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29 November, 13:43

What is the pH of a solution with [OH - ] = 1.60x10-9 M? Include two digits past the decimal in your answer.

What is the pH of a solution if [H3O+] = 2.00x10-5 M? Include two digits past the decimal in your answer.

A solution has a pH value of 3.90. What is the pOH for the solution? Include one digit past the decimal in your answer.

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Answers (2)
  1. 29 November, 16:21
    0
    1) pH = 5.20

    2) pH = 4.70

    3) pOH = 10.1

    Explanation:

    What is the pH of a solution with [OH - ] = 1.60x10-9 M?

    Step 1: Data given

    [OH-] = 1.60 * 10^-9 M

    Step 2: Calculate pOH

    pOH = - log[OH-]

    pOH = - log [1.60*10^-9]

    pOH = 8.80

    Step 3: Calculate pH

    pH = 14 - pOH

    pH = 14 - 8.8 = 5.20

    What is the pH of a solution if [H3O+] = 2.00x10-5 M?

    [H3O+] = [H+] = 2.00 * 10^-5 M

    pH = - log[H+]

    pH = - log[2.00*10^-5]

    pH = 4.70

    A solution has a pH value of 3.90. What is the pOH for the solution?

    pOH = 14 - pH

    pOH = 14 - 3.90 = 10.1
  2. 29 November, 17:27
    0
    Answer: 5.21, 4.69 & 10.1

    Explanation:

    Question 1:

    We have to determine the pOH of the solution first.

    pOH = - Log [OH-]

    = - Log (1.60 x 10∧-9)

    = 9 - 0.204

    = 8.79

    Using the mathematical equation;

    pH + pOH = 14

    ∴ pH + 8.79 = 14

    Making pH subject of formular; pH = 14 - 8.79 = 5.21

    Question 2:

    pH = - Log [H3O+]

    = - Log (2.00 x 10∧-5)

    = 5 - 0.301

    = 4.69

    Question 3:

    Using the mathematical equation, pH + pOH = 14

    3.90 + pOH = 14

    ∴ pOH = 14 - 3.90

    = 10.1
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