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If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO^– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10^-5.

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in Chemistry – Class 11 by (148k points)
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO^– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of  CH3COOH is 1.8 × 10^-5.

(a) 2.09

(b) 5.14

(c) 2.65

(d) 3.98

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My question is based upon Equilibrium in division Equilibrium of Chemistry – Class 11

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The correct answer is (b) 5.14

Explanation: We have henderson-hasselbalch equation as pH = pKa + log[salt]/[acid]. So by substituting the concentrations of silent and acid along with the acid dissociation constant, we get pH = -log[1.8 × 10^-5] + log [0.50mol/L]/[0.20mol/L] = 5.14.

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