Question

Determine the [H+], pH, and pOH of a solution with an [OH-] of 3.3 × 10^-13 M at 25 °C. [H+] = M pH = pOH = Determine the [H+], [OH-], and pOH of a solution with a pH of 11.31 at 25 °C. [H+] = M [OH-] = M pOH = Determine the [H+], [OH-], and pH of a solution with a pOH of 8.61 at 25 °C. [H+] = M [OH-] = M

          Determine the [H+], pH, and pOH of a solution with an [OH-] of 3.3 × 10^-13 M at 25 °C.
[H+] = M
pH =
pOH =
Determine the [H+], [OH-], and pOH of a solution with a pH of 11.31 at 25 °C.
[H+] = M
[OH-] = M
pOH =
Determine the [H+], [OH-], and pH of a solution with a pOH of 8.61 at 25 °C.
[H+] = M
[OH-] = M

Determine the [H+], pH, and pOH of a solution with an [OH-] of 3.3 × 10^-13 M at 25 °C.
[H+] = M
pH =
pOH =
Determine the [H+], [OH-], and pOH of a solution with a pH of 11.31 at 25 °C.
[H+] = M
[OH-] = M
pOH =
Determine the [H+], [OH-], and pH of a solution with a pOH of 8.61 at 25 °C.
[H+] = M
[OH-] = M

Added by Michael L.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Oluwapelumi Kolawole

07/02/2023

Step 1

Determine the [H+] , pH, and pOH of a solution with an [OH-] of 3.3 x 10^-13 M at 25°C. We know that Kw = [H+][OH-] = 1.0 x 10^-14 at 25°C. Therefore, we can calculate the [H+] as: [H+] = Kw/[OH-] = (1.0 x 10^-14)/(3.3 x 10^-13) = 0.0303 M pH = -log[H+] = Show more…

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Determine the [H+] , pH, and pOH of a solution with an [OH-] of 3.3 x 10^-13 M at 25 °C. [H+] = pH = pOH = Determine the [H+] , [OH-] and pOH of a solution with a pH of 11.31 at 25 °C [H+] = [OH-] = pOH = Determine the [H+] , [OH-] and pH of a solution with a pOH of 8.61 at 25 °C. [H+] = [OH-] =