Ammonia undergoes self dissociation according to the reaction `2 NH_(3(l)) hArr NH_(2(am))^(+)+NH_(2(am))^(-)` where am, stands for ammoniated. When 1 mol of `NH_(4)` CI is dissolved in 1 kg of liquid ammonia, the b.p. at 760 torr is observed as `-32.7^(@)C` (normal boiling b.p. of `NH_(3(l))` is `33.4^(@)C`). What conclusion is reached about the nature of the solution

Options

A. `NH_(4)` CI is completely dissociated in `NH_(3)`
B. `NH_(4)` CI is partially dissociated in `NH_(3)`
C. `NH_(4)`CI is not dissociated in `NH_(3)`
D. Boiling point is not raised

Answer

A

Explanation

`NH_(4)Cl` is a strong acid in liq. `NH_(3)`. Since, it ionizes to give `NH_(4)^(+)` (which is cation of the the solvent).
`NH_(4)Cl hArr NH_(4)^(+)+Cl^(-)`