Question:
Assertion (A):- \(MgSO_4\) is readily soluble in water
Reason (R):- The greater hydration enthalpy of \(Mg^{2+}\) ions overcomes its lattice enthalpy.
Assertion (A):- \(MgSO_4\) is readily soluble in water
Reason (R):- The greater hydration enthalpy of \(Mg^{2+}\) ions overcomes its lattice enthalpy.
Reason (R):- The greater hydration enthalpy of \(Mg^{2+}\) ions overcomes its lattice enthalpy.
Show Hint
Solubility of ionic compounds depends on the competition between:
Lattice enthalpy
and
Hydration enthalpy
If hydration enthalpy is sufficiently high, the compound dissolves easily in water.
Updated On: Jun 15, 2026
- A and R both are correct and R is the correct explanation of A.
- A and R both are correct but R is not the correct explanation of A.
- A is correct but R is not correct.
- A is incorrect but R is correct.
Show Solution
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The Correct Option is A
Solution and Explanation
Step 1: Analyze Assertion (A).
Magnesium sulphate \((MgSO_4)\) is soluble in water.
This is because water molecules strongly hydrate the ions formed during dissolution.
Hence, Assertion (A) is correct.
Step 2: Analyze Reason (R).
The \(Mg^{2+}\) ion is small in size and possesses high charge density.
Therefore, it has very high hydration enthalpy.
During dissolution, the hydration enthalpy released by water molecules surrounding \(Mg^{2+}\) ions helps to overcome the lattice enthalpy of \(MgSO_4\).
Thus, the salt dissolves readily in water.
Hence, Reason (R) is also correct.
Step 3: Check whether the reason explains the assertion.
The reason directly explains why \(MgSO_4\) dissolves in water.
Greater hydration enthalpy compensates for lattice enthalpy, favoring dissolution.
Therefore, R is the correct explanation of A.
Step 4: Final conclusion.
Hence, the correct statement is
\[ \boxed{\text{A and R both are correct and R is the correct explanation of A}} \]
Magnesium sulphate \((MgSO_4)\) is soluble in water.
This is because water molecules strongly hydrate the ions formed during dissolution.
Hence, Assertion (A) is correct.
Step 2: Analyze Reason (R).
The \(Mg^{2+}\) ion is small in size and possesses high charge density.
Therefore, it has very high hydration enthalpy.
During dissolution, the hydration enthalpy released by water molecules surrounding \(Mg^{2+}\) ions helps to overcome the lattice enthalpy of \(MgSO_4\).
Thus, the salt dissolves readily in water.
Hence, Reason (R) is also correct.
Step 3: Check whether the reason explains the assertion.
The reason directly explains why \(MgSO_4\) dissolves in water.
Greater hydration enthalpy compensates for lattice enthalpy, favoring dissolution.
Therefore, R is the correct explanation of A.
Step 4: Final conclusion.
Hence, the correct statement is
\[ \boxed{\text{A and R both are correct and R is the correct explanation of A}} \]
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