This document contains contact information and personal details for Abubakar Bhutta. It also outlines his skills including various software programs and languages spoken. The document further discusses van't Hoff factor which is the ratio of normal and observed molecular masses of solutes in solution. It can be used to express the extent of association or dissociation of solutes, with values less than 1 indicating association and greater than 1 indicating dissociation. Equations for colligative properties are modified using the van't Hoff factor.

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ABU BAKAR
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3. It is defined as the fraction of total molecules
which dissociate into simpler molecules or
ions.
α=i-1/m-1
m=number of particles in solution
DEGREE OF ASSOCIATION OF SOLUTES
It is defined as the fraction of the total
number of molecules which associate or
combine together resulting in the formation
of a bigger molecules.
α=i-1/(1/m)-1

4. In 1886, van't Hoff introduced a factor 'i' called van't hoff's
factor , to express the extent of association or dissociation
of solutes in solution. It is the ratio of the normal and
observed molecular masses of solutes.
i= Normal Molecular Mass/Observed Molecular Mass
In case of association observed molecules mass being
more then normal, the factor i has a value less then 1 . But
in case of dissociation, the van't hoff's factor is more then 1
because the observed molecular mass is less then normal
molecular mass. In case there is no dissociation the value
of 'i' because equal to one .
Since ,collegative properties are inversely proportional to
molecular mass, the van't hoff's factoray also be written as

5. i= observed value of collegative property/calculated
value of collegative
property assuming no association or dissociation
i=No of particles after association or
dissociation/no of particles before association or
dissociation
Factors modified the equations for the collegative
properties as follows ,
 Relative Lowering Of V.P = P'a - Pa/P'a=iXb
 Elevation of B.P. ΔTb = iKbm
 Depression of F.P . ΔTf =iKfm
 Osmotic Pressure

6. nA⇌ (A)n
Let a be the degree of assodation, then,
The number of unassociated moles=1-α
The number of associated moles= α/n
Total number of effective moles= 1-α+α/n
i=1-α+(α/n)/1
i=1-α+(α/n). Obviously : i<1

7. KCL ⇌K + CL
1 mole α α
1-α
α = degree of dissociation
Total Moles In Reaction = 1- α+ α+ α
= 1+ α
i = 1+ α
Effective Moles after dissociation = 1+(2-1)α
= 1+(n-1)α
Where n is no of ions after dissociation of 1
molecule
i>1