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)`

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 )

Calculate the equilibrium constant for the reaction at 298K 4 Br + O2 + 4H+ → 2 Br2 + 2H2O Given that Ecell = 0.16V​

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)

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]

Phenol associates in benzene to form a dimer (C_6H_5OH)_2 . The freezing point of a soluton contianing 5 g of phenol in 250 g of benzene is lowerd by 0.70^@C . Calculate the degree of association of phenol in benzene. (K_f for benzene=5.12 Km^-1)

Calculate the normal freezing point of a sample of sea water containing 3.8% NaCl and 0.12% MgCl_2 by mass. (K_f for water=1.86Km^-1)

Ethylene glycol (molar mass = 62gmol^-1) is a common automobile antifreeze. Calculate the freezing point of a solution containing 12.4 g of this substance in 100 g of water. Would it be advisable to keep this substance in car radiator during summer? (K_f for water=1.86Km^-1 and K_b for water=0.512Km^-1) .