Question

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.

Short answer

Answer: (a) The balanced net ionic equation for the electrolytic decomposition of hydrogen fluoride is: 2HF -> H2 + F2 (b) The balanced net ionic equation for the oxidation of iodide ion to iodine by hydrogen peroxide in acidic solution is: 2I- + H2O2 + 2H+ -> I2 + 2H2O

Step-by-step solution

(a) Balanced molecular equation for the electrolytic decomposition of hydrogen fluoride

First, we need to write a balanced molecular equation for the electrolytic decomposition of hydrogen fluoride (HF). During this process, hydrogen fluoride is decomposed into its constituent elements, hydrogen gas (H2) and fluorine gas (F2) at the electrodes. The balanced equation is: 2HF -> H2 + F2

(a) Spectator ions

Since this is a decomposition and there are no other species involved in the equation, there are no spectator ions in this reaction.

(a) Balanced net ionic equation

Since there are no spectator ions, the net ionic equation is the same as the balanced molecular equation: 2HF -> H2 + F2

(b) Balanced molecular equation for the oxidation of iodide ion to iodine by hydrogen peroxide in acidic solution

We are given that iodide ion (I-) is oxidized to iodine (I2) by hydrogen peroxide (H2O2) in acidic solution. Hydrogen peroxide is reduced to water (H2O). The balanced equation is: 2I- + H2O2 + 2H+ -> I2 + 2H2O

(b) Spectator ions

In this reaction, there are no spectator ions, as all species participate in the process.

(b) Balanced net ionic equation

Since there are no spectator ions, the net ionic equation is the same as the balanced molecular equation: 2I- + H2O2 + 2H+ -> I2 + 2H2O