Calculate the p H and the concentration of all species present (H3 O+ , A - , HA, and OH - in 0.50 M HA. Ka = 3.5 x 10-6
Weak acid dissociates as AH + H2O ⇌ A- + H3O+
Ka = [A-][H3O+] / [AH]
but [A-] = [H3O+] = x
Ka = [x][x] / [AH]
Substitute the value in equation
3.510-6 = [x]2/ 0.50
[x]2 = 3.510-60.50 = 1.7510-6
[x] = 1.322910-3 M
Concentration of H3O+ = 1.322910-3 M
pH = - log[H3O+]
pH = - log 1.322910-3
pH = 2.88
pOH = 14 - pH = 14 - 2.88 = 11.12
[OH-] = 10-pOH = 10-11.12 = 1.586 10-12
[OH-] = 1.586 10-12
concentration of HA after dissociation = (initial concentration of HA) - [H3O+]
= (0.50) - (1.322910-3) = 0.4986771 M
[HA] = 0.4989771 M
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