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CHEM212
MODULE 2
| Term | Definition |
|---|---|
| Colligative Properties | properties that depend on the number of solute particles, not their chemical identity |
| Strong electrolytes dissociate ________________ in water | completely |
| Weak electrolytes dissociate __________________ in water | very little |
| Solutions of nonvolatile nonelectrolytes contain solutes | that are not ionic, that do not volatilize |
| The vapor pressure of a solution of nonvolatile nonelectrolyte is always __________than the vapor pressure of the pure solvent | lower |
| The entropy of a solution is ____________ than that of a pure solvent | higher |
| the change of entropy when forming a gas from a solution (= entropy of valorization) is ____________ | lower |
| Raoult's law | Psolvent = Xsolvent x P°solvent |
| A solution always boils at a ___________ temperature than the pure solvent | higher |
| The boiling point elevation is ____________________ to the molality of the solution | proportional |
| Tb = Kbm Kb = ____?___ | molal boiling point elevation constant for the solvent |
| The freezing point (Tf) of a solution is the temperature at which the vapor pressure of the solution = _________________________________ | the vapor pressure of the solvent (when solid solvent and liquid solution coexist) |
| The freezing point depression is ____________________ to the molality of the solution | proportional |
| Tf = Kfm Kf = _____?_______ | molal freezing point depression constant for the solvent |
| Osmosis | movement of solvent particles from a higher concentration to a lower concentration through a semipermeable membrane |
| The solvent flows from a more dilute solution to a more ___________________ one | concentrated |
| Osmotic pressure Π) = | pressure to apply to oppose the flow of solvent |
| (Osmotic pressure)Π = MRT | M = molarity R = 0.0821 atm‐L/mol‐K T = Kelvin temperature |
| Water molecules pass through the semipermeable membrane, but | larger sugar molecules do not |
| The net flow of water increases... | ....the level of the solution |
| The osmotic pressure is measured by.... | ....the difference of the liquid levels at equilibrium |
| Reverse osmosis = | filtration system to remove salts from water by pushing water molecules under pressure through a semi‐permeable membrane |
| As the process progresses, the concentration of untreated water increases, until the osmotic pressure = | external pressure |
| P external = Π = MRT | M = molarity R = 0.0821 atm‐L/mol‐K T = Kelvin temperature |
| Each colligative property arises because.... | ....solute particles cannot move between two phases |
| By measuring a colligative property, one can determine... | the amount (mol) of solute particles and, with the mass of solute, the molar mass |
| For a volatile nonelectrolyte, the vapor of the solution contains both | the solute and the solvent |
| In such a solution, the vapor phase has a different composition than the liquid solution → | the vapor contains more of the more volatile component |
| van't Hoff factor (i) = | = number of ions formed from one solute particle |
| Most strong electrolyte solutions are not ideal: | the measured value of i is lower than the value from the formula |
| Solution = | = homogenous mixture: atoms, ions, or small molecules in solution (particles are invisible) |
| Colloid = | = heterogeneous mixture: particles are larger than simple molecules. but too small to settle out |
| Suspension = | = heterogeneous mixture: particles are large enough (>1000 nm) to be visible and settle down |
| Tyndall effect | Light passing through a colloid is scattered by the dispersed particles |
Created by:
manalkhalid
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