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Calculate the pOH of a solution at 25^@C...

Calculate the pOH of a solution at `25^@C` that contains `1 xx 10^(-10)` M of hydronium ions, i.e. `H_3O^+`.

A

`4.000`

B

`9.0000`

C

`1.000`

D

`7.000`

Text Solution

Verified by Experts

The correct Answer is:
A
Given `[H_3O^+]=1xx10^(-10)` M
At `25^@ C [H_3O^+][OH^-]=10^(-14)`
`therefore [OH^-]=10^(-14)/10^(-10)=10^(-4)`
Now, `[OH^-]=10^(-p^"OH") =10^(-p^"OH")`
`therefore` pOH=4
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