If the freezing point of a 0.01 molal aqueous solution of a cobalt(III) chloride-ammonia complex (which behaves as a strong electrolyte) is $- {0.0558}^{\circ} C$ , the number of chloride(s) in the coordination sphere of the complex is
$[K_{f} of water = 1.86 K k g m o l^{-} 1$ ]

Open in App

Solution

Given $Δ T f = {0.0558}^{\circ} C$
as we know, $Δ T_{f} = i \times K_{f} \times m$
$\Rightarrow 0.0558 = i \times 1.86 \times 0.01$
$\Rightarrow i = 3$
Therefore, the complex will be $[C o (N H_{3})_{5} C l] C l_{2}$ .
Hence, number of chloride in co-ordination sphere is 1.

Suggest Corrections

Similar questions

Q. If the freezing point of a 0.01 molar aqueous solution of a cobalt(III) chloride-ammonia complex (which behaves as a strong electrolyte) is

- {0.0558}^{\circ} C

, the number of chloride(s) in the coordination sphere of the complex is

[K_{f} o f w a t e r = 1.86 {K kg mol}^{- 1}]

If the freezing point of a 0.01 molal aqueous solution of a cobalt chloride ammonia complex ( which behaves as a strong electrolyte ) is 0.0558 degree Celsius, the number of chloride in the coordination sphere of the complex is ? (kf of water = 1.86k kg/mole

The freezing point of an aqueous solution of a non-electrolyte is