Module 3 Solution Chemistry Flashcards
have fixed composition such as elements and compounds.
Pure substances
have variable composition
mixtures
have a single phase and are the same in appearance throughout
Homogeneous mixtures
have two or more distinct phases.
heterogenous mixtures
are homogeneous mixtures that are consisted of solute and solvent.
solution
contains less amount of solvent
concentrated solution
contains more solvent.
dilute solutions
The solubility of a particular solute in a given solvent is affected by several factors which includes the following:
particle size, temp, nature of the solute & solvent, pressure
which is faster to dissolute, smaller or larger particles
Smaller particle size has larger surface area, thus, there is more points of interaction between the solute and solvent molecules. Therefore, smaller particle size favors a faster rate of dissolution.
what happens to the solubility of solid solute in liquid when a there is a higher temp
increases solubility
solubility of gas in liquid when temp increases
decreases
what rule does solubility follow:
Solubility follows the rule “like dissolves like”. Polar solutes dissolve in polar solvent while nonpolar solute dissolves in nonpolar solvent.
pressure affecting solubility only affects?
gaseous solute in liquid
increase in pressure is ______ proportional to the rate of solubility og gas
directly proprotional
% by mass =
m solute/m sol’n * 100
% m/v =
grams solute/mL sol’n *100
molarity =
n solute / L sol’n
molality =
n solute/kg solvent
mole fraction (X) =
n solute/n sol’n
Xsolute + Xsolvent =
1
ppm =
mg/L or mg/kg
ppb =
μg/L or μg/kg
ppt =
ng/L or ng/kg
Some analysis requires extremely small concentration unit such as those that are done for environmental and medical analysis. For such cases, it is more useful to use
parts per million (ppm), parts per billion (ppb) and parts per trillion (ppt)
concentration units that are of central importance to solution chemistry
molarity, molality and mole fraction
those that are dependent only on the amount of solute and not on its nature.
colligative properties
four specific colligative properties
1) freezing point depression, 2) boiling point elevation, 3) vapor pressure lowering and 4) osmotic pressure.
ΔTf =
kf m
ΔTf = freezing point depression =
Tf solvent - Tfsolution
ΔTb =
kb m
ΔTb = boiling point elevation =
ΔTb solution - ΔTbsolvent
Kf of H2O
1.86 C/m
Kb of H2O
0.512 C/m
the pressure that is needed to prevent the process of osmosis is called
osmotic pressure (π)
π =
MRT
R = gas constant =
0.0821 L-atm/mol K
temp in K
+ 273
when a solute is added the vapor pressure above the solution becomes lower compared to that of the pure solvent and this is phenomenon is called
vapor pressure lowering
formula for vapor pressure lowering according to Raoult’s Law is:
ΔP = mole fraction of solute * vapor pressure of the pure solvent
ΔP = P1o – P1
vp pure solvent - vp solvent above the sol’n