Q56. C6H6 freezes at 5. 5°C. The temperature at which a solution of 10 g of C4H10 in 200 g of C6H6 freeze is _______ ∘C. (nearest integer value), (The molal freezing point depression constant of C6H6 is 5. 12°C/m.)
What This Question Tests
This question involves calculating the solubility of a sparingly soluble salt (PbI2) in the presence of a common ion from a strong electrolyte, demonstrating the common ion effect.
Concepts Tested
Formulas Used
Ksp = [Pb2+][I−]2
📚 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.
1.35 — Henry’S Law Constant For The Molality Of Methane In Benzene At 298 K Is
Chemistry Class 11 · Chapter 1
1.35 Henry’s law constant for the molality of methane in benzene at 298 K is 4.27 × 105 mm Hg. Calculate the solubility of methane in benzene at 298 K under 760 mm Hg.
1.27 — If The Solubility Product Of Cus Is 6 × 10–16, Calculate The Maximum Molarity Of
Chemistry Class 11 · Chapter 1
1.27 If the solubility product of CuS is 6 × 10–16, calculate the maximum molarity of CuS in aqueous solution.
📋 Question Details
- Chapter
- Ionic Equilibrium
- Topic
- Solubility and solubility product
- Year
- 2021
- Shift
- 24 Feb Shift 2
- Q Number
- Q56
- Type
- Numerical
- NCERT Ref
- Class 11 Chemistry Ch 7: Ionic Equilibrium
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