1. Solutions

2. SoluteSolven t Solubility ConcentratedDilute : the ability to be dissolved temperature dependent a lot of solute little solute gets dissolved does the dissolving Solutions Homogeneous mixture made of two or more substances (aq) Solid-solid Solid -liquid Liquid-liquid Liquid-gas Gas-gas

3. miscible immiscible tincture unsaturated saturatedsupersaturated -does not hold the maximum -more can be dissolved -Under the line -does hold the maximum -no more can be dissolved -on the line -holds more than the maximum -no more can be dissolved -fallout, b/c unstable -above the line = g/100g H 2 O temperature Two substances that can be mixed together Two substances that can not be mixed together Solvent is alcohol - MUST BE HEATED AND THEN COOOLED

4. Table G- Solubility Curve

5. Factors that Influence Solubility Solubility Factors that increase the dissolving rate Solids Gas Temperature Pressure the ability to be dissolved temperature dependent Like dissolves like temperature Surface area Agitation Increase pressure No effect on the solubility of a solid Increase pressure Increase the solubility of a gas Increase Temperature Increase the solubility of a solid Increase Temperature decrease the solubility of a gas Polar solvents dissolve polar and ionic substances Non-Polar solvents dissolve non-polar substances

6. Measuring Concentration What is the molarity of a solution that has 25 g of NaCl dissolved in 500 ml of water? The concentration of solute in solution expressed as number of moles of solute dissolved in 1 liter of solution. Moles per liter Symbol M moles of solute liters of solution M= Molarity Percent by Mass The concentration of a solution is expressed as a percent (mass/mass) Percent by Mass = Mass of solute Mass of solution What is the % mass of 58g of glucose in a 2000g Solution? x 100 Parts Per Million A unit of concentration that expresses the mass of a solute dissolved in 1 million parts of a very dilute solution. Ppm= Grams of solute Grams of solution x 1,000,000 25/58= 0.43 mol 500/1000= 0.5L 0.43 = 0.86M 0.5 58 2000 X 100 2.9% How many parts per million are in a solution of 10g of NaCl in 100g of water? 10 X 1,000,000 110 90,909ppm

7. Effect of Ionic Substances on the Boiling and freezing point : The more ions you have the higher the boiling point and the lower the freezing point!!!

8. Colligative Properties-- factors that determine boiling and freezing point of a liquid by the changing the concentration of solute (number of particles) When a nonvolatile solute is added to a solvent, the freezing point will decrease Freezing Point Depression Boiling Point Elevation When a nonvolatile solute is added to a solvent, the boiling point will increase Effect of Electrolytes A solution that can conduct electricity due to the presence of ions Ionic-- metal/nonmetal --- splits NaCl --- Na + + Cl - --- 2 particles Covalent --nonmetals -- do not split C 6 H 12 O 6 ---C 6 H 12 O 6- --- 1 particle Need to look at how many particles are produced when solute dissolved Other examples: Ba(NO 3 ) 2 ------Ba 2+ + 2 NO 3- -----3 particles- CH 3 OH----- does not split ---CH 3 OH one particle The more particles you have, the greater the change

9. Molarity by Dilution- Concentrated solutions can be mixed with solvent to make weaker or dilute solutions. In dilutions the amount of solvent is increased, but the amount of solute is kept constant. The result is a decreased concentration, but a greater volume. number moles original = number of moles final Use the following formula: M 1 V 1 =M 2 V 2 M 1 = original concentration V 1 = original volume M 2 = final concentration V 2 = final volume Ex. You have 53 ml of a 1.5 M solution of NaCl, but 0.8 M solution is needed. How many ml of 0.8 M can you make? M 1 V 1 =M 2 V 2 (1.5M) (53mL) = (0.8M)x 79.5 =0.8x 99.4mL