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]`

0.01 m aqueous solution of sodium sulphate depresses the freezing point of water by 0.0284^@C . Calculate the degree of dissociation of the salt. (k_f of water = 1.86 Km^-1)

0.5 molal aqueous solution of a weak acid is 20% iionized. If K_f for water is 1.86K kg mol^-1 . The lowering in freezing point of the solution is

When 0.01 mole of a cobalt complex is treated with excess silver nitrate solution, 4.305 g silver chloride is precipitated. The formula of the complex is

Which of the following 0.1 M aqueous solution will have lowest freezing point?

0 . 6 ml of acetic acid (CH_(3) CO OH) having density 1 . 0 6 g mL^(-1) dissolved in 1 litre of water . The depression in freezing point observed for this strength of acid was 0.0205 K. Calculate the Van't Hoff factor and dissociation constant of the acid .( K_(f) for water = 1. 86 K kg mol^(-1) )

The measured freezing point depression for a 0.1 m aqueous CH_3COOH soluton is 0.19^@C . The acid dissociation constant K_a at this concentration will be (Give K_f , the molal cryoscopic constant= 1.86 K kg mol^-1 )

The freezing point of a 0.08 molal soluton of NaHSO_4 is -0.372^@C . Calculate the dissociation constant for the reaction: (HSO_4) Leftrightarrow H^+ + SO_4^(2-) (K_f for water= 1.86 Km^-1)