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Which of the following is the most favourable condition for the solubility of an ionic compound in water?

Option: 1

high lattice enthalpy and high hydration enthalpy of its ions


Option: 2

low lattice enthalpy and high hydration enthalpy of its ions


Option: 3

low lattice enthalpy and low hydration enthalpy of its ions


Option: 4

high lattice enthalpy and low hydration enthalpy of its ions


Answers (1)

best_answer

As we learnt, 

The solubility or the heat of solution of an ionic compound is related to the lattice energy and the heat of hydration of the ions

                    

The enthalpy of solution, enthalpy of hydration and the lattice energy can be related as

\mathrm{\Delta_{\text {sol }} H^{0}=\Delta_{\text {lattice }} H^{0}+\Delta_{\text {hyd }} H^{0}}

High negative values for \mathrm{\Delta_{sol} H^0} is a favourable condition for the solubility of ionic compounds

Thus, for greater solubility, the lattice energy should be low and the hydration enthalpy shoud be high.

Thus, the correct answer is Option (2)

Posted by

Nehul

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