Molarity of `K^(+)` ions in `0.33 M` potassium sulphate aqueous solution is

Options

A. less than 0.33 M
B. equal to 0.33 M
C. more than 0.33 M
D. `0.66 M`

Answer

4

Explanation

A `0.33 M` aqueous solution of potassium sulphate `(K_(2)SO_(4))` contains `0.33 mol` of the salt in 1 litre of solution. The molarities of the potassium and sulphateions in the solution are `0.66 M` and `0.33 M` respectively because `K_(2)SO_(4)` is a strong electroly to i.e., `1 mol K_(2)SO_(4)` gives `2 mol of K^(+)` ions and 1 mol of `SO_(4)^(2-)` ions on dissociation.