All alkali halides are soluble in water expect Lif. The low solubility of LiF in water is due to its `underline ((i))` the low solubility CsI is due to `underline ((ii)).` LiF is soluble in `underline ((iii))` solvent.

Options

A. `{:(""(i), (ii), (iii)),("low lattic", " larger hydrration" , "polar"),("enthalpy", "enthalpy","solvents"):}`
B. `{:(""(i), (ii), (iii)),("high lattice", " smaller" , "non-polar"),("enthalpy", "hydration enthalpy","solvents"):}`
C. `{:(""(i), (ii), (iii)),("high hydration", " high lattice" , "non-polar"),("enthalpy", "enthalpy","solution"):}`
D. `{:(""(i), (ii), (iii)),("smaller", " high lattice" , "polar"),("hydration enthalpy", "enthalpy","solvents"):}`

Answer

B

Explanation

The low solubility of liF is due to its high lattice enethalpy whereas the low solubility of CsI is due to smaller hydration enthalpy of two large size ions. LiF is soluble in non-polar solvents like ethanol, acetone, etc.