Question

Determine the [OH-] , pH, and pOH of a solution with a [H+] of 8.6 x 10^-13 M at 25 %"C. [OH-] = 1 x 10 M pH = 407 pOH = 93 Determine the [H+] , pH, and pOH of a solution with an [OH-] of 5.4 x 10^-12 M at 25 %"C. [H+] = 4.7 x 10^4 M pH = 2.3 x 10^-11 pOH = 10.7

          Determine the [OH-] , pH, and pOH of a solution with a [H+] of 8.6 x 10^-13 M at 25 %"C.
[OH-] = 1 x 10 M
pH = 407
pOH = 93
Determine the [H+] , pH, and pOH of a solution with an [OH-] of 5.4 x 10^-12 M at 25 %"C.
[H+] = 4.7 x 10^4 M
pH = 2.3 x 10^-11
pOH = 10.7

Determine the [OH-] , pH, and pOH of a solution with a [H+] of 8.6 x 10^-13 M at 25 %"C.
[OH-] = 1 x 10 M
pH = 407
pOH = 93
Determine the [H+] , pH, and pOH of a solution with an [OH-] of 5.4 x 10^-12 M at 25 %"C.
[H+] = 4.7 x 10^4 M
pH = 2.3 x 10^-11
pOH = 10.7

Added by Matthew W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Madhur L

02/01/2023

Step 1

4 x 10-12 M at 25 *C, we need to first determine the [OH concentration. To do this, we use the molarity of the [OH solution (8.6 x 10 13 M) and the pKa of water (10-12). We then divide this number by the molarity of water (1 x 10-23), which gives us a [OH Show more…

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Determine the [OH-], pH, and pOH of a solution with a [H+] of 8.6 x 10^-13 M at 25%"C. [OH-] = 1.2 x 10^-2 M pH = 12.07 pOH = 1.93 Determine the [H+], pH, and pOH of a solution with an [OH-] of 5.4 x 10^-12 M at 25%"C. [H+] = 1.9 x 10^-3 M pH = 2.72 pOH = 11.28