3. Determine the pH of each of the following solutions. (Hint: See Sample Problem B.) a. 1.0 x 10-2 M HCI c. 1.0 x 10-MHI b. 1.0 x 10-3 M HN

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3. Determine the pH of each of the following solutions. (Hint: See Sample Problem B.) a. 1.0 x 10-2 M HCI c. 1.0 x 10-MHI b. 1.0 x 10-3 M HNO3 d. 1.0 x 10-M HB​

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Khoii Minh 5 months 2021-08-30T13:46:47+00:00 1 Answers 10 views 0

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    2021-08-30T13:48:08+00:00

    Answer:

    a. pH = 2 b. pH = 3 c. pH = 1 d. Unanswerable

    Explanation:

    pH = -log[H+] OR pH = -log{H3O+]

                        and inversely

    pOH = -log[OH-]

    1. Determine what substance you are working with, (acid/base)

    2. Determine whether or not that acid or base is strong or weak.

    a. 1.0 x 10^-2M HCl

    HCl is a strong acid, therefore it will dissociate completely into H+ and Cl- with all ions going to the H+, therefore, the concentration of HCl and concentration of H+ are going to be equal, meaning we simply take the negative logarithm of the concentration of HCl and that would equal pH

    pH = -log[H+]

    pH = -log(1.0×10^-2)

    pH = 2

    b. 1.0 x 10^-3M HNO3

    HNO3 like part a, is a strong acid, therefore it would simply require you to take the negative logarithm of the concentration of the compound itself, to find its pH.

    pH = -log[H+]

    pH = -log(1.0 x 10^-3)

    pH = 3

    c. 1.0 x 10^-1M HI

    Like the previous parts, HI is a strong acid

    pH = -log[H+]

    pH = -log(0.10)

    pH = 1

    d. HB isn’t an element, nor is it a compound so that would be unanswerable.

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Giải phương trình 1 ẩn: x + 2 - 2(x + 1) = -x . Hỏi x = ? ( )