Question

Balance the following chemical reaction by the half reaction by the half reaction method under both acidic and basic conditions. What was oxidized and what was reduced?

IrO₃ + V(OH)₄⁺² → Ir(OH)₅⁺³ + V⁺²

Answer 1

To balance the equation:

The oxidation states of each of the elements of the equation must be placed, that is:

To determine the oxidation state of the chemical species that are being reduced and oxidized, the oxidation states of the elements present in the chemical species must be added and this must be equal to the net charge of the chemical species (compound or ion).

The element that is oxidized and reduced is determined:

The Ir goes from oxidation state +4 to +8, increases its oxidation state, oxidizing, while the V goes from oxidation state +6 to +2, decreases its oxidation state, reducing it

The reduction and oxidation semireactions are written:

Each semireaction is multiplied by the number of electrons transferred by the oxidizing and reducing agent respectively, that is:

Resolviendo, nos queda:

As observed in the previous equation, the atoms of Ir and V are balanced, that is, the number of atoms of each element is equal on both sides of the chemical equation. To complete the balance, the load must be balanced, as the reaction is done in acid medium, we add H+ ions and H2O molecules, this is:

With this the equation is balanced in atoms and charge.