The k= 4.95 × 10-5S cm-1 for a 0.00099 M solution. The reciprocal of the degree of dissociation of acetic acid, if m0 for acetic acid is 400 S cm2mol-1 will be:

1. 7 2. 8
3. 9 4. 10

Subtopic:  Conductance & Conductivity |
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Pure water is saturated with pure solid AgCl, a silver electrode is placed in the solution and the potential is measured against normal calomel electrode at 25°C. This experiment is then repeated with a saturated solution of AgI. If the difference in potential in the two cases is 0.177 V. What is the ratio of solubilities of AgCl and AgI at the temperature of the experiment ?

(1) 103   

(2) 106 

(3) 104 

(4) 102

Subtopic:  Relation between Emf, G, Kc & pH |
 51%
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A hydrogen electrode X was placed in a buffer solution of sodium acetate and acetic acid in the ratio a : b and another hydrogen electrode Y was placed in a buffer solution of sodium acetate and acetic acid in the ratio b : a. If reduction potential values for two cells are found to be E1and E2 respectively with respect to standard hydrogen electrode, the pKa value of the acid can be given as

(1) E1-E20.118                                           

(2) E1+E20.118

(3) E1E2×0.118                                      

(4) E2-E10.118

Subtopic:  Relation between Emf, G, Kc & pH |
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Calculate the useful work of the reaction \(Ag(s) + {1 \over 2} Cl_2(g) \rightarrow AgCl(s)\) 

Given,
E°Cl2/Cl-=+1.36 V, E°AgCl/Ag,Cl-=0.22 V
If PCl2=1 atm and T=298 K

(1) 110 kJ/mol

(2) 220 kJ/mol

(3) 55 kJ/mol

(4) 1000 kJ/mol

Subtopic:  Relation between Emf, G, Kc & pH |
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A resistance of 50Ω is registered when two electrodes are suspended into a beaker containing a dilute solution of a strong electrolyte such that exactly half of the them are submerged into solution. If the solution is diluted by adding pure water (negligible conductivity) so as to just completely submerge the electrodes, the new resistance offered by the solution would be

                                          

(1) 50Ω                                       

(2) 100 Ω

(3) 25Ω                                       

(4) 200Ω




Subtopic:  Conductance & Conductivity |
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Acetic acid has Ka = 1.8 × 10-5 while formic acid has Ka = 2.1 × 10-4. What would be the magnitude of the emf of the cell 

                  PtH20.1 M acetic acid + 0.1 M sodium acetate 0.1 M formic acid  0.1 M sodium formatePtH2 at 25°C ?

(1) 0.0315 volt                            

(2) 0.0629 volt

(3) 0.0455 volt                            

(4) 0.0545 volt

Subtopic:  Nernst Equation |
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Following cell has EMF 0.7995 V 

Pt | H2 (1 atm) | HNO3 (1M) || AgNO3 (1M) | Ag

If we add enough KCl to the Ag cell so that the final Cl-is 1M. Now the measured emf of the cell is 0.222 V. The KSP of AgCl would be :

(1) 1 × 109.8 

(2) 1 × 1019.6

(3) 2 × 1010  

(4) 2.64 × 1014

Subtopic:  Nernst Equation |
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A flashlight cell has the cathodic reaction 2MnO2 (s) + Zn+2+ 2'e- Zn Mn2O4 (S)

If the flashlight cell is to give out 4.825 mA, how long could it run if initially 8.7 g of the

limiting reagent MnO2 is present? [Mn = 55, O = 16]

(1) 2 × 106sec                                         

(2) 4 × 106sec

(3) 6× 106sec                                          

(4) 8 × 106sec

Subtopic:  Faraday’s Law of Electrolysis |
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An excess of granular zinc was added to 500 mL of 1M nickel nitrate till equilibrium was established. Find out the concentration of nickel at the equilibrium, if the standard electrode potential of Zn2+ / Zn and Ni2+/Ni  are – 0.75 and – 0.24 V, respectively.
(1) 5.56 x 10-18 M
(2) 0.56 x 10-18 M
(3) 2.16 x 10-18 M
(4) 4.12 x 10-18 M

Subtopic:  Nernst Equation |
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Calculate the cell EMF in mV for Pt | H2 (1atm) | HCl (0.01 M) | AgCl(s) | Ag(s) at 298 K 

If Gr° values are at 25°C -109.56kJmol for AgCl(s) & 130.79kJmol for (H++ Cl-) (aq)

(1) 456 mV                         

(2) 654 mV

(3) 546 mV                         

(4) None of these

Subtopic:  Faraday’s Law of Electrolysis |
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