Practice Solutions with authentic CBSE Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1, 2, 3 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of CBSE examiners.
When 19.5 g of F - CH2 – COOH (Molar mass = 78 g mol-1), is dissolved in 500 g of water, the depression in freezing point is observed to be 1oC. [Given: Kf for water = 1.86 K kg mol-1]
Calculate the degree of dissociation of F - CH2 - COOH.
What will be the van't Hoff factor for a dilute solution of K2SO4, assuming complete dissociation?
1.00 g of non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 K kg mol-1)
Assertion (A): Non-ideal solutions form azeotropic mixture.
Reason (R): Maximum boiling azeotropes are formed by a solution showing negative deviation.
A 10% solution (by mass) of sucrose in water has a freezing point of 269.15 K. Calculate the freezing point of 10% glucose in water, if freezing point of pure water is 273.15 K.
Calculate the freezing point of 10% glucose in water.
Calculate the van't Hoff factor for an unknown electrolyte if a 0.561m solution of it depresses the freezing point of water by 2.93°C. The freezing point depression constant (Kf) for water is 1.86°C kg mol^-1.
The depression in freezing point of water observed for the same amount of acetic acid, trichloroacetic acid and trifluoroacetic acid increases in the order given above.
Explain briefly why the depression in freezing point increases in the order: acetic acid < trichloroacetic acid < trifluoroacetic acid.
Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of KCl, which one will have higher boiling point and why?
Predict whether van't Hoff factor, (i) is less than one or greater than one in CH3COOH dissolved in water.
Predict whether van't Hoff factor, (i) is less than one or greater than one in CH3COOH dissolved in benzene.
15.0 g of unknown molecular material is dissolved in 450 g of water. The resulting solution freezes at - 0.34°C. (Kf for water = 1.86 K kg mol-1)
What is the molar mass of the material?
If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 L of water? Assume that N2 exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N2 at 293 K is 76.48 K bar.
Calculate the number of millimoles of N2 gas that would dissolve in 1 L of water under the given conditions.
The molecular masses of polymers are determined by the osmotic pressure method and not by measuring other colligative properties. Give two reasons.
Practice Solutions with authentic CBSE Chemistry exam questions for both SL and HL students. This question bank mirrors Paper 1, 2, 3 structure, covering key topics like atomic structure, chemical reactions, and organic chemistry. Get instant solutions, detailed explanations, and build exam confidence with questions in the style of CBSE examiners.
When 19.5 g of F - CH2 – COOH (Molar mass = 78 g mol-1), is dissolved in 500 g of water, the depression in freezing point is observed to be 1oC. [Given: Kf for water = 1.86 K kg mol-1]
Calculate the degree of dissociation of F - CH2 - COOH.
What will be the van't Hoff factor for a dilute solution of K2SO4, assuming complete dissociation?
1.00 g of non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 K kg mol-1)
Assertion (A): Non-ideal solutions form azeotropic mixture.
Reason (R): Maximum boiling azeotropes are formed by a solution showing negative deviation.
A 10% solution (by mass) of sucrose in water has a freezing point of 269.15 K. Calculate the freezing point of 10% glucose in water, if freezing point of pure water is 273.15 K.
Calculate the freezing point of 10% glucose in water.
Calculate the van't Hoff factor for an unknown electrolyte if a 0.561m solution of it depresses the freezing point of water by 2.93°C. The freezing point depression constant (Kf) for water is 1.86°C kg mol^-1.
The depression in freezing point of water observed for the same amount of acetic acid, trichloroacetic acid and trifluoroacetic acid increases in the order given above.
Explain briefly why the depression in freezing point increases in the order: acetic acid < trichloroacetic acid < trifluoroacetic acid.
Out of 0.1 molal aqueous solution of glucose and 0.1 molal aqueous solution of KCl, which one will have higher boiling point and why?
Predict whether van't Hoff factor, (i) is less than one or greater than one in CH3COOH dissolved in water.
Predict whether van't Hoff factor, (i) is less than one or greater than one in CH3COOH dissolved in benzene.
15.0 g of unknown molecular material is dissolved in 450 g of water. The resulting solution freezes at - 0.34°C. (Kf for water = 1.86 K kg mol-1)
What is the molar mass of the material?
If N2 gas is bubbled through water at 293 K, how many millimoles of N2 gas would dissolve in 1 L of water? Assume that N2 exerts a partial pressure of 0.987 bar. Given that Henry's law constant for N2 at 293 K is 76.48 K bar.
Calculate the number of millimoles of N2 gas that would dissolve in 1 L of water under the given conditions.
The molecular masses of polymers are determined by the osmotic pressure method and not by measuring other colligative properties. Give two reasons.