M 1 V 1 = M 2 V 2 6. If you dilute 50 mL of a 6 M solution to make 200 mL solution, what is the molarity of the new solution?
7. How many grams of magnesium sulfate would be dissolved in 1 L to make a 0.3 M solution?
8. If 0.65 g of a gas dissolves in 1 L of water at 2 atmospheres of pressure, how much will dissolve at 22 atmospheres of pressure?
15.3 Colligative Properties Colligative = “depends on the collection” Properties that depend on how many solute particles are present Does NOT depend on identity of solute
Vapor Pressure Lowering Vapor pressure = pressure created by particles going from liquid to gas inside a closed container If you add solute, not as much solvent can escape into the gas phase Pure solvent Solution
Boiling Point Elevation Boiling = liquid to gas The more solute added to a solution, the lower the vapor pressure and therefore the higher the boiling point Solution
A solvent has a boiling point of 200°C. When 10 grams of salt is dissolved in the solvent, what is the most likely new boiling point? a. 210°C b. 200°C c. 190°C
Freezing Point Depression Freezing = solvent particles moving into solid crystalline form Solute gets in the way of making crystals preventing the solvent from freezing. Lower temperature is needed to freeze
A solvent has a freezing point of 10°C. What is the most likely freezing point if 5 grams of salt is mixed with the solvent? a. 5°C b. 10°C c. 15°C
Osmotic Pressure Increase Osmosis-movement of water from low to high concentration. Goal is to balance the concentrations Osmotic Pressure Increases