molarity

(a)  

making a solution common mistake

(a)  

making dilutions using molarity equation

(a)  

making dilute solutions-

you can only

(a)  

mass percent

(a)  

mass percent equation

(a)  

volume percent

(a)  

volume percent equation

(a)  

a solution

(a)  

solvent

(a)  

solute

(a)  

Nature of the structure- some compounds are more soluble than others based on their (a)  

If in ionic compounds the attraction for the ions is greater than that of the water, then the substance (a)   dissolve well in water

in general, (a)   temperatures dissolve substances better

agitation- the more a solution is stirred, mixed, etc. , the (a)   the substance dissolves

particle size-

the smaller a particle, the (a)   the substance dissolves

the nature of a solute- some gases dissolve better in liquids than others based on their molecular

(a)  

in general, (a)   temperatures dissolve gases better

agitation- the more a solution is stirred, mixed, etc. , the (a)   a gas dissolves

pressure- the higher the pressure, the (a)   a gas dissolves

unsaturated solution

(a)  

saturated solution

(a)  

supersaturated solution

(a)  

if the salt (a)   crystallize out then the solution is supersaturated because it contains more than the maximum at the new cooler temperature.

a supersaturated solution can be made to crystallize by adding a (a)   crystal

what is a seed crystal

(a)  

dilute solution

(a)  

concentration solution

(a)  

a (a)   solution is concentrated

an (a)   saturated solution an be concentrated or dilute

miscible

(a)  

immiscible

(a)  

Colligative properties

(a)  

Colligative Properties-

example-

Vapor Pressure (a)  

Colligative Properties-

example-

Boiling Point (a)  

Colligative Properties-

example-

Freezing Point (a)  

The phenomenon that the boiling point of a liquid will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent.

(a)  

The number of solvent molecules escaping into vapour phase gets reduced and as a result the pressure exerted by the vapour phase is also reduced.

(a)  

The decrease of the freezing point of a solvent due to the addition of a solute into the solvent.

(a)  

Vapor Pressure

(a)  

a state in which opposing forces or influences are balanced.

(a)  

Pressure is the number of (a)   that are above (in gaseous state) a solution

as the number of solute particles increase, the vapor pressure (a)  

as the number of solute particles increase, the vapor pressure decreases. This is due to the water particles surrounding the solute and thus are less likely to gain enough (a)   to escape the surface

the adding of a solute to a pure solvent (a)   the boiling point of the solvent

the adding of a solute to a pure solvent (a)   the freezing point of the solvent

particles in a pure solvent (a)   the formation of a freezing pattern

electrolyte

(a)  

non electrolyte

(a)  

conductivity is (a)   a colligative property

conductivity is based on the number of (a)   in solution, not just the number of dissolved particles

a substance that dissolves and does not produce ions will (a)   conduct electricity

Beers law

(a)  

Chromatography

(a)  

Titration

(a)