solubility

what phase is water below 0C

solid

solubility of ionic compounds

1. group 1 ions

2. contains ammonium

3. contains nitrate

4. contains acetate

solvation

as a solution forms, solvent pulls solute molecules apart and surrounds/solvates them

interactions in solutions

solvent solvent

solute solute

solvent solute

solvent solvent

solvent molecules are separated, bonds are broken

ΔH of solvent -solvent

+

solute-solute

solute molecules are broken

is solute solute endothermic or exothermic

endothermic bc energy is required to break bonds

solvent - solute

solvent molecuels mix withs olute molecules due to IMF

is solvent-solute exothermic or endothermic

exothermic because bonds are formed (IMF)

what type of bonds are IMF

physical bonds

what is the extent of solubilty dependt on

naturaltendency for mixing (mixing increases entropy)

relative forces of attraction btween solute and olsvent

ΔHsoln

ΔH1+ΔH2+ΔH3

usually endothermic, ΔG=ΔH-tΔS=entropically driven

why are gases miscible

weak imf

entropy dominated process

solubility

max amt of a solute that will dissolve in a specific amnt of solvent at a given temp

saturated solns

contain max amt of solute at a given temp

cannotd issolve additional solute

unsaturated solns

contain less solute than it can dissolve at a given temp

additional solute will dissolves

supersaturated soln

solvent holds more solute than is normally possible at that temp

unstable

what would happen if additional solute was added to asupersaturated soln

rapid crystaillization

exampleo f supersaturated soln

handwarmers

factors that affect solubility

solubility of solids increases w/increasing temp

vs gas → deccrease with increasing temp

solubility of l and s does not change with pressure

vs gas → solubility of gas in a liquid increases with increasing partial pressure

why does solubility of gas decrease with increasing temp

decreased temp → decreased KE

gas particles are less able to leave liquid solution

keeps gas dissolved in