This page covers CAPF AC Solutions with complete concept notes, 16 graded practice MCQs, key points and exam-specific tips. Free to study.
16graded MCQs · easy to hard · full solution & trap analysis
A solution is prepared by dissolving 68 g of sucrose (C₁₂H₂₂O₁₁) in sufficient water to make 500 mL of solution. Calculate the molarity. (Molar mass of sucrose = 342 g/mol)
A solution contains 36 g of glucose (C₆H₁₂O₆) dissolved in 1000 g of water. Calculate the molality of the solution. (Molar mass of glucose = 180 g/mol)
Which of the following is a colligative property of solutions?
A 2.0 M solution of NaCl is prepared. What is the mass of NaCl required to prepare 500 mL of this solution? (Molar mass of NaCl = 58.5 g/mol)
What is the mole fraction of solute in a solution containing 46 g of ethanol (C₂H₅OH) dissolved in 72 g of water? (Molar mass: ethanol = 46 g/mol, water = 18 g/mol)
A solution is prepared by dissolving 5.85 g of NaCl in 1 L of water. If the density of the solution is 1.005 g/mL, what is the molarity of the solution? (Molar mass of NaCl = 58.5 g/mol)
Which of the following is NOT a colligative property of solutions?
If the osmotic pressure of a solution at 27°C is 4.92 atm, what is the molarity of the solution? (R = 0.082 L·atm·mol⁻¹·K⁻¹)
A solution contains 36 g of glucose (C₆H₁₂O₆) dissolved in 1000 g of water. What is the molality of this solution? (Molar mass of glucose = 180 g/mol)
The freezing point of a 0.5 m aqueous solution of a non-electrolyte is lowered by approximately:
Which term describes the pressure required to prevent the flow of solvent into a solution across a semipermeable membrane?
A solution prepared by dissolving 34.2 g of sucrose (C₁₂H₂₂O₁₁) in 200 mL of water has what approximate mass percentage of sucrose? (Molar mass of sucrose = 342 g/mol; assume density of solution ≈ 1 g/mL)
The van't Hoff factor (i) for a 0.1 m CaCl₂ solution is approximately 3. What is the freezing point depression of this solution? (Kf = 1.86 K·kg·mol⁻¹)
A solution is prepared by dissolving 6.84 g of a solute in 100 g of water at 25°C. If the relative molecular mass of the solute is 228 and the density of the solution is 1.08 g/mL, calculate the molality of the solution.
At 20°C, the solubility of KNO₃ is 13.3 g per 100 g of water. What is the mass percentage of KNO₃ in a saturated solution at this temperature?
An aqueous solution contains 5.85 g of NaCl (M = 58.5 g/mol) dissolved in 500 mL of water. Assuming the density of the solution is 1.02 g/mL, calculate the molarity of the NaCl solution.