Assertion (A): Beryllium sulphate is highly soluble in water. Reason (R): The Be2+ ion is so small that its hydration enthalpy is very low, which makes dissolution favourable.

ABoth A and R are true and R is the correct explanation of A
BBoth A and R are true but R is not the correct explanation of A
CA is true but R is false
DA is false but R is true

Answer: C

A is true: BeSO4 is freely soluble because the very small, highly charged Be2+ has an extremely large (very negative) hydration enthalpy that exceeds the lattice enthalpy. R is false because it claims a low hydration enthalpy. Hence A is true and R is false.

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