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Which of the following aqueous solutions should have the highest boiling point?
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Verified Answer
The correct answer is:
$1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4$
$1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4$
As we know greater the value of van't Hoff factor higher will be the elevation in boiling point and hence higher will be the boiling point of solution.
$$
\begin{array}{|l|c|}
\hline \text { Solution } & \text { van't Hoff factor }(i) \\
\hline 1.0 \mathrm{M} \mathrm{NaOH} & 2 \\
1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4 & 3 \\
1.0 \mathrm{M} \mathrm{NH}_4 \mathrm{NO}_3 & 2 \\
1.0 \mathrm{M} \mathrm{KNO}_3 & 2 \\
\hline
\end{array}
$$
$$
\text { Hence, } 1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4 \text { has highest value of boiling point. }
$$
$$
\begin{array}{|l|c|}
\hline \text { Solution } & \text { van't Hoff factor }(i) \\
\hline 1.0 \mathrm{M} \mathrm{NaOH} & 2 \\
1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4 & 3 \\
1.0 \mathrm{M} \mathrm{NH}_4 \mathrm{NO}_3 & 2 \\
1.0 \mathrm{M} \mathrm{KNO}_3 & 2 \\
\hline
\end{array}
$$
$$
\text { Hence, } 1.0 \mathrm{M} \mathrm{Na}_2 \mathrm{SO}_4 \text { has highest value of boiling point. }
$$
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