Consider the dissociation of strong versus weak acids: HCl aq +H20 1 rightarrow
ID: 839377 • Letter: C
Question
Consider the dissociation of strong versus weak acids: HCl aq +H20 1 rightarrow 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. The solubility reaction is Ca3 PO4 2 s 3Ca2+ aq + 2PO43- aq The addition of acid protonates the anion PO33- forming HPO32- The equilibrium shifts to compensate. A compound such as NiBr2 would not be impacted by the addition of an acid or a base since it is a salt composed of the conjugate of a strong acid HBr and a strong base Ba OH 2 . Strong acids and bases ionize completely in solution, and salts thus the addition of an acid or base will not impact the equilibrium. Part C Another metal phosphate is cobalt phosphate. It will behave similar to calcium phosphate in an acid solution. What is the net ionic equation including phases for CoPO4 s dissolving in H3O+ aq ? Express your answer as a net ionic equation.Explanation / Answer
The correct answer is CoPO4(s)+H3O+(aq)?Co3+(aq)+HPO42?(aq)+H2O(l)