Question

Complete and balance the following redox reaction in acidic solution. Be sure to include the proper phases for all species within the reaction. As 2

​
O 3
​
( s)+NO 3
​
(aq)→H 3
​
AsO 4
​
(aq)+N 2
​
O 3
​
(aq)

Answer 1

The balanced redox equation for the given reaction in acidic solution is 2As2O3(s) + 16HNO3(aq) → 6H3AsO4(aq) + 4NO2(g) + 11H2O(l)

Step-by-step explanation:

The balanced redox equation for the given reaction in acidic solution is:

2As2O3(s) + 16HNO3(aq) → 6H3AsO4(aq) + 4NO2(g) + 11H2O(l)

Answer 2

The balanced equation is;

`3As_2O_3 + 4NO_3 + 9H_2O ---- > 6H_3AsO_4 + 2N_2O_3`

It is important to make sure that each element has the same number of atoms on both sides of the equation in an acidic medium. To accomplish this balance, modify the reactant and product coefficients.

The coefficients of arsenic (As), oxygen (O), nitrogen (N), and hydrogen (H) in this equation must be changed in order to maintain the law of conservation of mass and produce a balanced equation in an acidic environment.

When the reaction is taking place in the acidic medium, it will balance as follows;
`3As_2O_3 + 4NO_3 + 9H_2O ---- > 6H_3AsO_4 + 2N_2O_3`