Which of the aqueous equimolal solution will have its vapour pressure near to solvent?

Urea

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B a {({N O}_{3})}_{2}

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N a {N O}_{3}

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A l {({N O}_{3})}_{2}

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Solution

The correct option is A Urea
$\frac{p - p_{s}}{p} = \frac{n}{n + N} i;$

$Δ P$ is minimum since $i = 1$ for urea.

Thus, urea solution will have its vapour pressure closer to solvent.

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