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0.6 mL of acetic acid (CH3COOH) having d...

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.

Answer

Step by step text solution for 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. by CHEMISTRY experts to help you in doubts & scoring excellent marks in Class 12 exams.

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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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Knowledge Check

  • The density of 2.05 M acetic acid in water is 1.02 g/ml . Calculate the molality of solution.

    A
    3.29
    B
    0.229
    C
    22.9
    D
    2.29

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