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

Calculate the pOH of a solution at 25^@C that contains 1 xx 10^(-10) M

1.	Calculate the pOH of a solution at 25^@C that contains 1 xx 10^(-10) M of hydronium ions, i.e. H_3O^+.
Answer» `4.000` `9.0000` `1.000` `7.000` Solution :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