Answer
Verified
375.9k+ views
Hint : First calculate the value of $ E{^\circ _{cell}} $ . The value of $ E{^\circ _{cell}} $ will be used in the Nernst equation to get the value of $ Q $ which is a ratio of molarity of products to molarity of reactants. The value of $ Q $ will be used to calculate the molarity of $ SO_4^{2 - } $ . Now we can calculate the dissociation constant $ K $ .
Complete Step By Step Answer:
First we have to calculate the value of $ E{^\circ _{cell}} $ ,
We know that,
$ E{^\circ _{cell}} = E{^\circ _R} - E{^\circ _L} $
It is given that,
$ E{^\circ _R} = - 0.126 $ and $ E{^\circ _L} = 0.356 $
Therefore,
$ E{^\circ _{cell}} = - 0.126 + 0.356 $
$ E{^\circ _{cell}} = 0.23V $
We can now use Nernst's equation to calculate the value of $ Q $ . Nernst equation is given as:
$ {E_{cell}} = E{^\circ _{cell}} - \dfrac{{0.0592}}{n}\log Q $
Where, $ {E_{cell}} \to $ max potential which can be generated when no current is flowing.
$ E{^\circ _{cell}} \to $ cell potential
$ n \to $ number of electrons gained or lost during reaction.
If we check the reaction, we can see that the number of electrons lost is $ 2 $ .
$ Pb(s) + SO_4^{2 - } \to PbS{O_4} + 2{e^ - } $
On putting the values in Nernst equation,
$ 0.061 = 0.23 - \dfrac{{0.0592}}{2}\log Q $
On further solving,
$ \log Q = 5.709 $
$ Q = 5.122 \times {10^5} $
Since,
$ Q = \dfrac{{[products]}}{{[reac\tan ts]}} $
$ Q = \dfrac{{[PbS{O_4}]}}{{[P{b^{2 + }}][SO_4^{2 - }]}} $
Hence,
$ 5.122 \times {10^5} = \dfrac{1}{{2.5 \times {{10}^{ - 5}} \times [SO_4^{2 - }]}} $
$ [SO_4^{2 - }] = \dfrac{1}{{5.122 \times {{10}^5} \times 2.5 \times {{10}^{ - 5}}}} $
$ [SO_4^{2 - }] = 0.078M $
Hence, $ 0.078M $ of $ SO_4^{2 - } $ will make $ {E_{cell}} = 0 $ , thus, we reach equilibrium and now we can calculate the value of dissociation constant.
The dissociation constant $ K $ for $ HSO_4^ - $ can be calculated as follows,
$ K = \dfrac{{[{H^ + }][SO_4^{2 - }]}}{{[HSO_4^ - ]}} $
$ K = \dfrac{{0.078 \times 0.078}}{{0.6}} $
Hence,
$ K = 0.0106 $
Since we are asked to multiply the value of $ K $ by $ 100 $ , thus, on multiplying,
$ K \times 100 = 1.06 $
On writing the value of $ K $ to its nearest integer,
$ \to K = 1.06 \approx 1 $
Hence the value of $ K $ is $ 1 $ .
Note :
Neither the value of $ Q $ nor the dissociation constant $ K $ has any unit as both of them are simply a ratio of molarity of products to their reactants. $ E{^\circ _R} $ and $ E{^\circ _L} $ can be understood as potential at anode and potential at cathode respectively. The dissociation constant $ K $ can also be written as $ {K_d} $ .
The dissociation constant is called ionization constant when it is applied for salts. The inverse of dissociation constant is called association constant.
Complete Step By Step Answer:
First we have to calculate the value of $ E{^\circ _{cell}} $ ,
We know that,
$ E{^\circ _{cell}} = E{^\circ _R} - E{^\circ _L} $
It is given that,
$ E{^\circ _R} = - 0.126 $ and $ E{^\circ _L} = 0.356 $
Therefore,
$ E{^\circ _{cell}} = - 0.126 + 0.356 $
$ E{^\circ _{cell}} = 0.23V $
We can now use Nernst's equation to calculate the value of $ Q $ . Nernst equation is given as:
$ {E_{cell}} = E{^\circ _{cell}} - \dfrac{{0.0592}}{n}\log Q $
Where, $ {E_{cell}} \to $ max potential which can be generated when no current is flowing.
$ E{^\circ _{cell}} \to $ cell potential
$ n \to $ number of electrons gained or lost during reaction.
If we check the reaction, we can see that the number of electrons lost is $ 2 $ .
$ Pb(s) + SO_4^{2 - } \to PbS{O_4} + 2{e^ - } $
On putting the values in Nernst equation,
$ 0.061 = 0.23 - \dfrac{{0.0592}}{2}\log Q $
On further solving,
$ \log Q = 5.709 $
$ Q = 5.122 \times {10^5} $
Since,
$ Q = \dfrac{{[products]}}{{[reac\tan ts]}} $
$ Q = \dfrac{{[PbS{O_4}]}}{{[P{b^{2 + }}][SO_4^{2 - }]}} $
Hence,
$ 5.122 \times {10^5} = \dfrac{1}{{2.5 \times {{10}^{ - 5}} \times [SO_4^{2 - }]}} $
$ [SO_4^{2 - }] = \dfrac{1}{{5.122 \times {{10}^5} \times 2.5 \times {{10}^{ - 5}}}} $
$ [SO_4^{2 - }] = 0.078M $
Hence, $ 0.078M $ of $ SO_4^{2 - } $ will make $ {E_{cell}} = 0 $ , thus, we reach equilibrium and now we can calculate the value of dissociation constant.
The dissociation constant $ K $ for $ HSO_4^ - $ can be calculated as follows,
$ K = \dfrac{{[{H^ + }][SO_4^{2 - }]}}{{[HSO_4^ - ]}} $
$ K = \dfrac{{0.078 \times 0.078}}{{0.6}} $
Hence,
$ K = 0.0106 $
Since we are asked to multiply the value of $ K $ by $ 100 $ , thus, on multiplying,
$ K \times 100 = 1.06 $
On writing the value of $ K $ to its nearest integer,
$ \to K = 1.06 \approx 1 $
Hence the value of $ K $ is $ 1 $ .
Note :
Neither the value of $ Q $ nor the dissociation constant $ K $ has any unit as both of them are simply a ratio of molarity of products to their reactants. $ E{^\circ _R} $ and $ E{^\circ _L} $ can be understood as potential at anode and potential at cathode respectively. The dissociation constant $ K $ can also be written as $ {K_d} $ .
The dissociation constant is called ionization constant when it is applied for salts. The inverse of dissociation constant is called association constant.
Recently Updated Pages
How many sigma and pi bonds are present in HCequiv class 11 chemistry CBSE
Mark and label the given geoinformation on the outline class 11 social science CBSE
When people say No pun intended what does that mea class 8 english CBSE
Name the states which share their boundary with Indias class 9 social science CBSE
Give an account of the Northern Plains of India class 9 social science CBSE
Change the following sentences into negative and interrogative class 10 english CBSE
Trending doubts
Fill the blanks with the suitable prepositions 1 The class 9 english CBSE
The Equation xxx + 2 is Satisfied when x is Equal to Class 10 Maths
In Indian rupees 1 trillion is equal to how many c class 8 maths CBSE
Which are the Top 10 Largest Countries of the World?
How do you graph the function fx 4x class 9 maths CBSE
Give 10 examples for herbs , shrubs , climbers , creepers
Difference Between Plant Cell and Animal Cell
Difference between Prokaryotic cell and Eukaryotic class 11 biology CBSE
Why is there a time difference of about 5 hours between class 10 social science CBSE