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2 November, 05:05

A buffer is made with sodium acetate (CH3COONa) and acetic acid (CH3COOH); the Ka for acetic acid is 1.80*10-5. The pH of the buffer is 3.98. What is the ratio of the equilibrium concentration of sodium acetate to that of acetic acid if you assume that the Henderson-Hasselbalch equation is accurate?

A. - 0.760

B. 0.174

C. 0.840

D. 5.75

E. Not enough information is given to answer this question.

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Answers (1)
  1. 2 November, 05:32
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    B. 0.174

    Explanation:

    A buffer is formed by a weak acid (CH₃COOH) and its conjugate base (CH₃COO⁻, coming from sodium acetate). We can calculate the pH of this buffer using the Henderson-Hasselbalch equation.

    pH = pKa + log [CH₃COO⁻]/[CH₃COOH]

    pH - pKa = log [CH₃COO⁻]/[CH₃COOH]

    3.98 - (-log 1.80 * 10⁻⁵) = log [CH₃COO⁻]/[CH₃COOH]

    -0.760 = log [CH₃COO⁻]/[CH₃COOH]

    [CH₃COO⁻]/[CH₃COOH] = anti log (-0.760)

    [CH₃COO⁻]/[CH₃COOH] = 0.174
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