In case of isotonic electrolytes ,
* the concentrations of both the electrolytes are equimolecular
* their osmotic pressures are equal
* both the electrolytes have same temperature
Therefore , considering the given electrolytes ,
{tex}\pi{/tex}(K2SO4) = {tex}\pi{/tex}(NaOH )
i(K2SO4) C(K2SO4) RT = i(NaOH) C (NaOH)RT
but , C(K2SO4) = C(NaOH)
{tex}\therefore{/tex} i (K2SO4) = i ( NaOH )
Now, we know that i (ie . vant Hoff' 's factor )
= No. of particles in dissociated molecule ( ie. after dissociation ) / No. of particles in undissociated molecule ( ie before dissociation )
ie. = degree of dissociation ({tex}\alpha{/tex})
So, let us calculate degree of dissociation for both the given electrolytes-
K2 SO4-----------------> 2K+ + SO42- ; NaOH -----------> Na+ + OH-
( 1 - {tex}\alpha{/tex} ).........................( 2 {tex}\alpha{/tex} )...........({tex}\alpha{/tex} ) -----------------------(1- {tex}\alpha{/tex} )..................({tex}\alpha{/tex}).............({tex}\alpha{/tex})
Therefore total number of particles ( ie ions / molecules ) after dissociation in both cases are -
( 1 - {tex}\alpha{/tex} + 2{tex}\alpha{/tex} + {tex}\alpha{/tex} ).............................................................................( 1 - {tex}\alpha{/tex} + {tex}\alpha{/tex} + {tex}\alpha{/tex} )
= (1 + 2{tex}\alpha{/tex} )................................. ...............................................................= ( 1 + {tex}\alpha{/tex} )
..........................................substituting the given value for degree of dissociation ({tex}\alpha{/tex}) in case of NaOH as = 1
.......................................................................................................................= 2
Further , i( K2 S O4 ) = [ (1 + 2{tex}\alpha{/tex} ) / 1 ] ........................& i (NaOH ) = ( 2 / 1 )
.......................................= [ ( 1 + 2{tex}\alpha{/tex} (K2 SO4 ) ] .......................................= 2....................................
Equating i(K2SO4) and i ( NaOH) , as inferred above we get -
1 + 2{tex}\alpha{/tex} (K2SO4) = 2
{tex}\therefore{/tex} 2 {tex}\alpha{/tex} (K2SO4) = 1
& {tex}\alpha{/tex} (K2SO4) = 1/ 2
...........................= 0.50
Hence , the degree of dissociation of given 17.4% K2 SO4 is 0.50 and is ,therefore ,50% dissociated when it is isotonic with given 4% NaOH solution .
Dr. Kamlapati Bhatt 6 years, 9 months ago
In case of isotonic electrolytes ,
* the concentrations of both the electrolytes are equimolecular
* their osmotic pressures are equal
* both the electrolytes have same temperature
Therefore , considering the given electrolytes ,
{tex}\pi{/tex}(K2SO4) = {tex}\pi{/tex}(NaOH )
i(K2SO4) C(K2SO4) RT = i(NaOH) C (NaOH)RT
but , C(K2SO4) = C(NaOH)
{tex}\therefore{/tex} i (K2SO4) = i ( NaOH )
Now, we know that i (ie . vant Hoff' 's factor )
= No. of particles in dissociated molecule ( ie. after dissociation ) / No. of particles in undissociated molecule ( ie before dissociation )
ie. = degree of dissociation ({tex}\alpha{/tex})
So, let us calculate degree of dissociation for both the given electrolytes-
K2 SO4-----------------> 2K+ + SO42- ; NaOH -----------> Na+ + OH-
( 1 - {tex}\alpha{/tex} ).........................( 2 {tex}\alpha{/tex} )...........({tex}\alpha{/tex} ) -----------------------(1- {tex}\alpha{/tex} )..................({tex}\alpha{/tex}).............({tex}\alpha{/tex})
Therefore total number of particles ( ie ions / molecules ) after dissociation in both cases are -
( 1 - {tex}\alpha{/tex} + 2{tex}\alpha{/tex} + {tex}\alpha{/tex} ).............................................................................( 1 - {tex}\alpha{/tex} + {tex}\alpha{/tex} + {tex}\alpha{/tex} )
= (1 + 2{tex}\alpha{/tex} )................................. ...............................................................= ( 1 + {tex}\alpha{/tex} )
..........................................substituting the given value for degree of dissociation ({tex}\alpha{/tex}) in case of NaOH as = 1
.......................................................................................................................= 2
Further , i( K2 S O4 ) = [ (1 + 2{tex}\alpha{/tex} ) / 1 ] ........................& i (NaOH ) = ( 2 / 1 )
.......................................= [ ( 1 + 2{tex}\alpha{/tex} (K2 SO4 ) ] .......................................= 2....................................
Equating i(K2SO4) and i ( NaOH) , as inferred above we get -
1 + 2{tex}\alpha{/tex} (K2SO4) = 2
{tex}\therefore{/tex} 2 {tex}\alpha{/tex} (K2SO4) = 1
& {tex}\alpha{/tex} (K2SO4) = 1/ 2
...........................= 0.50
Hence , the degree of dissociation of given 17.4% K2 SO4 is 0.50 and is ,therefore ,50% dissociated when it is isotonic with given 4% NaOH solution .
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