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The freezing point depression of 0.1 mol...

The freezing point depression of 0.1 molal solution of acetic acid in benzene is `0.256 K kg mol^(-1)`.Kf for benzene is 5.12`K kg Mol^(-1)`. What conclusion can you draw about the molecular state of acetic acid in benzene.

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

The depression in freezing point of a 0.1 molal solution of benzoic acid in benzene is 0.256K. (K_f for benzene =5.12K kg mol^(-1) ) . Calculate the value of van’t Hoff factor and predict whether benzoic acid is associated or dissociated.

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The freezing point of 1 molar NaCl solution assuming NaCl to be 100% dissociated in water is: ( K_f = 1.86 K molality^-1 )

Addition of 0.643 g of a compound to 50. mL of benzene .(density 0.879 g/mL lowers the freezing point from 5.51^0C to 5.03^0C. If K_(f) for benzene is 5.12 K kg mol^1 , calculate the molar mass of the compound.

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