What is [H3O+] and pH in a 0.10 M solution of HCN at 25

What is [H₃O+] and pH in a 0.10 M solution of HCN at 25

Expert Solution

We have , 0.10M HCN solution at 25^oc & Ka for HCN = 4.0 * 10^-10

HCN + H2O -----------> H3O⁺ + CN^-

Intial concentration 0.1 M 0 M 0 M

Change in concentration -x +X +X

Equilibrium concentration (0.1-x) X X

Ka = [H3O⁺][CN^-] / [HCN]

4.0 * 10^-10 = (X)(X) / (0.1-X)

4.0 * 10^-10 = (X)(X) / (0.1)

X² = (0.1) * (4.0 * 10^-10)

[H3O⁺] = X = 6.3 * 10^-6 M

[H3O⁺] = 6.3 * 10^-6 M

pH = -log[H3O⁺]

= -log (6.3 * 10-6)

pH = 5.2

queen_honey_blossom answered 2 years ago

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