The redox equation H3AsO3 + I2 → H3AsO4 + I− in acidic conditions is balanced by writing half-reactions, balancing atoms and charges, and combining them with the appropriate number of H+ ions to ensure charge balance.
Balance the Redox Equation in Acidic Conditions
To balance the equation H3AsO3 + I2 → H3AsO4 + I− in acidic conditions, we need to balance the atoms and charges by adding H+ ions and water molecules as necessary. First, we write the half-reactions for oxidation and reduction. For the oxidizing agent H3AsO3, it changes to H3AsO4, gaining oxygen atoms. For the reducing agent I2, it reduces to 2I−.
Next, we balance the atoms other than oxygen and hydrogen. Then, we add H2O to balance oxygen and H+ to balance hydrogen. Finally, we balance the charge by adding electrons as necessary. Once the half-reactions are balanced, we combine them, ensuring that the electrons cancel out. After balancing, we should add any necessary H+ ions to ensure the charge is balanced on both sides of the equation.
We then combine the two half-reactions and simplify to get the balanced equation.
Balancing the redox reaction in acidic conditions involves careful adjustment of atoms, charges, and incorporating H+ ions for charge balance, leading to a correctly balanced chemical equation.