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20 May, 09:47

What is the pH of each of the following aqueous solutions? (a) 0.036 M HCl WebAssign will check your answer for the correct number of significant figures. 1.44 Correct: Your answer is correct. (b) 0.17 M KOH WebAssign will check your answer for the correct number of significant figures. 13.23 Correct: Your answer is correct. (c) 0.19 M Ba (OH) 2

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  1. 20 May, 13:05
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    (a) 0.036 M HCl

    [HCl] = 0.036 M

    As HCl is a strong acid, it will completely dissociate and produce H + ions.

    [ H+] = M

    pH = - log [ H+]

    pH = - log[0.036]

    pH = - (-1.444)

    pH = 1.44

    (b) 0.17 M KOH

    pH + pOH = 14

    pH = - log10[H+], and pOH = 14-pH

    pH = 14 - pOH

    pH = 14 - (-log10 (0.17))

    pH = 14 - (0.77) = 13.23

    (c) 0.19 M Ba (OH) 2

    [H+] [OH-] = 1.0*10-14M

    [OH-] = 2 * 0.19 = 0.38M

    [H+] = 2.63 * 10-14M

    pH = - log10 ([H+])

    pH = - log10 (2.63 * 10-14) = 13.58.
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