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 ofCH3COOH is 1.8 × 10^-5.(a) 2.09(b) 5.14(c) 2.65(d) 3.98The question was asked in quiz.My question is based upon Equilibrium in division Equilibrium of Chemistry – Class 11

If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO^– together make a buffer

1.	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 ofCH3COOH is 1.8 × 10^-5.(a) 2.09(b) 5.14(c) 2.65(d) 3.98The question was asked in quiz.My question is based upon Equilibrium in division Equilibrium of Chemistry – Class 11
Answer» 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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