•phase of the solution •usually constitutes the largest proportion of the system in which the solute is dissolved

tyoes of solvent

proton accepting eg: acetone, ether, liquid ammonia

proton donating eg: formic, acetic, h2so4

both proton accepting and donating

neither proton accepting nor donating

types of solution according to solubility of solute

the solute is in EQUILIBRIUM with the solid phase

the solute is in CONCENTRATION BELOW that necessary for comolete saturation

the solute is in concentration ABOVE that necessary for complete saturation

when a non volatile solute is added to a volatile solvent, the solute reduces the escaping tendency of the solvent.

boiling point is when vapor pressure is equals to atmospheric pressure

freezing point is the temperature in which solid and liquid are in equilibrium under a pressure of 1 atm

osmosis: the movement of solvent from a higher to lower concentration

colligative properties

concepts in isotonicity

methods of determining tonicity

based on the effect of red blood cells suspended in solution

based on their COLLIGATIVE property, especially freezing point depression

theories of acids vs bases

substance that resist changes in pH •maintain pH •modify pH

capacity of substance to resist change in pH

the equation that can be used to estimate the pH of a buffered solution

attributed to the effects of the molecules found at the INTERFACE between two phases

liquid-to-liquid

solid to liquid; liquid to gas

attraction on the surface

rise of the liquid on the narrow tube

•surface active agents •lowers the interfacial, surface tension