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Test: Applications of EMF Measurements


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Test: Applications of EMF Measurements - Question 1

Only One Option Correct Type

This section contains 11 multiple choice questions. Each question has four choices (a), (b), (c) and (d), out of which ONLY ONE is correct

Q. 

For, Pt(H2)/H2O, electrode potential at 298 K and 1 bar is

Detailed Solution for Test: Applications of EMF Measurements - Question 1

It is an anode and thus oxidation takes place:

Test: Applications of EMF Measurements - Question 2

For the cell reaction at 298K, Cu2+(aq) + 2e- → Cu(s)

Variation of log[Cu2+ ] with is a straight line of intercept 0.34 V on axis .Then electrode potential of the half-cell. Cu/Cu2+ (0.1 M) will be   

Detailed Solution for Test: Applications of EMF Measurements - Question 2

Cu2+(aq) + 2e- → Cu



Given half-cell is oxidation half-cell (anode)

Test: Applications of EMF Measurements - Question 3

Given, Cu2+ + 2e- → Cu, E° = + 0.34V, Ksp of Cu(OH)2 = 1.0 x 10-19

What i s E°red of Cu2+/Cu couple at pH = 12? 

Detailed Solution for Test: Applications of EMF Measurements - Question 3

pH = 12
pOH = 2, [OH-] = 10-2M

Cu(OH)2,(s)  cu2+ (aq) + 2OH(aq)
∴    Ksp = [Cu2+][OH-]2
1 x 10-19 = [Cu2+][102-]2 

∴ Cu2+ + 2e→ cu

Reaction Quotient (Q) = 



 

Test: Applications of EMF Measurements - Question 4

EMF of the following cell is 0.67 V at 298K.

Thus, pH of the solution = 0.28 V

Detailed Solution for Test: Applications of EMF Measurements - Question 4

Hydrogen electrode has been coupled to calomel electrode.

Anode
H2(g) → 2H+(aq) + 2e     E0SHE = 0.00

Cathode
Hg2Cl2(s) + 2e- .→ 2 Hg(e)+2Cl- (aq)      E0cal, = 0.28 V

Hg2Cl2(s) + H2(g) → 2Hg(l) + 2H+(aq) + 2Cl- (aq)      E0cell, = 0.28 V

Reaction quotient (Q) =

 


Test: Applications of EMF Measurements - Question 5

Given,

A3+ + e  A2+  , E0. = 1.42 V

B4+ + 2e-  B2+   , E0. = 0.40 V

In the potentiometric titration of B2+ with A3+ the potential at the equivalence point is  

Detailed Solution for Test: Applications of EMF Measurements - Question 5




Test: Applications of EMF Measurements - Question 6

For the cell of 298 K,

Zn(s) + Cu2+ (aq)  Cu(s) + Zn2+ (aq) 

 
Variation of Ecell with logQ (where Q is reaction quotient ) is of the type  

                                          

 

 

 

 
At what value of ratio of molar  concentration of ions Ecell   would be 1.1591?      

Detailed Solution for Test: Applications of EMF Measurements - Question 6



This equation represents a straight line 


Test: Applications of EMF Measurements - Question 7

Given, Ag+ + e → Ag, 


Thus, E° of the following half-cell reaction at 298 K.

Detailed Solution for Test: Applications of EMF Measurements - Question 7



Test: Applications of EMF Measurements - Question 8

Ag/Ag electrode is immersed in 1.00 M KCl at 298 K. Ksp (AgCl) = 1.0 x 10-10

                 

Thus, EMF of the cell set up is   

Detailed Solution for Test: Applications of EMF Measurements - Question 8

In this case Ag+ ion collects as solid AgCI on the electrode itself. Some Ag+ exists in equilibrium with AgCI(s) in solution. 


Test: Applications of EMF Measurements - Question 9

For the following cell, Pt(H2) | HCI(aq) || AgCI | Ag

Ecell = 0.2650 V at 298 K and Ecell = 0.2595 V at 308 K

Thus, heat of reaction at 298 K is

Detailed Solution for Test: Applications of EMF Measurements - Question 9


By Gibbs Helmholtz equation


Test: Applications of EMF Measurements - Question 10

Quinhydrone electrode is an indicator electrode in contact with platinum metal and can be used in acid-base potentiometric titration

At the equivalence point, [A] = [B] and thus, EMF of the cell is dependent on pH. When NaOH is added to HCl in potentiometric titration, potentiogram is 

Detailed Solution for Test: Applications of EMF Measurements - Question 10




Initially in acid (HCI), pH < 7 at neutral point pH = 7 and after HCI is neutralised, pH increases due to further addition of NaOH. Hence, Ecell also increases.

