In which of the following cell, salt bridge is not needed?

P b | P b S O_{4} (s) | | H_{2} S O_{4} | P b O_{2} | P b

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C d | C d O (s) | K O H (a q) | N i O_{2} (s) | N i

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F e (s) | F e O (s) | | K O H (a q) - N i_{2} O_{3} (s) | N i

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Z n | Z n S O_{4} | C u S O_{4} | C u

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Solution

The correct options are
A $P b | P b S O_{4} (s) | | H_{2} S O_{4} | P b O_{2} | P b$
B $C d | C d O (s) | K O H (a q) | N i O_{2} (s) | N i$
C $F e (s) | F e O (s) | | K O H (a q) - N i_{2} O_{3} (s) | N i$
The salt bridge is used to separate the electrolytic solution in the cathode compartment from the electrolyte cell in the anode compartment.
Hence, in the cell $Z n | Z n S O_{4} | C u S O_{4} | C u$ , the salt bridge is required.
However if one of the half cells do not contain an electrolyte then salt bridge is not required.
Thus, the salt bridge is not required in the options $A$ to $C$ . It is required in the option $D$ .

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Similar questions

Q. The Edison storage cell is represented as:

F e (s) | F e O (s) | K O H (a q .) | N i_{2} O_{3} (s) | N i (s)

The half-cell reactions are:

N i_{2} O_{3} (s) + H_{2} O (l) + 2 e^{-} \to 2 N i O (s) + 2 O H^{-}; E^{\circ} + 0.40

F e O (s) + H_{2} O (l) + 2 e^{-} \to F e (s) + 2 O H^{-}; E^{\circ} = - 0.87

,
(a) What is the cell reaction?
(b) What is the emf of the cell? How does it depend on concentration of

K O H

?
(c) What is the maximum amount of energy that can obtained from one mole of

N i_{2} O_{3}

The Edison storage cell is represented as :
Fe(s)/FeO(s)/KOH(aq)/Ni₂O₃ (s)/Ni(s)
The half-cell reactions are:
$N i_{2} O_{3} (s) + H_{2} O (l) + 2 e^{-} \to 2 N i O (s) + 2 O H^{-}; E^{\circ} + 0.40$
$F e O (s) + H_{2} O (l) + 2 e^{-} \to F e (s) + 2 O H^{-}; E^{\circ} = - 0.87$ ,
What is the maximum amount of electrical energy that can be obtained from one mole of Ni₂O₃ ?

Q. Construct the cells in which the following reactions are taking place. Which of the electrodes shall act as anode (negative electrode) and which one as cathode (positive electrode)?
(a)

Z n + C u S O_{4} = Z n S O_{4} + C u

(b)

C u + 2 A g N O_{3} = C u (N O_{3})_{2} + 2 A g

(c)

Z n + H_{2} S O_{4} = Z n S O_{4} + H_{2}

(d)

F e + S n C l_{2} = F e C l_{2} + S n

Q. Which of the following metals will couple to provide a higher cell potential for a galvanic cell?

Z n^{2 +} (a q) + 2 e^{-} \to Z n (s); E^{0} = - 0.76 V

C u^{2 +} (a q) + 2 e^{-} \to C u (s); E^{0} = 0.34 V

N i^{2 +} (a q) + 2 e^{-} \to N i (s); E^{0} = - 0.25 V

P b^{2 +} (a q) + 2 e^{-} \to P b (s); E^{0} = - 0.13 V

F e^{2 +} (a q) + 2 e^{-} \to F e (s); E^{0} = - 0.44 V

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