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If the freezing point of a 0.01 molal aq...

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^(@)C`, the number of chloride (s) in the coordination sphere of the complex if `[K_(f)` of water `=1.86 K kg mol^(-1)]`

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If the freezing point of a 0.01 molal aq.solution of a cobalt (III chloride)-ammonia complex (which behaves a strong electrolyte) is -0.0372^(@)C , the no. of chloride (s) in the coordination sphere of the complex is ( K_(f) of water is 1.86K kg mol^(-1) )

If the freezing point of a 0.01 molal aqueous solution of a cobalt chloride ammonia complex is -0.0558^@C , the number of chloride in the coordination sphere of the complex is [K_f of water =1.86K kg mol^-1]

The freezing point of a 0.05 molal solution of a non-electrolyte in water is [K_(f)=1.86K//m]

The freezing points of a 0.05 molal solution of a non-electrolyte in water is: (K, = 1.86 K molality^-1 )

The freezing point of a 0.05 molal solution of a non-electrolyte in water is: ( K_(f) = 1.86 "molality"^(-1) )