Step-1: To identify the atoms whose oxidation numbers have undergone a change. Writing the oxidation number of each atom above its symbol,
we have
Step-2:
Oxidation:
[As, from +3 to +5 i.e., 2 unit change, S from to O also 2 in change]
Reduction:
Step-3: To balance the oxidation half Eq. (i)
(a) Balance all the atoms other than H and O. Multiply AsO43- by 2 and S by 3 on RHS of Eq. (i) we have,
(c) Balance charge by adding H+ ions. The total charge on RHS of Eq. (iv) is -16 and zero the LHS therefore, add 16H+ to RHS of Eq. (iv) we have,
(d) Balance O atoms by adding H2O molecules.
The H-atoms get automatically balanced. Thus Eq. (vi) represents the balanced oxidation half equation.
Step-4: To balance the reduction half Eq. (ii)
(a) Balance oxidation number by adding electrons.
(b) Balance charge by adding H+ ions.
(c) Balance H+ by adding H2O
Thus, Eq. (ix) represents the balanced reduction half equation Eq. (ix) by 10 and Eq, (vi) by 3 and (ix) 10 + (vi) x 3
Step-5: