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26 June, 06:52

Calculate the pH of a solution prepared by dissolving 0.147 moles of acetic acid and 0.405 moles of sodium acetate in water sufficient to yield of solution. The Ka of acetic acid is 1.76*10-5

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  1. 26 June, 07:52
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    pH = 5.19

    Explanation:

    Mixture of acetic acid with sodium acetate produce a buffer (Buffer is defined as the mixture of a weak acid with its conjugate base and vice versa). The pH of the buffer can be determined using Henderson-Hasselbalch equation:

    pH = pKa + log₁₀ [A⁻] / [HA]

    Where pKa is - log Ka = 4.75; [A⁻] is the concentration of conjugate base (Acetate ion) and [HA] is molar concentration of the weak acid.

    -You can use moles of the compounds rather than its concentrations, that is:

    [HA] = 0.147 moles

    [A⁻] = 0.405 moles

    Replacing in H-H equation:

    pH = 4.75 + log₁₀ [0.405] / [0.147]

    pH = 5.19
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