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21 May, 01:56

What is the pH of a 1.288 M solution of sodium acetate? Ka of acetic acid is 1.8*10^-5. (2 decimal places)

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  1. 21 May, 02:15
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    The pH of the solution is 9.43

    Explanation:

    sodium acetate = CH3COONa

    after removing the spectator ion Na

    CH3COO⁻ + H2O ⇄ CH3COOH + H3O⁺

    since sodium acetate is a weak base, it will not react completely with water. Thus a value "x" will be used to make the products.

    At equilibrium:

    [CH3COO⁻] = 1.288 - x

    [CH3COOH] = x

    [H3O⁺] = x

    Since a base is reacting with H2O, Kb is used at equilibrium: Kb = (1*10^-14) / (1.8*10^-5) = 5.6*10^-10)

    Kb = [CH3COOH][H3O⁺]/[CH3COO⁻]

    Kb = (x²) / (1.288-x) since the Kb is significantly lower than 1.288 we can make a mathematical assumption that x is significantly lower than 1.288.

    5.6*10⁻¹⁰ = x²/1.288

    x = [OH⁻] = 2.675*10⁻⁵ M

    pOH = - log[OH⁻] = 4.57

    pH=14-pOH = 14 - 4.57 = 9.43
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