Question

Which of the following options correctly describes the solubility behavior of potassium chloride $\left(KCl\right)$?

• A. Solubility in $C{Cl}_4>$ solubility in $C{H}_{3}C{H}_{2}OH>$ solubility in $H_{2}O$
• B. Solubility in $H_{2}O>$ solubility in $C{H}_{3}C{H}_{2}OH>$ solubility in $C{Cl}_4$
• C. Solubility in $C{H}_{3}C{H}_{2}OH>$ solubility in $C{Cl}_4>$ solubility in $H_{2}O$
• D. Solubility in $H_{2}O>$ solubility in $C{Cl}_4>$ solubility in $C{H}_{3}C{H}_{2}OH>$

Answer 1

Answer: (B)

Solubility in $H_{2}O>$ solubility in $C{H}_{3}C{H}_{2}OH>$ solubility in $C{Cl}_4$

As $KCl$ is the ionic compound, it dissolves in polar solvent.
More the polarity of the solvent , more will be solubility of KCl in that solvent.
Now, as the order of polarity of the solvent ( given ) is as follows:
$H_{2}O>C{H}_{3}C{H}_{2}OH>CC{l}_4$
Hence order of solubility is as also in the same order.
$H_{2}O>C{H}_{3}C{H}_{2}OH>CC{l}_4.$