The element bromine was first prepared by oxidation of aqueous potassium bromide with solid manganese(IV) oxide. Write a balanced net ionic equation for the reaction in an aqueous acidic solution. Mn2+ is also formed.

Verified step by step guidance

1. Identify the reactants and products in the reaction: Potassium bromide (KBr) and manganese(IV) oxide (MnO2) are the reactants, while bromine (Br2) and Mn2+ are the products.
2. Write the half-reaction for the oxidation of bromide ions (Br-) to bromine (Br2). In acidic solution, this involves the loss of electrons by bromide ions.
3. Write the half-reaction for the reduction of manganese(IV) oxide (MnO2) to Mn2+. In acidic solution, this involves the gain of electrons by MnO2.
4. Balance each half-reaction for mass and charge. This includes balancing the atoms other than O and H first, then balancing O atoms by adding H2O, H atoms by adding H+, and finally balancing the charge by adding electrons.
5. Combine the balanced half-reactions to form the overall balanced net ionic equation, ensuring that the electrons lost in the oxidation half-reaction equal the electrons gained in the reduction half-reaction.