The dissociation constant of acetic acid is 0.000018 and that for cyanoacetic acid is 0.0036 at 298 K. What would be the ratio of volumes of the two acid solutions, each containing equal moles of the

Question

The dissociation constant of acetic acid is 0.000018 and that for cyanoacetic acid is 0.0036 at 298 K. What would be the ratio of volumes of the two acid solutions, each containing equal moles of the acids, so that the solutions becomes isohydric?

Prashant Kotian · Accepted Answer

Correct answer: C. For isohydric: Ka1*C1 = Ka2*C2. C1/C2 = Ka2/Ka1 = 3.6*10^-3 / 1.8*10^-5 = 200. With equal moles n: C = n/V, so C1/C2 = V2/V1 = 200. V1/V2 = 1/200.

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