Question

For a particular redox reaction, SO2−3 is oxidized to SO2−4, and Ag+ is reduced to Ag. Complete and balance the equation for this reaction in basic solution. Phases are optional.

Answer 1

To balance the redox reaction of SO₂⁻³to SO₂⁻⁴ and Ag+ to Ag in a basic solution, the half-reactions are written, balanced for electrons, and then combined. Additional OH− and H₂O are added to balance for mass and charge in a basic solution, resulting in a balanced equation.

Step-by-step explanation:

The question is about balancing a redox reaction in a basic solution, where SO₂⁻³ is oxidized to SO₂⁻⁴, and Ag+ is reduced to Ag. Since we have two half-reactions, we need to write, balance, and then combine them. It's important to remember to balance the half-reactions for both mass and charge by adding H₂O, OH⁻, and electrons as needed.

First, we write the half-reactions:

• Oxidation (losing electrons): SO₂⁻³ → SO₂⁻⁴ + 2 e
• Reduction (gaining electrons): Ag+ + e→ Ag

Since the oxidation half-reaction involves the transfer of 2 electrons, we need to multiply the reduction half-reaction by 2 :

• Oxidation:SO₂⁻³ → SO₂⁻⁴ + 2 e−
• Reduction: 2 Ag+ + 2 e− → 2 Ag

Combining these balanced half-reactions, we get:

SO₂⁻³ + 2 Ag+ → SO₂⁻⁴ + 2 Ag

However, this is not completely balanced for a basic solution. We may need to add OH− to both sides to balance for H₂O and then adjust the waters if necessary.

For basic solution:

3 H₂O + SO₂⁻³ + 2 Ag+ → SO₂⁻⁴ + 2 Ag + 6 OH⁻

We have added 3 H₂O to the products and 6 OH⁻ to the reactants, ensuring mass balance. Now the equation is balanced, reflecting mass and charge conservation in a basic solution.

Answer 2

SO3^2- + 2Ag^+ + 2OH^- → SO4^2- + Ag(s) + H2O

Step-by-step explanation:

In this redox reaction, sulfur dioxide ion (SO3^2-) is oxidized to sulfate ion (SO4^2-), and silver ion (Ag^+) is reduced to silver metal (Ag) in a basic solution. To balance the equation, it's crucial to ensure that the number of atoms for each element is the same on both sides of the equation and that the charge is balanced.

Firstly, balance the atoms of each element other than hydrogen and oxygen. In this case, there is one sulfur atom on both sides, but the oxygen atoms need balancing. Add two hydroxide ions (OH^-) to the reactant side to balance the oxygens:

SO3^2- + 2Ag^+ + 2OH^- → SO4^2- + Ag(s)

Now, balance the hydrogen atoms by adding water molecules (H2O) to the reactant side. In this case, add two water molecules:

SO3^2- + 2Ag^+ + 2OH^- → SO4^2- + Ag(s) + 2H2O

Finally, balance the charge by adding electrons (e^-). In this reaction, electrons are added to the left side (reactant) to balance the charge. The overall balanced equation in basic solution is:

SO3^2- + 2Ag^+ + 2OH^- → SO4^2- + Ag(s) + H2O

This balanced equation ensures that the number of atoms for each element is the same on both sides and that the charge is balanced, representing the redox reaction in basic solution.