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13 September, 08:09

If the ionization constant of water, kw, at 40°c is 2.92 * 10-14, then what is the hydronium ion concentration and ph for an acidic solution?

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  1. 13 September, 10:00
    0
    The formula for Kw is:

    Kw = [H+] [OH-]

    For water, [H+] = [OH-]

    Therefore we can write

    Kw = [H+]²

    For the temperature (40C) given,

    Kw = 2.92 x 10^-14

    [H+]² = 2.92 x 10^-14

    [H+] = √ (2.92 x 10^-14)

    [H+] = 1.71 x 10^-7

    To determine the pH:

    pH = - log [H+]

    pH = - log (1.71 x 10^-7)

    pH = 6.76
  2. 13 September, 11:29
    0
    Answer is: the hydronium ion concentratio is 1.71*10⁻⁷ mol/dm³ and pH<6.76.

    The Kw (the ionization constant of water) at 40°C is 2.94*10⁻¹⁴ mol²/dm⁶ or 2.94*10⁻¹⁴ M².

    Kw = [H₃O⁺] · [OH⁻].

    [H₃O⁺] = [OH⁻] = x.

    Kw = x².

    x = √Kw.

    x = √2.94*10⁻¹⁴ M².

    x = [H₃O⁺] = 1.71*10⁻⁷ M; concentration of hydronium ion.

    pH = - log[H₃O⁺].

    pH = - log (1.71*10⁻⁷ M).

    pH = 6.76.

    pH (potential of hydrogen) is a numeric scale used to specify the acidity or basicity an aqueous solution.
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