solutions Flashcards
mass percentage of solute
mass of solute/mass of solution X 100
mass percentage of solute ( density)
mass of solute X 100/ volume of solution X density
mass fraction
mass of solute/mass of solution
mass percentage of solute ( mass fraction)
mass fraction X 100
percentage by vol
volume of solute X 100/ volume of sol
percentage mass by vol
mass of solute X 100/ volume of sol
strength of solution or conc of solution
mass of solute (in gram) /volume of solution in litre
parts per million
mass of solute X 10(power 6) / mass of soultion
mole fraction or fa
number of moles of a /total no of moles
no of moles of soluteor solvent
weight of solute or solvent/ molecular mass of solute / solvent
Fa + Fb + Fc=
1
molality (m)
no of moles of solute/ no of kg solvent
realation between mole fraction and molality
Xb X1000/ (1-Xb) molucle mass of a
molality (solubilty)
solubility X 10 / molecular mass of solute
solubilty
no of moles of solute/ no of moles of solvent
molarity ( M)
no of moles of solute/ no of litres of soultion
molarity ( density given)
(x) X d X 10 / molecular mass of solute
relation between molarity(M) and molality(m)
1/m = P/M - molecular mass of solute/ 1000
realtion between molarity and mole fraction
no of moles of solute X 1000 X density / mass of solution ( na ma + nb mb)
normality
Number of gram equivalents of solute/Number of litres of the solution
normality X eq mass
strenght of solution
relation of molarity and normality
(n=Molecular mass/ Equivalent mass)
n X molarity
absorption coeff
v/ V X P (v=volume of gas dissolved)(V= volume of solution) ( pressure in atm)
henrys law( solubility)
m= kp or s= kp
henrys law
partial pressure of the gas = mole fraction X henrys const
which gas dont follow raoults law
ideal gas
raoults law
P= X partial pressure(a) + X partial pressure (b)
The process of separation liquid from ‘a”nother liquid
(binary mixture) having diffrent
boiling points
If a
substance dissolves with absorption of heat, the, solubility
_________ with rise of temperature
increase
if a
substance dissolves with evolution of heat, the solubility
__________ with rise of temperature.
decrease
Two solutions having same vapour pressure at same temperature are known as
isotropic solutions
relative lowering of vapour pressure
(Po is the vapour pressure of pure solvent)
(d Ps is the
vapour pressure’ of the solution)
Po- Ps/ Po
relation between lowering vp and raoults law
Po- Ps/ Po = n/n+N (n= moles of solute and N moles of solvent)
Variation of vapour pressure with temperature
log10 ( P2/ P1)= delta H vap X (1/T1 - 1/T2)/ 2.303 R
the temperature at which its
vapour pressure is equal to the atmospheric pressure is called
boiling point
the boiling point of the solvent is elevated by the addition of
_______ solute
non-volatile solute
Elevation of boiling point,
(delta T)=
Boiling point of the solution - Boiling point of pure
solvent
Elevation of boiling point,
(delta T)=
K X no of moles of solute/ mass of solvent
the
elevation in boiling point produed when 1 mole of the solute
is dissolved in 100 g of the solvent is called
molecular elevation constant (K dash)
elevation in boiling point produced when 1 mole of the solute
is dissolved in 1000 g of the solvent is called
molal elevation constant ( Kb)
relation between molal elevation const and molality
deltaT == Molality x K b
Raou!t’s.
laws of elevation of boiling point(definition )?
The elevation in boiling point of a solution of non-electrolYte is propo!tional to its molality and equimolal
solutions of all the substances in the same solvent will show
equal elevation in boiling points
Raou!t’s.
laws of elevation of boiling point (formula)
K b = R Tb^2/ 1000 Ly (Tb is the boiling point of the solvent on kelvin scale) and (Tb is the boiling point of the solvent on kelvin scale)
the temperature at which the vapour pressure of its liquid is equal to the vapour pressure of the corresponding solid is called
freezing point
the depression of freezing point produced
when 1 mole of solute is dissolved in 1000 g of the solvent is called
K f molal depression constant
what solution is added to make a solution NOT FREEZE
ethylene glycol
what can be lowered to. the desired’ extent by varying the concentration of ethylene glycoL
freezing point
Glycerol can also
be used as anti-freeze.
its just facts (YOUR DOING GREAT :))
the solvent molecules
from a solution of lower concentration move towards a solution
of higher concentration IS called
osmosis
list two diff between Osmosis and Diffusion
In diffusion, solute as well as solvent molecules flow in opposite directions while in osmosis the flow of solvent molecules occurs in one direction only
For osmosis, a semipermeable membrane* is required
while for diffusion it is not required.
what is substance called if the solvent molecules to pass
through it but prevents the passage of solute molecules through it
semi permeable membrane
semipermeable
membranes name two substances
calcium phosphate and copper ferrocyanide, (ITS OKAY IF U DIDNT GET IT BUT MARK IT IMP)
Osmotic pressure equals
π = hdg (h = increase in level in the tube of unit cross section, d density of solution and g = acceleration due to gravity.)
osmotic pressure when
two solutions of different concentration are separated by
semipermeable membrane then
π= hdg := CRT (conc of solution= C)
A solution of high osmotic
pressure is termed
hypertonic
A solution of low osmotic
pressure is termed
hypotonic
when hypotonic solution is
separated from hypertonic solution using semipermeable
membrane, then osmosis takes place from hypotonic to hypertonic because solvent concentration is greater in hypotonic
solution
plasmolysis
solutions having same osmotic pressures are termed
isotonic
define Boyle-van’t Hoff law
The osmotic pressure (P or pi)
of a solution is directly proportional to its concentration (C )
when the temperature is kept constant
when concentration and
temperature both are changing, the osmotic pressure will be
given by
PV=nST or πV=nST(S is called molar solution constant.) (no of moles of solute)
when is no flow
of solvent molecules is observed on either side during osmosis
When two isotonic
solutions are separated by a semipermeable membrane
DETERMINATION OF MOLECULAR
MASSES by osmotic pressure
mb = Wb X S X T / PV
Let two solutions of same substance having
different osmotic pressures 1t1 and 1t2 are mixed. Osmotic
pressure of the resultant solution can be calculated as?
π1V1+ π2V2 = πr(VI + V2) [ πr= resultant osmoics pressure]
Let n l and n2 are the number of moles of two
different solutes present in VI and V2 volumes respectively.
Osmotic pressure of the mixture can be calculated as
π = (n1i1 +n2 i2 ) RT/( V1+V2) [ i1 and i
2 are van’t Hoff factor for the two solutes.]
,
If external pressure greater than osmotic pressure is applied, the flow of solvent molecules· can be made’ to proceed
from solution towards pure solvent is called
reverse osmosis
Abnormal colligative property/ normal colligative property is called
van hoff factor i
van hoff factor=
Actual no. of particles in solution/
No. of particles taken
Total number of particles in solution=
1+ (n -l)alpha (alpha= degree of association )
