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`)

Units of ebullioscopic constant are K kg mol^-1 .

0.2 m aqueous solution of a weak acid is 20% dissociated. The boiling point of this solution is (K_(b) of water= 0.52Km^-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 0.08 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)

The depression in freezing point of 0.01 m aqueous CH_(3)CooH solution is 0.02046^(@) , 1 m urea solution freezes at -1.86^(@)C . Assuming molality equal to molarity, pH of CH_(3)COOH solution is

Is CH_3COOH strong or weak acid? Will its 0.1 M solution have pH more or less than HCl of same concentration?

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) )

In a 0.5 molal solution KCl, KCl is 50% dissociated. The freezing point of solution will be ( K_(f) = 1.86 K kg mol^(-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