Calculate the H3O+ concentration of the following reaction if the initial concentration of hydrocyanic acid is...

Calculate the H3O+ concentration of the following reaction if the initial concentration of hydrocyanic acid is 0.0100 M. HCN(aq) + H2O(l) ⇔ H3O+ (aq) + CN– (aq) Kc=4.9 × 10^–10

Expert Solution

HCN(aq) + H2O(l) ⇔ H3O+ (aq) + CN– (aq)

0.01 0 0 (initial)

0.01 - x x x (at equilibrium)

Kc= [H3O+] [CN-] / [HCN]

4.9*10^-10 = x*x / (0.01-x)

since Kc is very small, x will be very small and it can ignored as compared to 0.01

so,0.01 -x will be approximately 0.01

4.9*10^-10 = x*x / (0.01)

x= 2.2*10^-6 M

Since [H3O+] = x

concentration of H3O + = 2.2*10^-6 M

queen_honey_blossom answered 2 years ago

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