How can strong ion-dipole interactions actually limit the ion solubility in wate

Question

How can strong ion-dipole interactions actually limit the ion solubility in water, despite being favorable from a potential energy standpoint?

A)

Strong ion-dipole interaction can cause the water molecules to localize around the ions, decreasing the number of configurations that the water molecules can adopt

B)

Strong ion-dipole interaction can cause the water molecules to localize around the ions, increasing the number of configurations that the water molecules can adopt

C)

Strong ion-dipole interaction can cause the water molecules to become more disordered, decreasing the number of configurations that the water molecules can adopt

D)

Strong ion-dipole interaction can cause the water molecules to become more disordered, increasing the number of configurations that the water molecules can adopt

A)

Strong ion-dipole interaction can cause the water molecules to localize around the ions, decreasing the number of configurations that the water molecules can adopt

B)

Strong ion-dipole interaction can cause the water molecules to localize around the ions, increasing the number of configurations that the water molecules can adopt

C)

Strong ion-dipole interaction can cause the water molecules to become more disordered, decreasing the number of configurations that the water molecules can adopt

D)

Strong ion-dipole interaction can cause the water molecules to become more disordered, increasing the number of configurations that the water molecules can adopt

Explanation / Answer

As due to strong ion-dipole interaction water molecules get localised around the ions which decreases the number of configurations that the water molecule can adopt and hence there will be no more water molecule left to interact with the ions after a certain point hence the solubility will be adversely affected.

Solubility of an ion directly depends upon the extent of interaction between the solute and solvent.

Hence option A is correct.

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