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Chem 2 ch 12
Chapter 12
Question | Answer |
---|---|
What Is a Solution? | A homogeneous mixture of 2 or more substances. |
What is a solute? | the substance present in the smaller amout. |
What is a solvent? | Substance present in larger amount. |
Exothermic | to release heat. |
Endothermic | absorbs heat |
Solubility | the measure of how much solute will dissolve at a specific temperature. |
saturated solution | contains the maximum amount of solute that will dissolve in a given solution. |
Unsaturated Solution | contains less solute the the solvent had the capacity to dissolve at a specific temperature |
supersaturated solution | contains more solute than is present in a saturated solution at a specific temperature. |
Crystallization | the process in which dissolved solute comes out of the solution and forms crystals |
miscible | two liquids that are completely soluble in each other in all proportions |
solvation | the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner. |
Hydration | when water is the solvent |
mole | number of grams/ molar mass |
like dissolves like | two substances with similar intermolecular forces are likely to be soluble in each other. |
concentration | is the amount of solute present in a given quantity of solution |
percent by mass | mass of solute/mass of the solution x 100 |
mole fraction | Xa= moles of a/ sum of all components |
molarity | moles of solute/Liters of solution |
molality | moles of solute/mass of the solvent (kg) |
Henry's Law | solubility of a gas in a liquid is proportional to the pressure of the gas over the solution c=kp |
c | the concentration of dissolved gas (mol/L) |
P | the pressure of gas over the solution (atm) |
k | is the constant for each gas (mol/L.atm) that depends only on the temperature |
colligative properties | properties that depend only on the number of solute particles in solution and not the nature of the solute particles |
Vapor-Pressure Lowering | P1=x1p°1 |
P1 | vapor pressure of solvent over a solution |
X1 | mole fraction of the solvent |
P°1 | vapor pressure of pure solvent |
ideal solution | any solution that obeys Raoult's law |
fractional distillation | a procedure for separating liquid components of a solution based on their different boiling points |
boiling-point elevation | (delta Tb) the boiling point of the solution (Tb) minus the boiling point of the pure solvent (t0b) deltaTb=KbMi |
Freezing-point depression | the freezing point of pure solvent (Tfo) minus the freezing point of the solution (Tf) DeltaTf=Kfmi |
osmotic pressure | The pressure require to stop osmosis. pi=MRTi |
Osmosis | is the selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one |
Semipermeable membrane | allows the passage of solvent molecules but blocks the passage of solute molecules |
M | molarity of the solution |
R | the gas constant (0.0821L.atm/k.mol) |
T | is the temperature in K. |
Van't Hoff factor | actual number of particles in soln after dissociation/number of formula units initially dissolved in soln |
colloid | is a dispersion of particles of one substance throughout a dispersing medium of another substance |
volatile | have a measurable vapor pressure |
nonvolatile | no measurable vapor pressure |
isotonic | two solutions of equal concentration that have the same osmotic pressure |
hypertonic | the more concentrated solution |
hypotonic | the less concentrated soulution |
crenation | process that causes cells to shrink and eventually to cease functioning |
ion pairs | made up of one or more cations and one or more anions held together by electrostatic forces. |
hydrophilic | water loving |
hydrophobic | water-fearing |
Tyndall Effect | the scattering of the visible light by colloid particles |
Roault's Law | the vapor pressure of the solvent over a solution is given of the pure solvent and the mole fraction of the solvent in the solution. |