Question

PbO2 + 4HCl --- PbCl2 + Cl2 + 2H2O who buys electrons and who loses electrons?​

Answer 1

Answer: Electrons are taken up by $PbO_2$ and they are lost by $HCl$

Explanation:

Redox reaction is defined as the reaction in which oxidation and reduction take place simultaneously. It is also called the reaction where the exchange of electrons takes place.

An oxidation reaction is defined as the reaction in which a chemical species loses electrons takes place. In this reaction, the oxidation state of a substance gets increased.

A reduction reaction is defined as the reaction in which a chemical species gains electrons takes place. In this reaction, the oxidation state of a substance gets reduced.

For the given chemical reaction:

$PbO_2+4HCl\rightarrow PbCl_2+Cl_2+2H_2O$

The half-reactions for this redox rection follows:

Oxidation half-reaction:  $2HCl\rightarrow ClO_2 + 2e^-$

Reduction half-reaction:  $PbO_2+2e^-\rightarrow PbCl_2$

Hence, electrons are taken up by $PbO_2$ and they are lost by $HCl$