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

A: 5.58 x 10^-15 M

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

Also Read :   In a 1.0× 10–2 M solution of NH4ClO4(aq), identify the relative molar amounts of these species.?

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