Write a balanced net ionic equation for (a) the electrolytic decomposition of hydrogen fluoride. (b) the oxidation of iodide ion to iodine by hydrogen peroxide in acidic solution. Hydrogen peroxide is reduced to water.

Step 1: Write the overall reaction First, we know that HF undergoes an electrolytic decomposition, which means that an electric current is used to break it down into its elements: hydrogen (H2) and fluoride (F2). HF → H2 + F2 Step 2: Write the half-reactions To write the net ionic equation, we need to identify the half-reactions involved. The oxidation half-reaction is: 2HF → H2 + 2F- + 2e- The reduction half-reaction is: 2F- + 2e- → F2 Step 3: Balance the half-reactions for mass and charge In this case, both half-reactions are already balanced for both mass and charge. If they were not balanced, we would need to adjust the coefficients accordingly. Step 4: Combine the half-reactions Now, we can combine the half-reactions to form the balanced net ionic equation: 2HF → H2 + F2 + 2F- + 2e- 2F- + 2e- → F2 ----------------------------------- Net ionic equation: 2HF → H2 + 2F2

Step 1: Write the overall reaction We know that iodide ion (I-) is oxidized to iodine (I2) by hydrogen peroxide (H2O2) in an acidic solution. 2I- + H2O2 → I2 + 2H2O Step 2: Write the half-reactions To write the net ionic equation, we need to identify the half-reactions involved. The oxidation half-reaction is: 2I- → I2 + 2e- The reduction half-reaction is: H2O2 + 2H+ + 2e- → 2H2O Step 3: Balance the half-reactions for mass and charge The oxidation half-reaction is already balanced, but the reduction half-reaction needs to be balanced for both mass and charge. H2O2 + 2H+ + 2e- → 2H2O Now both half-reactions are balanced. Step 4: Combine the half-reactions Now, we can combine the half-reactions to form the balanced net ionic equation: 2I- → I2 + 2e- H2O2 + 2H+ + 2e- → 2H2O ------------------------------------ Net ionic equation: 2I- + H2O2 + 2H+ → I2 + 2H2O