4 - Solutions Flashcards
Solution=
Solvent=
Solute=
*if neither dominates they are both called the ______.
Colloid=
Solution= is a homogenous mixture of two or more compounds in a single phase, such as solid, liquid, or gas.
Solvent= in a solution the compound of which there is more is called the solvent.
Solute= in a solution the compound of which there is less is called the solute.
*if neither dominates they are both called the solvents.
Colloid= like a solution, only that the solute particles are larger. But these particles are usually too small to be extracted by filtration but usually large enough or charged enough to be separated by a semipermeable membrane.
*Like _________ like*
London dispersion forces=
Solvation=
Hydration=
Electrolyte=
*Like dissolves like*
London dispersion forces= nonpolar molecules held together by weak intermolecular bonds resulting from instantaneous dipole moments.
Solvation= when ionic compounds dissolve, they break apart into their respective cations and anions and are surrounded by the oppositely charged ends of the polar solvent.
Hydration= when several water molecules attach to one side of an ionic compound, they are able to overcome the strong ionic bond and break apart the compound. Something that is hydrated is said to be in aqueous phase.
Electrolyte= when ions form in aqueous solution, the solution is able to conduct electricity, a compound which forms ions in aqueous solution is called an electrolyte.
Molarity=
M=
Molality=
m=
Mole fraction=
x=
Molarity= the moles of the compound divided by the volume of solution
M= moles of solute
volume of solution
Molality= is moles of solute divided by kilograms of solvent.
m= moles of solute
kilograms of solvent
Mole fraction= is the moles of a compound divided by the total moles of all species in solution.
x= moles of solute
Total moles of all solutes and solvent
Mass percentage=
Mass %=
Parts per million (ppm)=
Ppm=
Mass percentage= is 100 times the ratio of the mass of the solute to the total mass of the solution.
Mass %= _mass of solute _ X 100
total mass of solution
Parts per million (ppm)= is 10^6 times the ratio of the mass of the solute to the total mass of the solution.
Ppm= _mass of solute _ X 10^6
total mass of solution
Formation of a solution:
1)
2)
3)
Formation of a solution:
1) breaking of intermolecular bonds between solute molecules. (endothermic)
2) breaking of intermolecular bonds between solvent molecules. (endothermic)
3) formation of intermolecular bonds between solvent and solute. (exothermic)
Heat of solution=
*When solutions form, _______ increases!
Heat of solution= negative heat of solution results in stronger intermolecular bonds (lower vapor pressure), while positive results in weaker bonds (increase vapor pressure).
*When solutions form, entropy increases!
Vapor pressure=
- vapor pressure increases with ________
- boiling occurs when the vapor pressure of the liquid equals the _________
- melting occurs when the vapor pressure of the solid phase equals the _______ of the liquid phase.
Nonvolatile solute=
Volatile solute=
Vapor pressure= the pressure created by the molecules in the open space.
- vapor pressure increases with temperature (endothermic process)
- boiling occurs when the vapor pressure of the liquid equals the atmospheric pressure.
- melting occurs when the vapor pressure of the solid phase equals the vapor pressure of the liquid phase.
Nonvolatile solute= a solute with no vapor pressure.
Volatile solute= a solute with a vapor pressure.
Raoult’s law= P (v)=
P (v)=
- if 97% of the solution is solvent, then vapor pressure will be 97% of the vapor pressure of the __________
- if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the ______ PLUS 3% of the vapor pressure of the __________
Raoult’s law= P (v)= X (a)P (a)
P (v)= X (a)P (a) + X (b)P (b)
- if 97% of the solution is solvent, then vapor pressure will be 97% of the vapor pressure of the pure solvent. (nonvolatile)
- if 97% of the solution is solvent, then the vapor pressure will be 97% of the vapor pressure of the pure solvent PLUS 3% of the vapor pressure of the pure solute. (volatile)
Solubility=
Precipitation=
Saturated=
Solubility product (Ksp)=
*solubility product changes only with _______, while solubility depends upon the temperature and the ____ in solution.
Solubility= is a solute’s tendency to dissolve in a solvent. (max number of moles of the solute that can dissolve in solution)
Precipitation= forming a solid again.
Saturated= when the rate of dissolution and precipitation are equal.
Solubility product (Ksp)= the equilibrium of a solvation reaction has its own equilibrium constant.
*solubility product changes only with temperature, while solubility depends upon the temperature and the ions in solution.
Spectator ions=
Common ion effect=
*common ion added to a saturated solution will shift the equilibrium increasing ______ but wont affect the Ksp. When added to a solution not in equilibrium it wont affect equilibrium because there is no equilibrium to shift.
*Henry’s law demonstrates that the solubility of a gas is proportional to its _______
*as temperature increases the solubility of salts generally _______.
*FOR GASES: as temperature increase the solubility of gases ________.
Spectator ions= ions that have no effect on the solution.
Common ion effect= the disturbance of the equilibrium.
*common ion added to a saturated solution will shift the equilibrium increasing precipitate but wont affect the Ksp. When added to a solution not in equilibrium it wont affect equilibrium because there is no equilibrium to shift.
*Henry’s law demonstrates that the solubility of a gas is proportional to its vapor partial pressure.
*as temperature increases the solubility of salts generally increases.
*FOR GASES: as temperature increase the solubility of gases decreases.
