What is the [H+] in a solution with pOH of 0.253?

A: 5.58 x 10^-15 M

B: 1.79 x 10^-14 M

C: 3.21 x 10^-2 M

D: 5.58 x 10^-1 M

2 Answers

  • Okay so we know that pOH + pH = 14, so if pOH is 0.253 the pH would be 13.747.

    And pH = -log [H+], so [H+] = 10^(-pH) –>This is just the antillog…

    so [H+] = 1.791e-14, which would make sense for the strongly basic solution (so B is the correct answer)

    Hope this helps…

  • 14-.253=pH=13.74700

    pH=-log[H+]

    -13.74700=log[H+]

    10^(-13.74700)=[H+]

    1.79 × 10-14 =[H+]

    Source(s): woah

Leave a Comment