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0 . 6 ml of acetic acid (CH(3) CO OH)hav...

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)`)

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0.6 mL of acetic acid (CH_3COOH) having density 1.06 g mL^(-1) , is dissolved in 1 litre of water. The depression in freezing point observed for this strength of acid was 0.0205^@C . Calcuate the van't Hoff factor and the dissociation constant of acid.

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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)

3.9 g of benzoic acid dissolved in 49 g of benzene shows a depression in freezing point of 1.62K. Calculate the Van't Hoff factor and predict the nature of solute (associated or dissociated). (Given: Molar mass of benzoic acid= 122 gmol^-1 , K_f for benzene= 49 K 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)

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MODERN PUBLICATION-SOLUTIONS -EXERCISE
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