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28 January, 09:59

e sure to answer all parts. Calculate the pH of the following aqueous solutions at 25°C: (a) 9.5 * 10-8 M NaOH (b) 6.3 * 10-2 M LiOH (c) 6.3 * 10-2 M Ba (OH) 2

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  1. 28 January, 13:10
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    (a) 7.0

    (b) 12.8

    (c) 13.11

    Explanation:

    (a)

    NaOH is a strong base with 1 OH⁻. If [NaOH] = 9.5 * 10⁻⁸ M, then [OH⁻] = 9.5 * 10⁻⁸ M.

    The pOH is:

    pOH = - log [OH⁻] = - log 9.5 * 10⁻⁸ = 7.0

    The pH is:

    pH = 14 - pOH = 14 - 7.0 = 7.0

    (b)

    LiOH is a strong base with 1 OH⁻. If [LiOH] = 6.3 * 10⁻² M, then [OH⁻] = 6.3 * 10⁻² M.

    The pOH is:

    pOH = - log [OH⁻] = - log 6.3 * 10⁻² = 1.2

    The pH is:

    pH = 14 - pOH = 14 - 1.2 = 12.8

    (c)

    Ba (OH) ₂ is a strong base with 2 OH⁻. If [Ba (OH) ₂] = 6.3 * 10⁻² M, then [OH⁻] = 2 * 6.3 * 10⁻² M = 0.13 M

    The pOH is:

    pOH = - log [OH⁻] = - log 0.13 = 0.89

    The pH is:

    pH = 14 - pOH = 14 - 0.89 = 13.11
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