)
AgF(s)Ag+(aq)+F(aq)
The addition of acid has no effect on silver chloride. But for the second reaction, H3O+ will react with 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.
Q-
Another metal phosphate is aluminum phosphate. It will behave similar to calcium phosphate in an acid solution. What is the net ionic equation including phases for AlPO4(s) dissolving in H3O+(aq)?
Express your answer as a net ionic equation.
Explanation / Answer
AlPO4(s)+H3O+(aq)Al3+(aq)+HPO42(aq)+H2O(l)