[Equilibrinsane]

These are unbalanced but are the products correct.

NaCl + H₂O - not hydrolysis
Na₂CO₃  2Na⁺ + HCO₃^- + OH^-
NaHCO₃ + H₂O - not hydrolysis
NaC₂H₃O₂ + H₂O  HC₂H₃O₂ + NaOH
Al₂(SO₄)₃ + H₂O  Al(OH)₃ + H₂SO₄
ZnSO₄ + 2H₂O  Zn²⁺ + HSO₄^- + OH^-
Na₃PO₄ + H₂O  NaOH + H₃PO₄
NaH₂PO₄ + H₂O  H₃PO₄ + NaOH
NH₄Cl + H₂O - not hydrolysis
Pb(NO₃)₂ + H₂O  Pb(OH)₂ + HNO₃
KBr + H₂O  HBr + KOH
MnSO₄ +H₂O  H⁺ + SO₄^- + Mn(OH)₂

Could someone tell me which ones are wrong and also tell me how to figure out whether hydrolysis would actually occur.

[Arkcon]

Well, you can start by sorting your own list by hydrolysis or no hydrolysis, and see if you can recognize trends.  Many of your predictions seem wrong, and you seem to mixing up dissociation into ions with chemical reactions, so I really don't know where you're going by lumping them under the hydrolysis term.

[Equilibrinsane]

Well I guess the real problem I'm having is determining whether something will undergo hydrolysis or not. I was thinking that maybe hydrolysis only occurs when at least one of the components of the salt (i.e. anion or cation) is the conjugate base or acid of a weak base or acid. Is this correct or is it the other way around (conjugate base or acid of a strong base or acid)

I feel like an idiot, but the book for our class does no explaining of the necessities of a hydrolysis reaction

[Borek]

I was thinking that maybe hydrolysis only occurs when at least one of the components of the salt (i.e. anion or cation) is the conjugate base or acid of a weak base or acid.

That's a good idea, but apparently in some cases you failed to apply it correctly.

Also hydroxides solubility plays a role.