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    1.0 M solution of a strong acid, HA

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    Are the following statements about a 1.0 M solution of a strong acid, HA, true or false?
    [A-] › [H+]: True/False
    The pH is 0.00: True/False
    [H+] = 1.0 M: True/False
    [HA] = 1.0 M: True/False
    From the given solubility data given, calculate the value of Ksp for the following compounds.
    SrF2; 7.3 x 10-2 g/L
    Ag3PO4; 6.7 x 10-3 g/L

    Please provide step by step explanation. Thanks!

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    https://brainmass.com/chemistry/physical-chemistry/solution-strong-acid-537203

    Solution Preview

    a) Are the following statements about a 1.0 M solution of a strong acid, HA, true or false?
    [A-] › [H+]: True/False:
    False, When HA dissociates, it will form equal amounts of H+ and A_

    b) The pH is 0.00: True/False
    pH = -log[H+] = -log1 = 0
    True
    c) [H+] = 1.0 M: True/False
    True. Since strong acids completely dissociates, concentration of H+ = 1M

    d) [HA] = 1.0 M: True/False
    It is false. Since strong acid dissociates, there won't be any undissociated [HA] when dissolved in water.

    From the given solubility data given, calculate the value ...

    Solution Summary

    The expert examines a 1.0M solution of a strong acid HA. The solubility is calculated.

    $2.19

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