Term
| a property of a solution that depends only upon the number of solute particles, and not upon their identities; the boiling-point elevation, freezing-point depression, and vapor-pressure lowering |
|
Definition
|
|
Term
| what are three important colligative properties? |
|
Definition
| vapor pressure lowering, boiling point elevation, freezing point depression |
|
|
Term
| what is the decrease in a solutions vapor pressure proportional? |
|
Definition
| the number of particles the solute makes in solution |
|
|
Term
| the difference in temperature between the freezing point of a solution and the freezing point of the pure solvent |
|
Definition
| freezing point depression |
|
|
Term
| what is the magnitude of the freezing point depression proportional to? |
|
Definition
| the number of solute particles dissolved in the solvent and does not depend on their identity |
|
|
Term
| the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent |
|
Definition
|
|
Term
| what is the magnitude of the boiling point elevation proportional to? |
|
Definition
| the number of soulte particles dissolved in the solvent |
|
|
Term
|
Definition
| the pressure exerted by a vapor that is in dynamic equilibrium with its liquid in a closed system |
|
|
Term
|
Definition
|
|
Term
| do nonvolatile solutions have a higher or lower vapor pressure? |
|
Definition
|
|
Term
| what are two volatile substances? |
|
Definition
| glucose and sodium chloride |
|
|
Term
| do ionic solutes in solutions have a greater effect vapor pressure than other solutes? |
|
Definition
|
|
Term
| why would NaCl lower the vapor pressure of a solution twice as much as potassium? |
|
Definition
| NaCl has two different elements and potassium only has one |
|
|
Term
| what happens to the structure of the particles of a substance when it freezes? |
|
Definition
| the particle structure becomes more organized |
|
|
Term
| whaat does a solute in water do to the structuring of the particles when the liquid turns to a solid? |
|
Definition
| it disrupts the arrangment of the particles and more energy must be withdrawn for the structure to happen |
|
|
Term
| do solutions have a lower or higher freezing point than solvents? |
|
Definition
|
|
Term
| how much does one mole of solute lower the freezing point of water? |
|
Definition
| 1.86 degrees celsius per 1000 grams of water |
|
|
Term
| how many degrees does the addition of 2 moles of solute lower the freezing point? |
|
Definition
| 2 times 1.86 degrees celsius per 1000 grams of water |
|
|
Term
| how many degrees does the boiling point rise when 1 mole of solute is added? |
|
Definition
| 0.512 degrees celsius per 1000 grams of water |
|
|
