States of Matter & Solutions- Ch 10 &12

Vaporization

boiling, liquid to gas

Evaporation

any temp, liquid to gas

Condensation

gas to liquid

Equilibrium

when opposite force occurs at the same time

Freezing Point

32F

Sublimation

Solid to gas

Deposition

Gas to solid

Triple point

Temp and pressure share all 3 phases will coexist

Solution

homogeneous mixture, particles dissolve completely

Solvent

the part doing the dissolving

Solute

substance being dissolved

Suspension

heterogeneous mixture with large particles that DO settle out upon standing “shake before use”

Colloid

mixture with a 1-1000mm size, doesn’t settle with a cloudy clarity that passes tyndall

Electrolyte

ionic compounds break into ions and conduct electricity when dissolved

Nonelectrolyte

compounds that don’t break into ions and don’t conduct electricity

Saturated Solution

solution holding max amount of solute that can be dissolved

Unsaturated Solution

solution holding less than max amt of solute that can be dissolved

Supersaturated Solution

solution holding more than max amt of solute that can be dissolved

Solubility

amount of solute dissolved in given amount of solvent at a specific temp

Immiscible

2 liquids that don’t mix

Miscible

2 liquids that mix

Henry’s Law

pressure on gas is related to solubility

Effervescence

gas comes out of solution

solution

mixture with particles smaller than 1mm, doesn’t settle with a clear clarity

suspension

mixture with particles larger than 1000mm that settles, very cloudy and sometimes passes tyndall

endothermic

takes in heat, feels cold to the touch and heat of solution is positive

exothermic

heat exits, hot to the touch and heat of solution is negative

critical point

end of liquid to gas line

solid solute factors

agitation, surface area, temp

gas solute factors

agitation, temp, pressure, concentration

morality

M = mol/L

Molality

m = mol/kg

heat of solution

energy is absorbed when specific amount of solute dissolves