NaC2H3O2 + HOH ==> NaOH + HC2H3O2. That is step 1.
Step 2. Look at the products. If the product is a weak acid or weak base, that cation/anion hydrolyzes. If not , it does not. Thus NaOH is a strong base; therefore Na^+ does NOT hydrolyze. HC2H3O2 is a weak acid; therefore, C2H3O2^- does. The net ionic equation for the hydrolysis of NaC2H3O2 is the following:
C2H3O2^- + HOH ==> HC2H3O2 + OH^-
The others follow the same set of rules. For the NH4^+, it is much easier to write BOTH as half reactions. For example, for NH4C2H3O2
NH4^+ + H2O ==> NH3 + H3O^+
NH3 is a weak base, therefore, the NH4^+ hydrolyzes.
You already know, from the first example I did, that C2H3O2^- hydrolyzes; therefore, BOTH NH4^+ and C2H3O2^- hydrolyze.
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