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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

Respuesta :

Stephen46

Answer:

The answer is option B

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

[tex][H+] = 1.79 \times {10}^{ - 14} M[/tex]

Hope this helps you

adwright424

Answer:

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...

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