Question

$342$ g of $20\%$ by mass of $Ba(OH{)}_2$ solution (specific gravity $=0.57$) is reacted with $200$ mL of $2MHN{O}_3$ according to given balanced reaction.

$Ba(OH{)}_2+2HN{O}_3⟶Ba(N{O}_3{)}_2+2H_{2}O$

The nature of the final solution is :

• A. acidic
• B. neutral
• C. basic
• D. None of the above

Answer 1

Answer: (C)

basic

The molar mass of $Ba(OH{)}_2$ is $137+34=171$ g/mol.

$342$ g of $20\%$ by mass of $Ba(OH{)}_2$ solution corresponds to $\frac{342\times 20}{100\times 171}=0.4$ moles.

$200$ mL of $2M$ $HN{O}_3$ corresponds to $\frac{200\times 2}{1000}=0.4$ moles.

Thus, equal moles of $Ba(OH{)}_2$ and $HN{O}_3$ are present.

$Ba(OH{)}_2$ is a diacidic base and $HN{O}_3$ is a monobasic acid.

Thus, $Ba(OH{)}_2$ is present in excess.

Hence, the solution is basic in nature.

The correct option is C.