Summary of Chapter 14 about Solutions, Includes brief notes on Vapor Pressure with Volatile and Nonvolatiles, Osmotic Pressure, Boiling Point Elevation and Freezing Point Depression, Henry's Law, Gas Constants, Nonpolar and Polar Solvents, What Affects Solubility. Orange Coast College
Solution concentration Factors affecting
units solubility
- mass % : mass solute +100 - “like dissolves like”
mass solution - polar solvents tend to
-ppt: above ✗ 1000 dissolve polar molecules &
Equation
ionic cmpds
-ppm: ✗ 1,000,000 - b/c pos/neg end of polar
solvent (like h2o)
-Ppb: ✗ 11000,000 ,
000
attracted to pos/neg end
of polar molecule
moles solute
-mole fraction: ✗ =
moles solution
-nonpolar solvents dissolve
nonpolar molecules
MO I solute
- Molarity: M = -for solids, solubility ↑ as
L solution
temp *
- molality: m= Moles solute - for gas, solubility as temp i •
solvent
kg - for liquid and solid:
Vapor pressure of a pressure has little affect
solution w/ nonvolatile on solubility in h2o
- nonvolatile = no vp - for gas: higher partial
- adding nonvolatile solute pressure, the more soluble
to solvent lowers vp b/c it -define by Henry’s law:
takes up space in the solution C. K P gas Partial
g.
= .
& interfers w/ escape of
solvent contentration P
constant
'
- raoult’s law shows
relationship b/w solvent vp & Vapor pressure of
concentration solution w/ volatile
- in ideal solution where
LP ✗ P
= °
•
, ,
solute and solvent follow
VP
pure mole VP Raoult’s, vp=sum of vp from
solvent fraction each component
over
solvent
solvent - do raoult’s law twice:
solution ✗A
{
PA = •
PAO P total =
PBO PA + PB
PB= ✗ B •
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