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  4. At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure? (Mol. wt. mathrmNaCl=58.5, mathrmH2 mathrmSO4=98.0 mathrm~g mathrm~mol-1 )

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Q. At a constant temperature, which of the following aqueous solutions will have the maximum vapour pressure?

(Mol. wt. $\mathrm{NaCl}=58.5, \mathrm{H}_2 \mathrm{SO}_4=98.0 \mathrm{~g} \mathrm{~mol}^{-1}$ )

NTA AbhyasNTA Abhyas 2020Solutions

Solution:

One molar $\text{(1} \, \text{M)}$ aqueous solution is more concentrated than one molal aqueous solution of the same solute. In solution, $H_{2}SO_{4}$ provides three ions. While $\text{NaCl}$ provides two ions. Hence, vapour pressure of solution of $\text{NaCl}$ is higher (as it gives less ions). Therefore, $\text{1} \, \text{molal} \, \text{NaCl}$ will have the maximum vapour pressure.