Week Twelve

Question 1

liquid solution - parts

Answer 1

non voliatile solute and a liquid solvent

Question 2

non volatile solute

Answer 2

solutes that have no significant vapor pressure

Question 3

magnitude of boiling point elevation of solution

Answer 3

depends on the amount of particles dissolved

Question 4

colligative properties

Answer 4

properties of solutions prepared from non volatile solutes

depend on number of particles rather than chemical identities

Question 5

non volatile solutes - evaporation

Answer 5

dont evaporate from solution

Question 6

Molarity

Answer 6

c= n/V

Question 7

molarity vs temp

Answer 7

molarity decreases as temp increases

Question 8

molality

Answer 8

molar amount of solute per mass

Question 9

molality equation

Answer 9

b = n/m

Question 10

mole fraction

Answer 10

number of moles in a compound divided by total number of moles of material

Question 11

mole fraction equation

Answer 11

n(A)/ n(A) + n(B) + n(C)

Question 12

Raoult’s Law

Answer 12

boiling point of a solution containing a nonvolatile solute is higher than that of a pure solvent
solution has lower vapor pressure than a pure solvent

Question 13

Raoult’s Law equation

Answer 13

relationship between vapor pressure, mole fraction of solvent and vapor pressure of solvent
p(solution) = x(solvent) x p*(solvent)

Question 14

x solvent

Answer 14

mole fraction of solvent

Question 15

p* solvent

Answer 15

vapour pressure of pure solvent

Question 16

Ideal solution

Answer 16

obeys raoults law
only the case
- a high dilution
- when enthalpy of mixing is small

Question 17

solutions with more than one volatile component

Answer 17

all partial pressures combine to total vapor pressure of solution

Question 18

boiling point elevation

Answer 18

delta T= i x Kb x b 
where delta T = T(solution) - T(solvent) 
kb = ebullioscopic constant 
b = molality of solution 
i = van't hoff factor

Question 19

Freezing point depression

Answer 19

delta T= i x Kf x b 
where delta T = T(solvent) - T(solution) 
kb = cryoscopic constant 
b = molality of solution 
i = van't hoff factor

Question 20

dialysis

Answer 20

dialysing membrane allows both water and small solute particles through

Question 21

osmosis

Answer 21

net shift of only solvent through an osmotic membrane

Question 22

osmotic pressure

Answer 22

pressure needed to prevent any osmotic flow when one liquid is a pure solvent

Question 23

Osmotic pressure equation

Answer 23

O = i x c x R x T
where i = van’t hoff factor
R = gas constant
c = molar concentration

Question 24

osmometer

Answer 24

measures osmotic pressure

Question 25

isotonic

Answer 25

same osmotic pressure as red blood cells

Question 26

hyper tonic

Answer 26

solution with higher salt concentration

Question 27

hypotonic

Answer 27

solution with lower osmotic pressure

Question 28

van’t hoffs factor

Answer 28

shows the degree of dissociation of the solute

Question 29

solute dissociation - vant hoffs factor equation

Answer 29

i = theeoret x dissociation factor x (change in temp obsered)/(change in temp theorectical)