Metals have conductivity of the order of (ohm-1 m-1):-
1. 1012
2. 108
3. 102
4. 10-6
The specific conductance of a 0.1 M KCl solution at 23 °C is 0.012 Ω-1 cm-1 . The resistance of cells containing the solution at the same temperature was found to be 55 Ω. The cell constant will be:
1. | 0.142cm-1 | 2. | 0.66 cm-1 |
3. | 0.918 cm-1 | 4. | 1.12cm-1 |
The highest electrical conductivity of the following aqueous solution is of:
1. 0.1 M acetic acid
2. 0.1 M chloroacetic acid
3. 0.1 M fluoro acetic acid
4. 0.1 M difluoro acetic acid
Equivalent conductances of NaCl, HCl and C2H5COONa at infinite dilution are 126.45, 426.16 and 91 . The equivalent conductance of C2H5COOH is :
1. 201.28
2. 390.71
3. 698.28
4. 540.48
Pick out the incorrect statement
1. Equivalent conductance increases with dilution
2. Molar conductance increases with dilution
3. Specific conductance increases with dilution
4. Specific resistance increases with dilution
The molar conductivity of a solution of AgNO3 (considering the given data for this solution) at 298 K is:
(a) Concentration: 0.5 mol/dm3
(b) Electrolytic conductivity: 5.76×10–3 S cm–1
1. | 2.88 S cm2/mol | 2. | 11.52 S cm2/mol |
3. | 0.086 S cm2/mol | 4. | 28.8 S cm2/mol |
For the cell (at 298 K)
Ag(s) | AgCl(s) | Cl–(aq) || AgNO3(aq) | Ag(s)
Which of the following is correct –
(1) The cell emf will be zero when [Ag+]a = [Ag+]c ([Ag+] in anodic compartment = [Ag+] in cathodic compartment)
(2) The amount of AgCl(s) precipitate in anodic compartment will decrease with the working of the cell.
(3) The concentration of [Ag+] = constant, in anodic compartment during working of cell.
(4) Ecell = E°Ag+ | Ag –E°Cl–|AgCl|Ag
Equivalent conductivity of is related to molar conductivity by the expression:
1. =
2. =
3. =
4. =
Specific conductance has the unit:
1.
2. ohm.cm
3.
4.
What is the value of if for 0.04 of a at ?
(A) 9.3
(B) 9.2
(C) 4.7
(D) 4.8