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22 December, 20:25

A certain weak acid, ha, has a ka value of 3.6*10-7. part a calculate the percent ionization of ha in a 0.10 m solution. express your answer to two significant figures and include the appropriate units. view available hint (s)

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  1. 22 December, 21:33
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    Answer is: the percent ionization is 0,19%.

    Chemical reaction: HA (aq) ⇄ H⁺ (aq) + A⁻ (aq).

    Ka (HA) = 3,6·10⁻⁷.

    c (HA) = 0,1 M.

    [H⁺] = [A⁻] = x; equilibrium concentration.

    [HA] = 0,1 M - x.

    Ka = [H⁺] · [A⁻] / [HA].

    0,00000036 = x² / 0,1 M - x.

    Solve quadratic equation: x = 0,00019 M.

    α = 0,00019 M : 0,1 M · 100% = 0,19%.
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