`50 mL` of `0.2 M HCl, 50 mL` of `0.2 NH_(2) SO_(4)`, and `200 mL` of `0.2 M Ba (OH)_(2)` are mixed together and the volume was made to `1 L` by adding `H_(2) O`. What is the final concentration of the solution, and what is the nature of the final solution: acidic, basic or neutral?

Explanation

In this case, strong acids and strong bases are mixed. Equal amount of mili equivalents of acid and base will neutralise. Concentrations of `HCl` and `Ba(OH)_(2)` are in molarties, they have to the converted to normalitites as concentration of `H_(2) SO_(4)` is given in normality.
`:.` Total acids `= 50 xx 0.2 xx 1 + 50 xx 0.2 xx 1` ltbgt `= 10 + 10 = 20 mEq`
Total base `= 200 xx 0.2 xx 2` (n factor)
`= 80 mEq`
Since 20 mEq of acid would neutralise 20 mEq of base, thus,
Base left `= 80 - 20 = 60 mEq`
Total volume of solution `= 1 L = 1000 mL`
So, final concentration of solution `= (mEq)/(mL) = (60)/(1000) = 0.06 N`
Final resulting mixture of solution is basic, since 60 mEq of strong base is left.