Q.
Ammonia undergoes self-dissociation according to the reaction,
$2 NH _{3}(l) \rightleftharpoons NH _{4}^{+}{ }_{(a m)}^{+}+ NH _{2(a m)}^{-}$
where am, stands for ammoniated. When $1$ mole of $NH _{4} Cl$ is dissolved in $1\, kg$ of liquid ammonia, the b. p. at $760$ tour is observed at $-32^{\circ} C$ (Normal b.p. of $N H_{3(l)}$ is $-33.4^{\circ} C$ ). What conclusions are reached about the nature of the solution?
AMUAMU 2012Equilibrium
Solution: