Find Net Ionic equation for hydrolysis , Expression for equilibrium constant (Ka or Kb) and Value of (Ka or Kb)

Net Ionic equations I've got

NaC2H3O2 == CH3COO^-+H2O -->CH3COOH+OH^-

Na2CO3 ==== CO3 + 2H2O → H2CO3 + 2-OH
Kb = [H2CO3] [-OH]2 / [CO3].
Kb = 1/Ka1Ka2 = 7.1x10^13

NH4Cl === NH4Cl+H2O --> NH4OH + HCl

ZnCl2 === Zn2+H2O--> ZnO+2H^+

KAl(SO4)2 === Al^+3 + 3OH--> Al(OH)3

I have no idea about the rest.

Thank you!!!

For the hydrolysis of NaC2H3O2:

The net ionic equation is:
CH3COO^- + H2O → CH3COOH + OH^-

For the equilibrium constant expression (Ka):

Ka = [CH3COOH][OH^-] / [CH3COO^-]

The value of Ka can be determined experimentally under specific conditions.

For the hydrolysis of Na2CO3:

The net ionic equation is:
CO3^2- + 2H2O → H2CO3 + 2OH^-

For the equilibrium constant expression (Kb):

Kb = [H2CO3][OH^-]^2 / [CO3^2-]

The value of Kb can be determined experimentally under specific conditions. In this case, you have mentioned that Kb is equal to 7.1x10^13.

For the hydrolysis of NH4Cl:

The net ionic equation is:
NH4^+ + H2O → NH4OH + H^+

For the equilibrium constant expression (Kb):

Kb = [NH4OH][H^+] / [NH4^+]

The value of Kb can be determined experimentally under specific conditions.

For the hydrolysis of ZnCl2:

The net ionic equation is:
Zn^2+ + 2H2O → ZnO + 2H^+

For the equilibrium constant expression (Kb):

Kb = [ZnO][H^+]^2 / [Zn^2+]

The value of Kb can be determined experimentally under specific conditions.

For the hydrolysis of KAl(SO4)2:

The net ionic equation is:
Al^3+ + 3OH^- → Al(OH)3

For the equilibrium constant expression (Kb):

There is no Kb expression for this reaction as there are no hydroxide ions in the reactants or products.

I hope this helps! Let me know if you have any further questions.

To find the net ionic equation for hydrolysis, you need to first write the balanced chemical equation for the reaction. Then, identify the ions that participate in the reaction and write the net ionic equation by omitting the spectator ions.

For example:
1. NaC2H3O2 hydrolysis:
The balanced chemical equation is:
NaC2H3O2 + H2O → CH3COOH + NaOH

Breaking down the compounds into ions:
NaC2H3O2: Na+(aq) + C2H3O2^-(aq)
H2O: H2O(l)
CH3COOH: CH3COOH(aq)
NaOH: Na+(aq) + OH^-(aq)

Writing the net ionic equation:
C2H3O2^-(aq) + H2O(l) → CH3COOH(aq) + OH^-(aq)

2. Na2CO3 hydrolysis:
The balanced chemical equation is:
Na2CO3 + H2O → 2NaOH + CO2

Breaking down the compounds into ions:
Na2CO3: 2Na+(aq) + CO3^2-(aq)
H2O: H2O(l)
2NaOH: 2Na+(aq) + 2OH^-(aq)
CO2: CO2(g)

Writing the net ionic equation:
CO3^2-(aq) + H2O(l) → CO2(g) + OH^-(aq)

Next, to express the equilibrium constant (Ka or Kb) and find its value, you need to write the equilibrium expression for the reaction.

For the hydrolysis reactions:
1. NaC2H3O2:
The equilibrium constant Ka is the equilibrium constant for the acidic equilibrium, which can be expressed as:
Ka = [CH3COOH][OH^-] / [C2H3O2^-]

2. Na2CO3:
The equilibrium constant Kb is the equilibrium constant for the basic equilibrium, which can be expressed as:
Kb = [CO2][OH^-]^2 / [CO3^2-]

Finally, the values of Ka or Kb can be determined experimentally or by using mathematical calculations. These values are specific to each reaction and cannot be determined without additional information or experimental data.

It is important to note that the examples you provided may not represent complete hydrolysis reactions, as they only show one molecule reacting with water. In some cases, multiple molecules or ions can react with water resulting in different equilibrium expressions and equilibrium constants.

#1 you have is close but not right.

I would have written for the hydrolysis of NaC2H3O2 as a net ionic equation.

CH3COO^- + H2O ==> CH3COOH + OH^-
Kb for CH3COO^- = (Kw/Ka for CH3COOH) = about 1E-14/1.8E-5 = ?

CO3^2- + HOH ==> HCO3^- + OH^-
Kb for CO3^2- = (Kw/K2 for H2CO3) = ?

NH4^+ + H2O ==> H3O^+ + NH3
Ka for NH4^+ = (Kw/Kb for NH3) = ?

Al^3+ + 6HOH ==> Al(H2O)6^3+
Then Al(H2O)6^3+ + H2O ==> Al(H2O)5^2+ + H3O^+

Ka = Kw/Kb