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Class 12 · Chemistry
→If 20% of a substance forms tetramers, what is the van’t Hoff factor?
Class 12 · Chemistry
→If the observed molar mass in a solution is 1.25 times the normal molar mass, what is the van’t Hoff factor i?
Class 12 · Chemistry
→When 1.6 g of a substance is dissolved in 200 g of water, the freezing-point depression is 0.744 K. If the normal molar mass is 80 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹, what is the van’t Hoff factor i?
Class 12 · Chemistry
→A 0.05 mol kg⁻¹ solution is prepared by dissolving 3.0 g of a nonelectrolyte in 500 g of solvent. What is the molar mass of the solute?
Class 12 · Chemistry
→The observed molar mass of a substance is 50 g mol⁻¹ and its van’t Hoff factor is 2.4. What is its normal molar mass?
Class 12 · Chemistry
→A solution contains 0.6 g of a solute in 0.2 L of solution. If its osmotic pressure at 300 K is 0.369 atm, what is the molar mass? Use R = 0.082 L atm K⁻¹ mol⁻¹.
Class 12 · Chemistry
→In a boiling-point elevation problem, w₂ = 2.0 g solute, w₁ = 400 g solvent, Kb = 0.52 K kg mol⁻¹, and ΔTb = 0.026 K. What is the molar mass of the solute?
Class 12 · Chemistry
→A solution contains 1.0 g solute in 100 g water. If Kf = 1.86 K kg mol⁻¹, the depression in freezing point is 0.093 K, and the normal molar mass is 100 g mol⁻¹, what is the van’t Hoff factor?
Class 12 · Chemistry
→If the observed molar mass of an AB₃ salt is half of its normal molar mass, what is the degree of dissociation?
Class 12 · Chemistry
→A salt of type AB₃ undergoes 50% dissociation. If its normal molar mass is 200 g mol⁻¹, what will be its observed molar mass?
Class 12 · Chemistry
→A 0.2 M electrolyte has an osmotic pressure of 7.38 atm at 300 K. If R = 0.082 L atm K⁻¹ mol⁻¹, what is i, and what type of dissociation does it indicate?
Class 12 · Chemistry
→When 1.5 g of a non-electrolyte substance is dissolved in 250 g of a solvent, the depression in freezing point is 0.1116 K. If the cryoscopic constant of the solvent is 1.86 K kg mol⁻¹, what is the molar mass of the substance?
Class 12 · Chemistry
→A solution contains 2.0 g solute in 100 g solvent. If the observed molar mass is 80 g mol⁻¹ and the normal molar mass is 120 g mol⁻¹, what is the ratio of normal molality to effective molality?
Class 12 · Chemistry
→A 3.0 g solute dissolved in 100 g solvent forms a 0.3 m solution. If the solution shows i = 2 in colligative-property measurements, what is its effective molality?
Class 12 · Chemistry
→A 0.05 M solution has an osmotic pressure of 2.46 atm at 300 K. Taking R = 0.082 L atm K⁻¹ mol⁻¹, what are the van’t Hoff factor and the effective number of solute particles?
Class 12 · Chemistry
→When 0.8 g of a substance is dissolved in 200 g of water, the depression in freezing point is 0.186 K. If the actual molar mass is 40 g mol⁻¹ and Kf = 1.86 K kg mol⁻¹, what is the behaviour of the solute?
Class 12 · Chemistry
→When 1.0 g of a nonelectrolyte is dissolved in 50 g camphor, the freezing-point depression is 8 K. If K_f = 40 K kg mol⁻¹ for camphor, what is the molar mass of the substance?
Class 12 · Chemistry
→For a solution, the observed freezing-point depression is 0.558 K. For the same amount assuming normal behaviour, the expected depression is 0.372 K. What is the van’t Hoff factor?
Class 12 · Chemistry
→If a 0.2 M nonelectrolyte solution has an osmotic pressure of 4.92 atm at 300 K, what will be the osmotic pressure of a 0.1 M solute with i = 3 at the same temperature?
Class 12 · Chemistry
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