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DEGREE OF DISSOCIATION OF SOLUTES

The degree of dissociation can be defined as the fraction of solute molecules that dissociates. - It can also be defined as the generation of current carrying free ions which dissociate from the fraction of the solute at a given temperature.

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DEGREE OF DISSOCIATION OF SOLUTES

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  2. DEGREE OF DISSOCIATION OF SOLUTES 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 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

  3. VAN'T HOFF'S FACTOR In 1886, van't Hoff introduced a factor 'i' called van'thoff'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'thoff'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'thoff'sfactoray also be written as

  4. 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

  5. Van't Hoff Factor with association Reactions 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

  6. Van't Hoff Factor For Dissociation KCL ⇌K + CL 1 mole αα 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

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