Q55.A 0. 5 percent solution of potassium chloride was found to freeze at −0. 24 °C. The percentage dissociation of potassium chloride is (Nearest integer) (Molal depression constant for water is 1. 80 K kg mol−1 and molar mass of KCl is 74. 6 g mol−1 )
What This Question Tests
This question assesses the ability to calculate the percentage dissociation of an electrolyte using the colligative property of depression in freezing point and the Van't Hoff factor.
Concepts Tested
Formulas Used
ΔTf = i Kf m
i = 1 + (n-1)α
molality = (mass of solute / molar mass of solute) / mass of solvent (kg)
📚 NCERT Sections This Tests
1.32 — Calculate The Depression In The Freezing Point Of Water When 10 G Of
Chemistry Class 11 · Chapter 1
1.32 Calculate the depression in the freezing point of water when 10 g of CH3CH2CHClCOOH is added to 250 g of water. Ka = 1.4 × 10–3, Kf = 1.86 K kg mol–1. 1.33 19.5 g of CH2FCOOH is dissolved in 500 g of water. The depression in the freezing point of water observed is 1.00 C. Calculate the van’t Hoff factor and dissociation constant of fluoroacetic acid.
2.8 — The Conductivity Of 0.20 M Solution Of Kcl At 298 K Is 0.0248 S Cm–1. Calculate
Chemistry Class 11 · Chapter 2
2.8 The conductivity of 0.20 M solution of KCl at 298 K is 0.0248 S cm–1. Calculate its molar conductivity.
1.34 — Vapour Pressure Of Water At 293 K Is 17.535 Mm Hg. Calculate The Vapour
Chemistry Class 11 · Chapter 1
1.34 Vapour pressure of water at 293 K is 17.535 mm Hg. Calculate the vapour pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water.
📋 Question Details
- Chapter
- Solutions
- Topic
- Colligative properties (Depression in freezing point)
- Year
- 2022
- Shift
- 26 Jun Shift 1
- Q Number
- Q55
- Type
- Numerical
- NCERT Ref
- Class 12 Chemistry Ch 2: Solutions
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