Write all possible quilibrium equations for KHP dissovled in water and then write the quilibrium constanst expressions for the equation.
This should get you started.
KHP + HOH ==> K^+(aq) + HP^-(aq)
HP^- + H20 ==> H3O^+ + P^2-
k2 = (H^+)(P^2-)/(HP^-)
To determine the equilibrium equations and write the corresponding equilibrium constant expressions for potassium hydrogen phthalate (KHP) dissolved in water, we need to consider the dissociation reaction:
KHP (s) + H2O (l) ⇌ K+ (aq) + HP− (aq) + H3O+ (aq)
The equilibrium equations for this reaction is as follows:
1. Mass Balance Equation:
n(KHP initial) = n(KHP dissociated) + n(KHP remaining)
2. Charge Balance Equation:
n(KHP dissociated) = n(K+) + n(HP−) + n(H3O+)
3. Water Balance Equation:
n(H2O initial) = n(H3O+) + n(H2O remaining)
Now, let's write the equilibrium constant expressions for the reaction:
1. Kc (concentration equilibrium constant):
Kc = [K+][HP−][H3O+] / [KHP]
Where:
[K+] = concentration of K+ (aq)
[HP−] = concentration of HP− (aq)
[H3O+] = concentration of H3O+ (aq)
[KHP] = concentration of KHP (solute)
Note: The concentrations in the equilibrium constant expression should be written in mol/L or M (molarity).
2. Kw (the autoionization constant for water):
Kw = [H3O+][OH−]
Where:
[H3O+] = concentration of H3O+ (aq)
[OH−] = concentration of OH− (aq)
Note: The autoionization constant for water (Kw) is a special case of an equilibrium constant expression for the self-ionization of water.
Please keep in mind that these equilibrium equations and equilibrium constant expressions hold true at a specific temperature.