ch 13 - concentrations

Question 1

Mass % equation

Answer 1

Component/total mass

Question 2

london dispersal force

Answer 2

brief periods of polarity

Question 3

mole fraction equation

Answer 3

mole of component/total moles

Question 4

molarity equation

Answer 4

mole of solute/Liters of solution

Question 5

molality equation

Answer 5

mole of solute/Kg of solvent (mass dependent, not temp)

Question 6

energetics equation

Answer 6

H(sol)ex=H1(break solute interations)ex+H2(seperate solvent interactions)endo+H3(solute-solvent interactions)ex

Question 7

Entropy

Answer 7

disorder of the system

Question 8

saturated

Answer 8

solution in equilibrium with undissolved solute

Question 9

solubality

Answer 9

amt of solvent required to form a saturated sol’n (long chains decrease solubility in h20)

Question 10

likes disolve

Answer 10

likes

Question 11

effective pressure equation

Answer 11

Sg=KPg (molarityof gas=henry’s constant*pressure of gas)

Question 12

vapor pressure

Answer 12

volatile gases in a closed system will establish equilibrium with its liquid

Question 13

VP Raoults law equation

Answer 13

Pa=Xa Pa1 (solvent pressure=(mole fraction sol/sol’n)*VP of pure liquid)

Question 14

boiling point elevation

Answer 14

bp of sol’n > bp of pure liquid

Question 15

BP/FP equation

Answer 15

Tbp=KbMa (change in T=constant*Molality)

Question 16

Osmotic equation

Answer 16

Pi=n/vRT (osmotic pressure=Molatity*.0821L atm/mol * K)

Question 17

osmotic pressure

Answer 17

pressure required to prevent osmosis

Question 18

chemical equalibrium

Answer 18

rate of decomp=rate of formation

Question 19

equalibrium constant equation

Answer 19

Keq=Pc^c * Pd^d / Rxa^a * Rxb^b (pressure or concentration for product and reactant)

Question 20

Clausius-Clapperon equation (VP)

Answer 20

lnP= (-changeHvap/RT)+C (natural log)

Question 21

CC equation if you know two points

Answer 21

Ln P1/P2 = (-Hvap/R)*(1/T2 - 1/T1)