Question

$50ml$ of $2MNaOH$ solution and $10ml$ of $2N{H}_{2}S{O}_4$ solutions are mixed together, the resulting solution will be:

• A. Alkaline
• B. Acidic
• C. Strongly Acidic
• D. Neutral

Answer 1

The correct option is A Alkaline

We know, normality = $molarity\times n-factor$

For $NaOH$ = n - factor is 1
Thus for $NaOH$, molarity = normality
Therefore, number of milliequivalents =
$=2N\times 50ml$ = $100$

For $H_{2}S{O}_4$ ,
number of milliequivalents =
$\therefore N_2=2N\times 10ml$ = $20$
Since number of milliequivalents for alkali is greater the solution willl be basic
The resulting solution will be Alkaline.