solutions Flashcards
this is a homogeneous mixture that disperses uniformly throughout another
solution
effect that does not scatter a light beam, properly observed for suspensions
Tyndall effect
maximum amount of a substance that can be dissolved in a volume of solvent
solubility
describes 2 liquids when it is soluble in each other
miscibility
give an example of immiscible liquids
oil and water
FACTORS AFFECTING SOLUBILITY
“like dissolves like”
- the higher the difference of this factor, the lower the solubility
polarity
FACTORS AFFECTING SOLUBILITY
the factor that determines heat increases solubility
temperature
FACTORS AFFECTING SOLUBILITY
pressure has high effects on gaseous soluted
ture or false
true
DEGREE OF SOLUBILITY
when the rates of dissolution ad preceipitation are equal
equilibrium
DEGREE OF SOLUBILITY
contains maximum amount of a solute that will dissolve in a given solvent and temperature
saturated
DEGREE OF SOLUBILITY
when the solution contains less solute than its capacity to dissolve
unsaturated
DEGREE OF SOLUBILITY
contains more solute and is not stable. some solute will come out as crystals over time
supersaturated
DEGREE OF SOLUBILITY
in the phamaceutical industry, most drugs are supersaturated to allow precise doses/deliver drugs with low solubility in water
true or false
true
in the formations of solutions, what holds liquid and solid molecules together
intermolecular solutions
when solvent particles surround/ wrap around particles to create a solution
solvation
DISOLUTION
when more energy is released in making bonds than is used in breaking bonds
- releases energy, temp increases
exothermic
DISOLUTION
when more energy is being used than is being released
- absorbs energy and temperature decreases
endothermic
which law states that “regardless of the multiple stages or steps of a reaction, the total enthalpy change for the reaction is the sum of all changes”
hess’ law
formula of hess’ law
DHsoln = DH1+DH2+DH3
which law states that “the solubility of gasses is directly proportional to the partial pressure of gas above liquid”
henry’s law: gases
FORMULAS
mass percentage
mass (g) of solute / total mass (g) of solution x100
FORMULAS
parts per million
mass of solute / mass of solution x 1,000,000
FORMULAS
mole fraction
moles of component / total moles of solution
FORMULAS
moles
mass of a substance / molar mass of the substance
FORMULAS
molarity
moles of solute / liter of solution
FORMULAS
molality
moles of solute / kg of solvent
FORMULAS
dilution
C1 V1 = C2 V2
C1 V1 + C2 V2 = C3 V3
properties that depend only on the number of solute particles in the solution and not in the nature of the solute particles
- depends on the ratio of the solute and solvent amount
colligative properties
what are the 3 major colligative properties
- vapor pressure lowering
- freezing point depression
- boiling point elevation
(note* all properties are inversely proportional to solute molar mass)
provides more solutes to solution via dissociation; hence, the colligative properties are considerably changed
- depend on the amount of solute regardless of the nature of solute
electrolytes
provides low solute to the solution since there is no dissociation; hence the colligative properties are not considerably changed
nonelectrolytes
ELECTROLYTE OR NONELECTROLYTE
sodium chloride
electrolyte
- it dissociates, so 1 would yeild 1 molar Na+ ion and 1 molar Cl- ion
a unitless constant, directly associated with the degree of dissociation
Van’t Hoff Factor
TRUE OR FALSE
the vant hoff factor for non electrolytes is always 0
FALSE
- it is always 1 or greater because it does not dissociate
vant hoff is equal to the number of atoms formed in an aqueous solution
what is i of :
- NaCl
- AlCl3
- HCl
- NaCl: 2 VHF
- AlCl3: 4 VHF
- HCl: 2 VHF
when vapor is a mixture of solvent and solute
volatile solutes
when vapor is pure solvent
non volatile solute
formula for Raoult’s law for nonvolatile vapor pressure lowering
P solution =X solvent (P solvent)
formula for Raoult’s law for volatile vapor pressure lowering
P solution = X solvent P solvent + X solute P solute
when does boiling point elevation occur
when the BP of a solution becomes higher than the BP of a pure solvent
formula for Boiling Point elevation
change in temp = i Kb m
i = Vant Hoff constant
Kb = celsius per molal (ebullioscopic constant)
m = molaltity
when pure solvent particles become more ordered as the intermolecular forces that opperate between molecules become more permanent
freezing point depression
selective path if solvent molecules through a porous membrane from a dilute solution to a more concentrated one
osmosis
allows the passage of solvent molecules but blocks the passage of solute molecules
semi-permeable membrane
what is the pressure required to stop osmosis and its formula
osmotic pressure
= iMRT
i = vant hoff
M = molarity
R = gas constant
T = absolute temp
2 solutions are of equal concentration
isotonic
the more concentrated solution
- when it is on the outside of the cell, it causes it to crenate
hypertonic
when the cell is more concentrated inside the cells, causing it to swell up and pop
hypotonic
