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0.6 mL of acetic acid (CH3COOH), 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. Calculate the van’t Hoff factor and the dissociation constant of acid.

0.6 mL of acetic acid (CH3COOH), 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. Calculate the van’t Hoff factor and the dissociation constant of acid.

Grade:11

2 Answers

Gaurav
askIITians Faculty 164 Points
6 years ago
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Yash Chourasiya
askIITians Faculty 256 Points
11 months ago
Hello Student

please see the solution in the attachment.
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I hope this Solution will help you.

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