Q. No.The variation of molar conductivity with the concentration of an electrolyte (X) in an aqueous solution is shown in the given figure.
The electrolyte X is:
1.
CH3COOH
2.
KNO3
3.
HCl
4.
NaCl
The electrolyte X is:
The molar conductivity of 0.007 M acetic acid is 20 S cm2 mol–1. The dissociation constant of acetic acid is :
(\(\mathrm{\Lambda_{H^{+}}^{o} \ = \ 350 \ S \ cm^{2} \ mol^{-1} }\))
(\(\mathrm{\mathrm{\Lambda_{CH_{3}COO^{-}}^{o} \ = \ 50 \ S \ cm^{2} \ mol^{-1} }}\))
1. mol L–1
2. mol L–1
3. mol L–1
4. mol L–1
Consider the following graph.
The strong electrolyte in the above graph is represented by:
1. X
2. Y
3. Both X and Y
4. Data given is not sufficient to predict.
The concentration of solution will change when it is placed in a container which is made of:
| 1. | Al | 2. | Cu |
| 3. | Ag | 4. | None |
The potential of hydrogen electrode in contact with a solution with pH =10, is:
| 1. | −0.0591 V | 2. | −5.91 V |
| 3. | 0.0591 V | 4. | −0.591 V |
Molar conductivities at infinite dilution of
NaCl, HCl, and are 126.4, 425.9, and 91.0 S cm2 mol–1 respectively.
for will be:
| 1. | \(180.5~S~cm^2~mol^{-1}\) | 2. | \(290.8~S~cm^2~mol^{-1}\) |
| 3. | \(390.5~S~cm^2~mol^{-1}\) | 4. | \(425.5~S~cm^2~mol^{-1}\) |
In a typical fuel cell, the reactants (R) and products (P) are:
| 1. | R = H2(g), O2(g); P = H2O2(l) |
| 2. | R = H2(g), O2(g); P = H2O(l) |
| 3. | R = H2(g), O2(g), C l2(g); P = HClO4(aq) |
| 4. | R = H2(g), N2(g); P = NH3(aq) |
1. \(K_{a}=\frac{C \Lambda_{m}^{\infty}}{\left(\Lambda_{m}-\Lambda^{\infty}\right)}\)
2. \(K_{a}=\frac{C \Lambda_{m}^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)} \)
3. \(K_{a}=\frac{C\left(\Lambda_{m}^{\infty}\right)^{2}}{\Lambda_{m}^{\infty}\left(\Lambda_{m}^{\infty}-\Lambda_{m}\right)}\)
4. None of the above
| 1. | weight of cathode increases |
| 2. | pH of the solution remains unchanged |
| 3. | product at the anode is \(O_2\) gas |
| 4. | weight of the anode is unchanged |
The half-cell reaction at the anode during the electrolysis of aqueous sodium chloride solution is represented by :
1. Na+(aq) + e- ⟶ Na(s) ; \(E_{cell}^{o} \ = \ -2.71 \ V \)
2. 2H2O(l) ⟶ O2(g) + 4H+(aq) + 4e- ; \(E_{cell}^{o} \) = 1.23 V
3. H+(aq) + e- ⟶ \(\frac{1}{2}\)H2(g) ; \(E_{cell}^{o} \) = 0.00 V
4. Cl-(aq) ⟶ \(\frac{1}{2}\)Cl2(g) + e- ; \(E_{cell}^{o}\)
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