A porous plate or a salt bridge is used so that electrolytes of both electrodes do not intermix with each other.
In lead storage cell, only single electrolyte (dilute H2SO4) is used in both electrodes and no separation for electrodes is needed.
03. Na and K can displace hydrogen from acids but Pt, Pd, and Cu cannot. Explain.
Na and K have less reduction potential than hydrogen and acts as good reducing agents. They displace hydrogen from an acid.
Na + H2SO4 ------> Na2SO4 + H2
Pt, Pd, and Cu have greater reduction potential than hydrogen and are very weak reducing agents. These metals do not displace hydrogen from an acid.
Pt + H2SO4 ------> No reaction
04. The equilibrium is set up between metal atom of electrolyte and ions of metal in a cell. Explain.
When a metal electrode is dipped in the solution of the same metal ion, there two possibilities: (1) Metal can lose an electron and dissolved in the solution to form metal ions.
M (s) -------> M(aq)+ + e−
(2) Metal ion can absorb electron from the metal atom and get deposit at electrode.
M(aq)+ + e− -------> M (s)
There is an equilibrium between metal atoms and ions. This equilibrium shifts toward the right or left depending upon the second electrode which is attached to it.
05. A salt bridge maintains electrical neutrality in the cell. OR what is the function of the salt bridge?
The solution of electrolyte in a cell is electrically neutral. This neutrality is maintained by the salt bridge which contains KCl in it. K+ ions of the salt bridge move toward the cathode and Cl− ions of salt bridge move toward the anode.
08. SHE acts as an anode when connected with Cu but as a cathode when connected with the Zn electrode. Explain.
When SHE connected with Cu, copper has a greater reduction potential and acts as a cathode while SHE acts as the anode. When SHE is connected with Zinc, hydrogen has greater reduction potential and acts as a cathode while SHE acts as the anode.
In Galvanic cells, the electrode which has greater reduction potential acts as the cathode.
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