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Chemistry chapter 12
| Question | Answer |
|---|---|
| solvent | solution component that determines the state of matter of the solution (present in greatest amount) |
| solute | substance dissolved in solvent |
| molarity | mol solute/volume solution |
| 1 ppm | 1mg/L |
| 1ppb | 1mu g/L |
| 1ppt | 1nano g/L |
| molarity | varies with temperature if temp increases, then molarity decreases |
| molality | mol solute/mass solvent, not temp dependent |
| mole fraction | xi is mol component i/total mols of solution |
| mole percent | mole fractionx100 |
| ideal solution | no net energy change and change in volume=0 |
| nonideal solution | volume is less than sum of volumes |
| ion-dipole forces | attraction of water dipoles for cations and anions |
| miscible | liquids that mix in all proportions |
| saturated | when equilibrium between undissolved solute and solution, solute has attained its maximum value |
| solubility | concentration of the solute |
| unsaturated | any solution containing less solute than can be held at equilibrium |
| ionic compound solubility | 95% of ionic compounds have solubilities that increase significantly w/increasing temp |
| solubility curve | graph of solubility as function of temperature |
| supersaturated | if a solution can be cooled without crystallization occurring |
| Henry's law | S=kPgas, increasing the pressure of a gas in contact w/saturated solution increases the number of molecules per unit volume in gas |
| colligative properties | properties that depend on # of solute particles present but not on the identity of solute |
| Raoult's law | Psolv=xsolv*Pat temp solv, vapor pressure of the solvent above a solution is the product of the vapor pressure of solvent and the mole fraction of the solvent in solution |
| Raoult's law | strictly followed only in an ideal solution. not limited to the solvent if a solution also contains volatile solutes |
| fractional distillation | use constant pressure and boil a solution in n aparatus that does vaporizations and condenstations at a constant temp. |
| Kf | molal freezing point depression constant and molal |
| Kb | boiling point elevation constant |
| Semipermeable membranes | sheets or films of amaterial containing a network of microscopic holes or pores through which small solvent molecues can pass, but larger solute molecules cannot |
| Osmosis | net flow of solvent molecules through a semipermeable membrance from a solution of lower concentration to a solution of higher concentration |
| osmotic pressure | pressure required to stop osmosis |
| pi | osmotic pressure in atm |
| pi=MRT | (blank) |
| isotonic | solution hqving same osmotic pressure as body flluids |
| hypertonic | solution has higher pressure than red blood cells |
| hypotonic | solution has less pressure than red blood cells |
| can't Hoff Factor | (i) used to modify equations for colligative properties by accounting for the presence of ions in solution |
| heterogeneous mixture | sand-water mix |
| colloids | mixtures that lie between true solutions and suspensions |
| colloid | dispersion in an appropriate medium of particles ranging in size from 1 nm to 1000 nm |
| tyndall effect | properties of colloids are diff from true solutions and suspensions. sometimes appear milky/cloudy and scater beams of light passing through them |
| coagulate/precipitate | high concentration of an electrolyte can cause this |
| electrodialysis | process facilitated by the attractions of ions to an electrode having the opposite charge |
Created by:
jlvon425
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