Question

What would the concentration of hydroxide anions be in an aqueous solution that has `["H"_3"O"^(+)] = "0.325 M"` ? Given: `K_w = 10^(-14)` `"mol"^2"L"^2`

Answer 1

`3.08xx10^(-14)" ""mol""/""l"`

Explanation:

At `25^@"C"` the ionic product of water is given by:

`K_w=[H_3O_((aq))^(+)][OH_((aq))^(-)]=10^(-14)" ""mol"^(2)."l"^(-2)`

`:.[OH_((aq))^(-)]=K_w/[[H_3O_((aq))^(+)]]`

`[OH_((aq))^(-)]=10^(-14)/0.325=3.08xx10^(-14)" ""mol""/""l"`