Test: Applications of EMF Measurements - NEET MCQ

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

Thus, pH of the solution = 0.28 V

Given,

A³⁺ + e^-   A²⁺  , E^{0. = 1.42 V}

B⁴⁺ + 2e^-  B²⁺   , E^{0. = 0.40 V}

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

For the cell of 298 K,

Zn(s) + Cu²⁺ (aq)  Cu(s) + Zn²⁺ (aq) 

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

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

Given, Ag⁺ + e^-  → Ag, 

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

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

Thus, EMF of the cell set up is   

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

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

Thus, heat of reaction at 298 K is

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 

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

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/M^z+ (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.

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

(2.303 RT/F = 0.059 V at 298 K)   

Passage I

The electrochemical cell shown below is a concentration cell :

M/M^z+ (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)  

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 (K_sp) the appropriate cell representation and its EMF respectively are    

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 log_e K_sp for Fe(OH)₃ at 298 K is

Passage III 

Tollen's reagent is used for the detection of aldehydes.When a solution of AgNO₃ is added to glucose with NH₄OH, then gluconic acid is formed. 

Q.

For the reaction,
   

Passage III 

Tollen's reagent is used for the detection of aldehydes.When a solution of AgNO₃ is added to glucose with NH₄OH, then gluconic acid is formed. 

Q. 

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

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?

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. K_sp value of Cu(OH)₂ is x x 10^-4. 

What is the value of x?