In a particular redox reaction, clo2– is oxidized to clo4– and ag is reduced to ag. complete and balance the equation for this reaction in acidic solution. phases are optional.

To write a complete balanced reaction of a redox reaction, we need to know the half reactions of the molecules involved in the reaction and to balance these reactions. From, the problem statement ClO2- is oxidized to ClO4- so the half reaction would be:

(ClO)2- = (ClO)4- 

To balance,
We first balance the elements except O and H in the reaction.
(ClO2)- = (ClO4)- 
Then, we balance O by adding H2O and balance H by adding H+
(ClO2)- + 2H2O = (ClO4)- + 2H+ 
Then, we balance the charges by adding electrons,
(ClO2)- + 2H2O = (ClO4)- + 2H+ + e-

Then for Ag+ to Ag,
Ag+ = Ag

We just need to balance the charge,
Ag+ + e- = Ag

To determine the final equation, we add both half reactions:

(ClO2)- + 2H2O = (ClO4)- + 2H+ + e-
Ag+ + e- = Ag

ClO2- +Ag+ +2H2O---> ClO4^- + Ag + 2H+
 

It would be

Woah that’s a lot to read xd i’ll try though. i’ll get back t you if. i know the andwer