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Chapter 11: Properties of Solutions

Chapter 11: Properties of Solutions. Types of Solutions Units of Concentration: molarity, mass %, mole fraction, molality, normality Heat of Solution Factors Affecting Solubility: structure, pressure, temperature P vap of solutions & Raoult’s Law

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Chapter 11: Properties of Solutions

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  1. Chapter 11: Properties of Solutions • Types of Solutions • Units of Concentration: molarity, mass %, mole fraction, molality, normality • Heat of Solution • Factors Affecting Solubility: structure, pressure, temperature • Pvap of solutions & Raoult’s Law • Colligative Properties: boiling point elevation, freezing point depression, osmotic pressure, colligative properties of electrolyte solutions

  2. Example 1 Find the molality of a mixture of CH3OH and C2H5OH if the mole fractions are 0.150 CH3OH and 0.850 C2H5OH. Answer: 3.83 m

  3. Example 2 Find the mass percent of NaCl in a 1.50 M NaCl solution. Assume the density of the solution is 1.00 g/mL. Answer: 8.77%

  4. Example 3 1.00 liter of H2O at 25°C dissolves 0.0404 g of O2 when the partial pressure of the O2 is 1.00 atm. Find the solubility of O2 in water if the O2 is in air where its partial pressure is 159 mmHg. Answer: 8.45x10-3 g/L

  5. Example 4 Calculate the vapor pressure lowering when 10.0 mL of glycerol (C3H8O3) is added to 500.0 mL of water at 50.0°C. At this temperature, the vapor pressure of pure water is 92.5 torr and its density is 0.988 g/mL. Glycerol is nonvolatile and has a density of 1.26 g/mL. Answer: 0.459 torr

  6. Example 5 When 11.2 g of sulfur are dissolved in 40.0 g of carbon disulfide, the boiling point of the CS2 increases by 2.63°C. What is the molecular formula of sulfur? Answer: S8

  7. Example 6 Find the osmotic pressure at 25.0°C of a solution containing 5.00 g of sugar (C12H22O11) in 100.0 mL of solution. Answer: 3.51 atm

  8. Example 7 If 8.5 g of horse hemoglobin is dissolved in 750 mL of water, the solution has an osmotic pressure of 3.1 mmHg at 25°C. What is the molecular weight of horse hemoglobin? Answer: 6.8 x 104 g/mole

  9. Example 8 Aqueous CaCl2 is used as a ballast in tractor tires. What molal concentration of CaCl2 is needed to prevent freezing down to -20.0°C? Assume i=3. Answer: 3.59 m

  10. Example 9 The freezing point of 0.109m formic acid is -0.210°C. Find the % of formic acid molecules that are ionized. Formic acid is HCHO2. Answer: 3.58%

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