In electrolytic refining, the pure metal is used as:
a cathode
In electrolytic refining, a thin strip of pure metal is made the cathode (the negative electrode) and the impure metal is made the anode (the positive electrode), with a solution of a salt of the metal acting as the electrolyte.
When current is passed, the impure anode dissolves into the electrolyte and pure metal is deposited onto the pure cathode, so the cathode grows in purity and thickness.
"Sulphur" is wrong because sulphur is a non-metal and plays no role as the electrode here.
"An electrolyte" is wrong because the electrolyte is the dissolved metal-salt solution, not the solid pure metal.
"An anode" is wrong because the anode is made of the impure metal that dissolves away, not the pure metal.
Hence, in electrolytic refining the pure metal is used as a cathode.
Similar Questions
During the electrolytic refining of copper, which of the following correctly matches the components and their roles?
Component Role in Refining Process A. Pure Copper i. Anode B. Impure Copper ii. Cathode C. Acidified Copper Sulphate iii. Electrolyte Which of the following statements are correct for electrolytic refining? a. Copper, zinc, and nickel are refined electrolytically. b. In this method, a thin strip of pure metal is used as cathode. c. The insoluble impurities settled at bottom of the anode are known as anode mud.
What happens at the anode during anodising?
Which method is commonly used to extract sodium from its compound?
Which of the following metals is usually extracted from its ore by electrolytic reduction?
Which of the following is a product formed at the cathode during the electrolysis of brine?
Anodising is a process used to improve the appearance and durability of aluminium articles. Which of the following statements best explains the principle behind anodising?
Select the option that is true regarding the following two statements labelled Assertion (A) and Reason (R).
Assertion (A): Metals such as sodium and potassium are extracted by electrolysis.
Reason (R): These metals are highly reactive and cannot be obtained by reduction with carbon.
What is used as an anode in the electrolytic refining of nickel?
Important Questions from Electrochemistry
- At $298 \, K$, given the standard electrode potentials: $E^\circ_{Cu^{2+}/Cu} = 0.34 \, V$, $E^\circ_{Zn^{2+}/Zn} = -0.76 \, V$, $E^\circ_{Fe^{2+}/Fe} = -0.44 \, V$, and $E^\circ_{Ag^{+}/Ag} = 0.80 \, V$.
Based on these values, which of the following reactions is NOT expected to occur spontaneously under standard conditions? You are given three metals 'X', 'Y' and 'Z'. Metal 'X' is found to react with an aqueous solution of both YSO 4and ZSO 4whereas metal 'Z' is found to react only with aqueous solution of YSO 4. Based on these observations, select the correct statement from the following.
If the overpotential of an electrolysis process is increased from 0.5 V to 0.6 V, then the ratio of current densities (In \(\frac{\int0.6 }{\int0.5}\)) of the electrolysis will be equal to (given transfer co - efficient = 0.5)
The chemical potential (μ) of a 2 molar Na2SO4 solution is expressed in terms of mean ionic activity co - efficient (γ±) as
The E°(M+/M) of the cell, SHE||MX|M can be obtained from the plot of (E cell is the cell potential and m is the molality of ideal dilute solution of MX)
