You need to learn to do these. The easy way, in the beginning, is to write the hydrolysis as if the salt (all of them) reacted completely with water, then apply rules to know what happens. For example, for NaC2H3O2,
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.
The Hydrolysis Reactions - Write net-ionic equations for the reaction of each salt with water below. If there is no reaction, write N.R.
1. NH4C2H3O2
2. NH4Cl
3. NaCl
4. Na2CO3
5. NaC2H3O2
6. NaHSO4
7. FeCl3
8. NaH2PO4
9. NaHCO3
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