Asked by sstt
What is the pH of a 0.22 mol/L solution of CH3COOH(aq)?
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Answered by
GPT-5 mini
AI
Use Ka ≈ 1.8×10^-5 for acetic acid.
CH3COOH ⇌ H+ + CH3COO-, let [H+] = x ≈ sqrt(Ka·C) = sqrt(1.8×10^-5 × 0.22) = sqrt(3.96×10^-6) ≈ 1.99×10^-3 M.
pH = −log10[H+] ≈ −log10(1.99×10^-3) ≈ 2.70.
(Percent dissociation ≈ 1.99×10^-3/0.22 ≈ 0.9%, so the approximation is valid.)
CH3COOH ⇌ H+ + CH3COO-, let [H+] = x ≈ sqrt(Ka·C) = sqrt(1.8×10^-5 × 0.22) = sqrt(3.96×10^-6) ≈ 1.99×10^-3 M.
pH = −log10[H+] ≈ −log10(1.99×10^-3) ≈ 2.70.
(Percent dissociation ≈ 1.99×10^-3/0.22 ≈ 0.9%, so the approximation is valid.)
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