Vapor Pressure of Solutions
Chemistry ⇒ Solutions and Colloids
Vapor Pressure of Solutions starts at 11 and continues till grade 12.
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A binary solution of liquids A and B has mole fractions X_A = 0.3 and X_B = 0.7. The vapor pressures of pure A and B are 120 mmHg and 80 mmHg, respectively. Calculate the total vapor pressure of the solution.
A solution contains 0.5 mol of benzene (P⁰ = 100 mmHg) and 0.5 mol of toluene (P⁰ = 32 mmHg). Calculate the total vapor pressure of the solution assuming ideal behavior.
A solution contains 1 mol of NaCl dissolved in 1000 g of water. If the vapor pressure of pure water is 23.8 mmHg, estimate the vapor pressure of the solution. (Assume complete dissociation of NaCl)
A solution is made by dissolving 2 mol of a non-volatile solute in 98 mol of water. If the vapor pressure of pure water is 30 mmHg, what is the vapor pressure of the solution?
A solution is made by dissolving 5 g of a non-volatile solute in 95 g of water. The vapor pressure of pure water is 25 mmHg. The vapor pressure of the solution is 24.5 mmHg. Calculate the molar mass of the solute.
A solution is prepared by dissolving 10 g of glucose (C₆H₁₂O₆) in 90 g of water at 25°C. The vapor pressure of pure water at 25°C is 23.8 mmHg. Calculate the vapor pressure of the solution. (Molar mass of glucose = 180 g/mol, water = 18 g/mol)
A solution is prepared by mixing 0.2 mol of ethanol (P⁰ = 44 mmHg) and 0.8 mol of water (P⁰ = 32 mmHg). Calculate the partial vapor pressure of ethanol in the solution.
A solution is prepared by mixing 0.4 mol of acetone (P⁰ = 200 mmHg) and 0.6 mol of chloroform (P⁰ = 150 mmHg). Assuming ideal behavior, calculate the partial vapor pressure of chloroform.
A solution of urea in water has a vapor pressure of 22.5 mmHg at 25°C. The vapor pressure of pure water at this temperature is 23.8 mmHg. Calculate the mole fraction of urea in the solution.
Define vapor pressure in the context of solutions.
Describe how Raoult's Law can be used to distinguish between ideal and non-ideal solutions.
Describe the difference between volatile and non-volatile solutes with respect to their effect on vapor pressure.
Describe the effect of temperature on the vapor pressure of a solution.
Explain the term 'non-volatile solute' with an example.
Explain the term 'relative lowering of vapor pressure' and give its mathematical expression.
Explain why solutions showing negative deviation from Raoult's Law have lower vapor pressure than predicted.
Explain why the addition of a non-volatile solute to a solvent lowers the vapor pressure of the solvent.
Explain why the vapor pressure of a solution is important in industrial applications such as distillation.
If a solution shows a positive deviation from Raoult's Law, what can you infer about the intermolecular forces between solute and solvent?
State Raoult's Law mathematically for a binary solution.