Test: Applications of EMF Measurements - Question 11

Potential at the equivalence point in the potentiometric titration of Fe2+ with MnO4- in acidic medium is

Detailed Solution for Test: Applications of EMF Measurements - Question 11

When equivalence point is reached 


Test: Applications of EMF Measurements - Question 12

Comprehension Type

Direction : This section contains 3 paragraphs, each describing theory, experiments, data, etc. Six questions related to the paragraph have been given. Each question has only one correct answer among the four given options (a), (b), (c) and (d).

Passage I

The electrochemical cell shown below is a concentration cell :

M/Mz+ (saturated solution of a sparingly soluble salt(MX2) || M2+(0.001 mol dm-3)|M

The EMF of the cell depends on the difference in concentration of M2+ ions at the two electrodes .The EMF of the cell at 298 K is 0.059 V.

Q.

Ksp mol3 dm-9 (the solubility product) of MX2 at 298 K is

(2.303 RT/F = 0.059 V at 298 K)   

Detailed Solution for Test: Applications of EMF Measurements - Question 12




Test: Applications of EMF Measurements - Question 13

Passage I

The electrochemical cell shown below is a concentration cell :

M/Mz+ (saturated solution of a sparingly soluble salt(MX2) || M2+(0.001 mol dm-3)|M

The EMF of the cell depends on the difference in concentration of M2+ ions at the two electrodes .The EMF of the cell at 298 K is 0.059 V.

Q.

The value of ΔG (kJ mol-1) is (1F = 96500 C mol-1)  

Detailed Solution for Test: Applications of EMF Measurements - Question 13




Test: Applications of EMF Measurements - Question 14

Passage II

The standard half-cell reduction potential of  

Fe3+(aq) | Fe is -0.036V and that of OH- | Fe(OH3)(s) | Feis -0.786V.

Q.

For the determination of solubility product of Fe(OH)3 (Ksp) the appropriate cell representation and its EMF respectively are    

Detailed Solution for Test: Applications of EMF Measurements - Question 14


Above reaction is the net reaction in a cell for determination of Ksp.


Test: Applications of EMF Measurements - Question 15

Passage II

The standard half-cell reduction potential of  

Fe3+(aq) | Fe is -0.036V and that of OH- | Fe(OH3)(s) | Feis -0.786V.

Q.

The value of loge Ksp for Fe(OH)3 at 298 K is

Detailed Solution for Test: Applications of EMF Measurements - Question 15


Above reaction is the net reaction in a cell for determination of Ksp.

Thus,

Anode

Fe → Fe3+ (aq) + 3e-, E0ox = 0.036V

Half - cell is Fe|Fe3+ (aq). OH-(aq)

Cathode

Fe(OH)3(s) + 3e→ Fe+ 3OH-, E0red = -0.786 V

Half-cell set up is Fe(OH)3(s)|Fe

complete cell is Fe|Fe3+(aq), OH- (aq)||Fe(OH)3 (s)|Fe

and E0cell = E0ox + E0red = 0.036 + (-0.786) = -0.750V

By net reaction, K = Ksp = [Fe3+][OH-]3

∴ 

Test: Applications of EMF Measurements - Question 16

Passage III 

Tollen's reagent is used for the detection of aldehydes.When a solution of AgNOis added to glucose with NH4OH, then gluconic acid is formed. 

Q.

For the reaction,
   

Detailed Solution for Test: Applications of EMF Measurements - Question 16

2Ag+ + 2e- → 2Ag

C6H12O6 +H2O → C6H12O7 + 2H+ + 2e-
E0r = 0.80V  E0 = -0.05V

2Ag+ + C6H12O6 + H2O → 2Ag+ C6H12O+ 2H+ 

E0cell = 0.75 V

At equilibrium,  Ecell = 0


When NH3 is added, pH increases to 11 

Test: Applications of EMF Measurements - Question 17

Passage III 

Tollen's reagent is used for the detection of aldehydes.When a solution of AgNOis added to glucose with NH4OH, then gluconic acid is formed. 

Q. 

In the presence of NH3, pH is raised to 11.Thus,

Detailed Solution for Test: Applications of EMF Measurements - Question 17



When NH3 is added, pH increases to 11 

*Answer can only contain numeric values
Test: Applications of EMF Measurements - Question 18

One Integer Value Correct Type

This section contains 2 questions, when worked out will result in an integer value from 0 to 9 (both inclusive)

Q.

For the following half-cell,

EMF at 298 K is 0.2364 V. What is pH?


Detailed Solution for Test: Applications of EMF Measurements - Question 18


It is oxidation half-cell, and anode reaction is


*Answer can only contain numeric values
Test: Applications of EMF Measurements - Question 19

For Cu(OH)2|Cu hall-cell at pH = 12, electrode potential is 0.0455 at 298 K.

For Cu2+ (aq) + 2e- → Cu, E° = 0.34 V. Ksp value of Cu(OH)2 is x x 10-4

What is the value of x?    


Detailed Solution for Test: Applications of EMF Measurements - Question 19



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