The solubility order for alkali metal fluoride in water is :
Show Hint
- \(\mathrm{LiF} \lt \mathrm{RbF} \lt \mathrm{KF} \lt \mathrm{NaF}\)
- \(\mathrm{RbF} \lt \mathrm{KF} \lt \mathrm{NaF} \lt \mathrm{LiF}\)
- \(\mathrm{LiF} \gt \mathrm{NaF} \gt \mathrm{KF} \gt \mathrm{RbF}\)
- \(\mathrm{LiF} \lt \mathrm{NaF} \lt \mathrm{KF} \lt \mathrm{RbF}\)
The Correct Option is D
Solution and Explanation
F- is very small, so with the very small Li+ the lattice energy is very high and is not compensated by hydration enthalpy: LiF is the least soluble.
Going down the group the cation grows larger and the lattice energy falls faster than the hydration enthalpy, so the solubility of the fluorides increases.
Order: \(\mathrm{LiF} \lt \mathrm{NaF} \lt \mathrm{KF} \lt \mathrm{RbF}\).
Answer: (4) \(\mathrm{LiF} \lt \mathrm{NaF} \lt \mathrm{KF} \lt \mathrm{RbF}\)
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