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Solutions Test Revew

Solutions Test Revew. Chemistry 2010. Vocabulary: matching. Saturated solution: solution containing the maximum amount of solute that can be dissolved at a given temperature Unsaturated solution: contains less solute that can be theoretically dissolved at a given temperature.

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Solutions Test Revew

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  1. Solutions Test Revew Chemistry 2010

  2. Vocabulary: matching • Saturated solution: solution containing the maximum amount of solute that can be dissolved at a given temperature • Unsaturated solution: contains less solute that can be theoretically dissolved at a given temperature. • Supersaturated solution: contains more solute that can be theoretically dissolved at a given temperature

  3. Concentrated solution: a solution with a large amount of solute compared to solvent • Dilute solution: contains only a small amount of the maximum solute that can be dissolved at a given temperature • Miscible: describes liquids that dissolve in each other • Immiscible: describes liquids that are insoluble in each other • Colligative properties: depend upon the number of particles of solute in solution • Molarity: moles of solute per 1 liter of solution • Henry’s Law: at a given temperature the solubility of a gas is directly proportional to the pressure of the gas above the liquid

  4. Multiple Guess facts: need to know • Increasing the temperature of a liquid-solid solution will increase the rate of dissolving and the amount of crystalline material that dissolves • Agitating, crushing, and heating increase the rate of dissolving • As pressure of a gas decreases above a solution solubility into the liquid decreases proportionally (Henry’s Law) • If solubility of a gas is 1g/L @ 100 Kpa of pressure what pressure would be required to increase solubility to 3g/L

  5. Name the three colligative properties: boiling point elevation, freezing point depression, vapor pressure lowering • The more particles an ionic compound breaks into the more it will change the colligative properties (ex: CaCl2 = 3 particles, NaCl =2, C6H12O6 = 1) • Molarity = moles/liter • Ex: 50 moles in 10L = 50moles/10L = 5M • Molality = moles of solute/1kg of solvent 116g NaCl in 450mL(.450kg) of water = 2 moles of NaCl/.450kg = 4.44 molal or 4.44m • Percent (mass/volume) is based on mass of solute/mL of solvent. Remember I mL of water weights 1 gram • Ex: 30 grams of solute in 150mL of water = 30/150 = .20 x 100/% = 20%

  6. To turn an unsaturated solution into a saturated solution: add solute, or lower the temperature • Study notes from today and review sheet, test next class • No net ionic equations on test • Questions ???????

  7. Practice

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