grams) dissolved in total mass of solution (in grams) is called mass fraction of the solute.
Mass fraction = w w W
(b) Mass percentage:- The amount of solute in grams dissolved in 100 gms of the solution.
Mass percentage = w 100 w W
Where w = Mass of solute
W = Mass of solent
2. Volume Percentage:-
(a) Volume fraction:- The volume of a liquid (solXII
- Chemistry Solutions
17
N =
Number of gramequivalentsof solute
Volumeof solution in litre
=
Number of grams equivalent of solute 1000
Volume of solution in ml
Since
Number of grams equivalents =
Mass
Equivalent mass
N =
Mass of solute in grams 1000
Equivalent mass Vol.of solution (in ml)
Normality of a solution = Molarity ×
Molecularweight
Equivalentweight of solute
CALCULATION …show more content…
Relationship between Molarity and Mass
Percentage:-
Molarity = p d 10
Molar mass
Normality = p d 10
Equivalent mass
Where p = mass percentage d = density of the solution
3. Relationship between Molarity and Molality:- m = B
1000 M
1000 d m GMM
Where GMMB = Gram Molecular mass of solute d = Density of the solution
4. Dilution Formula:-
1 1 2 2 M V M V
1 1 2 2 N V N V
5. Molarity of a mixture of Solutions:-
1 1 2 2
1 2
M MV M V
V V
6. Relationship between Molality and
Molefraction of solute:-
A
B
A B
X m GMM m GMM GMM 1000d
B
A A B B m 1000 d X
X GMM X GMM
Where,
XB = Molefraction of Solute
XA = Molefraction of Solvent m = Molality of Solution d = Density of Solution
GMMA = Gram Molecular Mass of Solvent
GMMB = Gram Molecular Mass of Solute
HENRY’S LAW
It state that the solubility of a gas at a given temperature is directly proportional to the pressure at which it is dissolved.
B X p or B p X
H B p K .X
Where p = Partial pressure of the gas
B X = Mole fraction of the gas
H K = Henry law constant
(1) Significance of Henry law constant:-
(a) The unit of Henry law constant are some as those of pressure i.e. torr or k bar.
(b) Different gases have different values of Henry law
Mass fraction = w w W
(b) Mass percentage:- The amount of solute in grams dissolved in 100 gms of the solution.
Mass percentage = w 100 w W
Where w = Mass of solute
W = Mass of solent
2. Volume Percentage:-
(a) Volume fraction:- The volume of a liquid (solXII
- Chemistry Solutions
17
N =
Number of gramequivalentsof solute
Volumeof solution in litre
=
Number of grams equivalent of solute 1000
Volume of solution in ml
Since
Number of grams equivalents =
Mass
Equivalent mass
N =
Mass of solute in grams 1000
Equivalent mass Vol.of solution (in ml)
Normality of a solution = Molarity ×
Molecularweight
Equivalentweight of solute
CALCULATION …show more content…
Relationship between Molarity and Mass
Percentage:-
Molarity = p d 10
Molar mass
Normality = p d 10
Equivalent mass
Where p = mass percentage d = density of the solution
3. Relationship between Molarity and Molality:- m = B
1000 M
1000 d m GMM
Where GMMB = Gram Molecular mass of solute d = Density of the solution
4. Dilution Formula:-
1 1 2 2 M V M V
1 1 2 2 N V N V
5. Molarity of a mixture of Solutions:-
1 1 2 2
1 2
M MV M V
V V
6. Relationship between Molality and
Molefraction of solute:-
A
B
A B
X m GMM m GMM GMM 1000d
B
A A B B m 1000 d X
X GMM X GMM
Where,
XB = Molefraction of Solute
XA = Molefraction of Solvent m = Molality of Solution d = Density of Solution
GMMA = Gram Molecular Mass of Solvent
GMMB = Gram Molecular Mass of Solute
HENRY’S LAW
It state that the solubility of a gas at a given temperature is directly proportional to the pressure at which it is dissolved.
B X p or B p X
H B p K .X
Where p = Partial pressure of the gas
B X = Mole fraction of the gas
H K = Henry law constant
(1) Significance of Henry law constant:-
(a) The unit of Henry law constant are some as those of pressure i.e. torr or k bar.
(b) Different gases have different values of Henry law