Q59.The overall stability constant of the complex ion [Cu (NH3)4]2+ is 2. 1 × 1013. The overall dissociation constant is y × 10−14 . Then y is (Nearest integer)
What This Question Tests
This question requires the calculation of the freezing point of a solution using the colligative property of freezing point depression, involving molality calculation.
Concepts Tested
Formulas Used
ΔT_f = i * K_f * m
m = moles solute / kg solvent
📚 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.
5.28 — How Many Ions Are Produced From The Complex Co(Nh3)6Cl2 In Solution?
Chemistry Class 11 · Chapter 5
5.28 How many ions are produced from the complex Co(NH3)6Cl2 in solution? (i) 6 (ii) 4 (iii) 3 (iv) 2 139 Coordination Compounds Reprint 2025-26
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
- Solutions
- Topic
- Freezing point depression
- Year
- 2021
- Shift
- 26 Aug Shift 2
- Q Number
- Q59
- Type
- Numerical
- NCERT Ref
- Class 12 Chemistry Ch 2: Solutions
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