[jsmith613]

I was wondering if someone could check my understanding of Hydrolysis.

a) In a reaction where there is a relatively strong acid, and a relatively strong base the equilibrium lies in the middle.
HCl (aq) + NaOH (aq) --> NaCl + H2O
The Na+ ion comes from NaOH which is a strong alkali, SO Na+ is a weak acid
The Cl+ ion comes from HCl which is a strong acid, SO Cl- is a weak base
this means there are so few H+ and OH- ions in solution, that they all react a neutralize to form water

b) In a reaction where there is a relatively strong acid, and a relatively weak base the equilibrium lies towards the left (lower pH).
Example: Na2CO3 in solution
Na2CO3 (aq) --> 2Na+ + CO3-
the Na+ is a weak acid (NaOH is a strong alkali therefore Na+ is a weak acid)
the CO3- is a strong base (CO3- comes from HCO3- which is a weak acid - therefore CO3- is relatively strong)

Therefore the Na+ + H2O --> NaOH + H+ (Please can someone explain why there is little H+)
CO3- + H2O --> HCO3 - + OH- (in this reaction there is excess OH- as the HCO3 - is relativley weak so less H+ is needed)

c) with a strong alkali and a weak acid it is the opposite of b

[Borek]

Looks OK.

[savy2020]

...the Na+ is a weak acid (NaOH is a strong alkali therefore Na+ is a weak acid).

....Therefore the Na+ + H2O --> NaOH + H+ (Please can someone explain why there is little H+).

In the quote above,
The first statement explains what you want

[jsmith613]

...the Na+ is a weak acid (NaOH is a strong alkali therefore Na+ is a weak acid).

....Therefore the Na+ + H2O --> NaOH + H+ (Please can someone explain why there is little H+).
In the quote above,
The first statement explains what you want

so are you saying that becasue Na+ is weak, it results in less H+ ions in solution?

[savy2020]

so are you saying that becasue Na+ is weak, it results in less H+ ions in solution?

Yes the equation as you wrote will be more tending to go backward since of Na+ and H+,  Na+ is weaker than H+. and hence can't accept OH- as readily as H+.