Question

What is the [H+] in a solution with pOH of 0.253? A. 5.58 × 10−15 M B. 1.79 × 10−14 M C. 3.21 × 10−2 M D. 5.58 × 10−1 M

Answer 1

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...

Answer 2

The answer is option B

Step-by-step explanation:

To find [H+] in the solution we must first find the pH

That's

pH = - log[H+]

pH + pOH = 14

pOH = 0.253

pH = 14 - 0.253

pH = 13.747

Since we've found the pH we can now find the [H+] in the solution

We have

pH = - log[H+]

13.747 = - log[H+]

Take antilog of both sides

We have the final answer as

`[H+] = 1.79 * {10}^( - 14) M`

Hope this helps you