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Properties of Solutions

Properties of Solutions. Classification of Matter. Solutions are homogeneous mixtures. Solute. A solute is the dissolved substance in a solution. Salt in salt water. Sugar in soda drinks. Carbon dioxide in soda drinks. Solvent. A solvent is the dissolving medium in a solution.

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Properties of Solutions

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  1. Properties of Solutions

  2. Classification of Matter Solutions are homogeneous mixtures

  3. Solute A solute is the dissolved substance in a solution. Saltin salt water Sugarin soda drinks Carbon dioxidein soda drinks Solvent A solvent is the dissolving medium in a solution. Waterin salt water Waterin soda

  4. Calculations of Solution Concentration Mass percent - the ratio of mass units of solute to mass units of solution, expressed as a percent

  5. Calculations of Solution Concentration Mole fraction – the ratio of moles of solute to total moles of solution

  6. Calculations of Solution Concentration Molality – moles of solute per kilogram of solvent

  7. Calculations of Solution Concentration Molarity - the ratio of moles of solute to liters of solution

  8. Heat of Solution TheHeat of Solutionis the amount of heat energy absorbed (endothermic) or released (exothermic) when a specific amount of solute dissolves in a solvent.

  9. Steps in Solution Formation H1Expanding the solute Separating the solute into individual components H2Expanding the solvent Overcoming intermolecular forces of the solvent molecules H3Interaction of solute and solvent to form the solution Salt dissolving Flash.swf

  10. “Like Dissolves Like” Nonpolar solutesdissolve best innonpolar solvents Polar and ionic solutesdissolve best inpolar solvents

  11. Predicting Solution Formation

  12. Solubility Trends • The solubility of MOST solids increases with temperature. • The rate at which solids dissolve increases with increasing surface area of the solid. • The solubility of gases decreases with increases in temperature. • The solubility of gases increases with the pressure above the solution.

  13. Therefore… Solids tend to dissolve best when: • Heated • Stirred • Ground into small particles Gases tend to dissolve best when: • The solution is cold • Pressure is high

  14. Saturation of Solutions • Asolution that contains the maximum amount of solute that may be dissolved under existing conditions issaturated. • A solution that contains less solute than a saturated solution under existing conditions isunsaturated. • A solution that contains more dissolved solute than a saturated solution under the same conditions issupersaturated.

  15. Solubility Chart

  16. Henry’s Law The concentration of a dissolved gas in a solution is directly proportional to the pressure of the gas above the solution Applies most accurately for dilute solutions of gases that do not dissociate or react with the solvent Yes  CO2, N2, O2 No  HCl, HI

  17. Raoult’s Law The presence of a nonvolatile solute lowers the vapor pressure of the solvent. Psolution=Observed Vapor pressure of the solution solvent=Mole fraction of the solvent P0solvent=Vapor pressure of the pure solvent

  18. Liquid-liquid solutions in which both components are volatile Modified Raoult's Law: P0is the vapor pressure of the pure solvent PAandPBare the partial pressures

  19. Raoult’s Law – Ideal Solution A solution that obeys Raoult’s Law is called an ideal solution

  20. Negative Deviations from Raoult’s Law Strong solute-solvent interaction results in a vapor pressure lower than predicted Exothermic mixing = Negative deviation

  21. Positive Deviations from Raoult’s Law Weak solute-solvent interaction results in a vapor pressure higher than predicted Endothermic mixing = Positive deviation

  22. Definition of Electrolytes and Nonelectrolytes An electrolyte is: • A substance whose aqueous solution conducts • an electric current. A nonelectrolyte is: • A substance whose aqueous solution does not • conduct an electric current. Try to classify the following substances as electrolytes or nonelectrolytes…

  23. Electrolytes vs. Nonelectrolytes The ammeter measures the flow of electrons (current) through the circuit. If the ammeter measures a current, and the bulb glows, then the solution conducts. If the ammeter fails to measure a current, and the bulb does not glow, the solution is non-conducting.

  24. Electrolytes? • Pure water • Tap water • Sugar solution • Sodium chloride solution • Hydrochloric acid solution • Lactic acid solution • Ethyl alcohol solution • Pure sodium chloride

  25. Answers to Electrolytes NONELECTROLYTES: ELECTROLYTES: • Pure water • Sugar solution • Ethanol solution • Pure NaCl • Tap water (weak) • NaCl solution • HCl solution • Lactate solution (weak)

  26. Colligative Properties Colligative properties are those that depend on the concentration of particles in a solution, not upon the identity of those properties. • Boiling Point Elevation • Freezing Point Depression • Osmotic Pressure

  27. Freezing Point Depression Each mole of solute particles lowers the freezing point of 1 kilogram of water by 1.86 degrees Celsius. Kf = 1.86 C  kilogram/mol m = molality of the solution i = van’t Hofffactor

  28. Boiling Point Elevation Each mole of solute particles raises the boiling point of 1 kilogram of water by 0.51 degrees Celsius. Kb = 0.51 C  kilogram/mol m = molality of the solution i = van’t Hofffactor

  29. Freezing Point Depression and Boiling Point Elevation Constants, C/m

  30. The van’t Hoff Factor, i Electrolytes may have two, three or more times the effect on boiling point, freezing point, and osmotic pressure, depending on its dissociation.

  31. Dissociation Equations and the Determination of i i = 2 NaCl(s)  Na+(aq) + Cl-(aq) i = 2 AgNO3(s)  Ag+(aq) + NO3-(aq) i = 3 MgCl2(s)  Mg2+(aq) + 2 Cl-(aq) i = 3 Na2SO4(s)  2 Na+(aq) + SO42-(aq) AlCl3(s)  Al3+(aq) + 3 Cl-(aq) i = 4

  32. Ideal vs. Real van’t Hoff Factor The ideal van’t Hoff Factor is only achieved in VERY DILUTE solution.

  33. Osmotic Pressure The minimum pressure that stops the osmosis is equal to the osmotic pressure of the solution

  34. Osmotic Pressure Calculations  = Osmotic pressure M = Molarity of the solution R = Gas Constant = 0.08206 Latm/molK  = Osmotic pressure

  35. Suspensions and Colloids Suspensions and colloids are NOT solutions. Suspensions: The particles are so large that they settle out of the solvent if not constantly stirred. Colloids: The particles intermediate in size between those of a suspension and those of a solution.

  36. Types of Colloids Types of Colloids

  37. The Tyndall Effect Colloids scatter light, making a beam visible. Solutions do not scatter light. Which glass containsa colloid? colloid solution

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