Match the column (for electrolytic refining of Cu):
Column−I Column−II(a)Anode(p)Thin sheets of pure Cu(b)Cathode(q)An aqueous solution of copper sulphate containing H2SO4(c)Electrolyte(r)Ag,Au(d)Anode mud(s)Impure metal of Cu
(a) s; (b) p; (c) q; (d) r
Irrespective of the cell type - Daniel or electrolytic - at the anode, it is always oxidation.
Since the context is the electrolytic refining of copper, we want impure copper to become Cu2+ ions and move into the electrolyte. We then expect Cu2+ to get reduced at the cathode. So at the cathode, pure copper will be deposited (reduced). This clearly means that the anode will be made of impure metal, which has some valuable impurities like Ag,Au and Pt. These impurities (metals which are highly unreactive and low on the electrochemical series), will get deposited below anode as anode mud.