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Chapter 22: Problem 58

Write complete balanced half-reactions for (a) reduction of nitrate ion to \(\mathrm{NO}\) in acidic solution, \((\mathbf{b})\) oxidation of \(\mathrm{HNO}_{2}\) to \(\mathrm{NO}_{2}\) in acidic solution.

Short Answer

Expert verified
The balanced half-reactions for the given scenarios are: (a) Reduction of nitrate ion to NO in acidic solution: \(NO_3^- + 6H^+ + 5e^- → NO + 3H_2O\) (b) Oxidation of HNO2 to NO2 in acidic solution: \(HNO_2 → NO_2 + H_2O\)

Step by step solution

01

Write the unbalanced half-reaction

The given half-reaction is the reduction of nitrate ion (\(NO_3^-\)) to nitric oxide (NO). Write it down as: \(NO_3^- → NO\)
02

Balance the oxygen atoms

There are three oxygen atoms in the reactant and none in the product. To balance them, add three water (\(H_2O\)) molecules to the right side of the equation: \(NO_3^- → NO + 3H_2O\)
03

Balance the hydrogen atoms

There are six hydrogen atoms on the right side of the equation and none on the left side. To balance them, add six proton (\(H^+\)) ions to the left side of the equation: \(NO_3^- + 6H^+ → NO + 3H_2O\)
04

Balance the charges

The left side of the equation has a total charge of +5, and the right side has a total charge of 0. To balance the charges, add five electrons (\(e^-\)) to the left side of the equation: \(NO_3^- + 6H^+ + 5e^- → NO + 3H_2O\) The balanced half-reaction for the reduction of nitrate ion to NO in acidic solution is: \(NO_3^- + 6H^+ + 5e^- → NO + 3H_2O\) #Part (b): Oxidation of HNO2 to NO2 in acidic solution#
05

Write the unbalanced half-reaction

The given half-reaction is the oxidation of nitrous acid (\(HNO_2\)) to nitrogen dioxide (\(NO_2\)). Write it down as: \(HNO_2 → NO_2\)
06

Balance the oxygen atoms

Both sides of the equation have two oxygen atoms, so they are already balanced.
07

Balance the hydrogen atoms

There is one hydrogen atom on the left side of the equation and none on the right side. To balance it, add one water molecule (\(H_2O\)) to the right side of the equation: \(HNO_2 → NO_2 + H_2O\)
08

Balance the charges

The left side of the equation has a total charge of 0, and the right side also has a total charge of 0. Adding electrons is not necessary in this case. The balanced half-reaction for the oxidation of HNO2 to NO2 in acidic solution is: \(HNO_2 → NO_2 + H_2O\)

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Most popular questions from this chapter

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