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Solutions

Solutions. Outline Solutions Units of Concentration Colligative Properties. Chapter 12. What are the types of colloids?. Aerosol – liquid in gas. Solid Aerosol – solid in gas. Sol -- solid in liquid like protein particles in milk.

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Solutions

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  1. Solutions Outline Solutions Units of Concentration Colligative Properties Chapter 12

  2. What are the types of colloids? Aerosol – liquid in gas Solid Aerosol – solid in gas Sol -- solid in liquid like protein particles in milk

  3. Emulsion – liquid in liquid like oil droplets in mayonnaise. Foams – gases in liquids like whipped cream Solid emulsion – liquid in a solid like milk in butter Gel – a solid emulsion which is soft but holds its shape like Jell-O

  4. What type of mixture exhibits the Tyndall Effect?

  5. What is Brownian motion? Tro: Chemistry: A Molecular Approach, 2/e

  6. How do mixtures differ?

  7. How does the solubility of a solid change with increasing temperature?

  8. What are the three types of solutions?

  9. How does temperature affect gas solubility?

  10. How does gas solubility change with increasing temperature?

  11. How does pressure affect gas solubility?

  12. How does changing the pressure affect equilibrium?

  13. Chapter 12: Examples – Henry’s Law The solubility of pure nitrogen gas at 25 ˚C and 1.00 atm is 6.8 x 10-4 mol/L. What is the solubility of nitrogen gas under those conditions if the partial pressure of nitrogen gas is 0.78 atm?

  14. What interactions must be overcome for an ionic compound to dissolve?

  15. Are solute-solute interactions exothermic or endothermic?

  16. Are solvent-solvent interactions exothermic or endothermic?

  17. Are solute-solvent interactions exothermic or endothermic?

  18. Chapter 12: Examples – Units of Concentration 28.0g of NaF are dissolved in 455g of water. What is the % concentration of this solution?

  19. Chapter 12: Examples – Units of Concentration How many grams of water are required to dissolve 13.00 g of KOH in order to prepare a 7.0% KOH solution?

  20. Chapter 12: Examples – Units of Concentration What is the molarity of a 1.2% NaCl solution? The density of this solution is 1.02 g/mL.

  21. Chapter 12: Examples – Units of Concentration How many grams of NH4Cl are in 313 mL of a 12.00% ammonium chloride solution? The density of this ammonium chloride solution is 1.05g/mL.

  22. Chapter 12: Examples – Units of Concentration How many grams of water should you add to 32.5 g of sucrose, C12H22O11, to get a 0.85 m solution?

  23. Chapter 12: Examples – Units of Concentration What is the molality of a 40% ethylene glycol, C2H6O2, solution?

  24. Chapter 12: Examples – Units of Concentration A 0.944 M solution of glucose, C6H12O6, in water has a density of 1.0624 g/mL at 20°C. What is the concentration in: mass percent, mole fraction, and molality?

  25. New equilibrium Pure solvent and nonvolatile solute pure solvent at equilibrium How does the vapor pressure change when a nonvolatile solute is added to the solvent?

  26. What does the distilled water transfer to the seawater?

  27. How do ions affect the van’t Hoff factor? Tro: Chemistry: A Molecular Approach, 2/e

  28. How does a solute change the phase diagram of a solvent?

  29. How do intermolecular forces affect Raoult’s Law?

  30. How does a volatile solute affect a solution’s vapor pressure? • P total = PA + PB • PA = (XA)(PAo) • PB = (XB)(PBo) • PAo is the vapor pressure of the pure solvent.

  31. Chapter 12: Examples – Colligative Properties Calculate the vapor pressure of water at 100 ˚C of a solution prepared by dissolving 5.00 g sucrose, C12H22O11, in 100 g water. The vapor pressure of the pure solvent is 760 torr.

  32. Chapter 12: Examples – Colligative Properties A solution was prepared by adding 20.0 g of urea to 125 g of water at 25 °C, a temperature at which pure water has a vapor pressure of 23.76 torr. The observed vapor pressure of the solution was found to be 22.67 torr. Calculate the molar mass of urea.

  33. How does a solution’s molality affect it’s freezing point?

  34. Chapter 12: Examples – Colligative Properties Calculate the boiling point of a solution containing 100 g of ethylene glycol (C2H6O2 ) in 900 g water. kbwater = 0.512 ˚C/m.

  35. Chapter 12: Examples – Colligative Properties An elemental analysis of adrenaline is 59.0% C, 26.2% O, 7.10% H, and 7.60% N by mass. When 0.64 g of adrenaline was dissolved in 36.0 g benzene, kf = 5.12 ˚C/m, the freezing point decreased by 0.50 ˚C. What is the molecular formula?

  36. What is osmotic pressure?

  37. What is osmotic pressure?

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