Questions: The following reaction occurs in basic solution. Please balance the following reaction and fill in the missing coefficients ClO2^-(aq) + HPO3^2-(aq) -> Cl^-(aq) + PO4^3-(aq) - Do not include the state (phase) information. - Include all coefficients, even those equal to 1. Provide your answer below: OH^- ClO2 HPO3^2- Cl^-+ PO4^3-+ H2O

The following reaction occurs in basic solution. Please balance the following reaction and fill in the missing coefficients
ClO2^-(aq) + HPO3^2-(aq) -> Cl^-(aq) + PO4^3-(aq)
- Do not include the state (phase) information.
- Include all coefficients, even those equal to 1.

Provide your answer below:
OH^- ClO2 HPO3^2- Cl^-+ PO4^3-+ H2O

Transcript text: The following reaction occurs in basic solution. Please balance the following reaction and fill in the missing coefficients \[ \mathrm{ClO}_{2}^{-}(\mathrm{aq})+\mathrm{HPO}_{3}^{2-}(\mathrm{aq}) \longrightarrow \mathrm{Cl}^{-}(\mathrm{aq})+\mathrm{PO}_{4}^{2-}(\mathrm{aq}) \] - Do not include the state (phase) information. - Include all coefficients, even those equal to 1. Provide your answer below: $\square$ $\mathrm{OH}^{-}$ $\square$ $\mathrm{ClO}_{2}$ $\square$ $\mathrm{HPO}_{3}{ }^{2-}$ $\square$ $\mathrm{Cl}^{-}+$ $\square$ $\mathrm{PO}_{4}{ }^{3-}+$ $\square$ $\mathrm{H}_{2} \mathrm{O}$

Solution

Solution Steps

Step 1: Identify Oxidation and Reduction Half-Reactions

In the given reaction, we need to identify which species are oxidized and reduced.

Oxidation: The oxidation state of phosphorus in $\mathrm{HPO}_{3}^{2-}$ is +3, and it changes to +5 in $\mathrm{PO}_{4}^{3-}$. Therefore, $\mathrm{HPO}_{3}^{2-}$ is oxidized.
Reduction: The oxidation state of chlorine in $\mathrm{ClO}_{2}^{-}$ is +3, and it changes to -1 in $\mathrm{Cl}^{-}$. Therefore, $\mathrm{ClO}_{2}^{-}$ is reduced.

Step 2: Write the Half-Reactions

Write the oxidation and reduction half-reactions separately.

Oxidation Half-Reaction: \[ \mathrm{HPO}_{3}^{2-} \rightarrow \mathrm{PO}_{4}^{3-} \]
Reduction Half-Reaction: \[ \mathrm{ClO}_{2}^{-} \rightarrow \mathrm{Cl}^{-} \]

Step 3: Balance Atoms Other Than O and H

Balance all atoms except for oxygen and hydrogen in each half-reaction.

Oxidation Half-Reaction: Phosphorus is already balanced.
Reduction Half-Reaction: Chlorine is already balanced.

Step 4: Balance Oxygen Atoms

Add $\mathrm{H}_2\mathrm{O}$ to balance the oxygen atoms.

Oxidation Half-Reaction: \[ \mathrm{HPO}_{3}^{2-} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{PO}_{4}^{3-} \]
Reduction Half-Reaction: \[ \mathrm{ClO}_{2}^{-} \rightarrow \mathrm{Cl}^{-} + 2\mathrm{H}_2\mathrm{O} \]

Step 5: Balance Hydrogen Atoms

Add $\mathrm{OH}^{-}$ to balance the hydrogen atoms in basic solution.

Oxidation Half-Reaction: \[ \mathrm{HPO}_{3}^{2-} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{PO}_{4}^{3-} + 2\mathrm{H}^{+} \] Add $\mathrm{OH}^{-}$ to both sides: \[ \mathrm{HPO}_{3}^{2-} + \mathrm{H}_2\mathrm{O} + 2\mathrm{OH}^{-} \rightarrow \mathrm{PO}_{4}^{3-} + 2\mathrm{H}_2\mathrm{O} \]
Reduction Half-Reaction: \[ \mathrm{ClO}_{2}^{-} + 4\mathrm{H}^{+} \rightarrow \mathrm{Cl}^{-} + 2\mathrm{H}_2\mathrm{O} \] Add $\mathrm{OH}^{-}$ to both sides: \[ \mathrm{ClO}_{2}^{-} + 4\mathrm{OH}^{-} \rightarrow \mathrm{Cl}^{-} + 2\mathrm{H}_2\mathrm{O} + 4\mathrm{OH}^{-} \]

Step 6: Balance Charge

Balance the charge by adding electrons.

Oxidation Half-Reaction: \[ \mathrm{HPO}_{3}^{2-} + 2\mathrm{OH}^{-} \rightarrow \mathrm{PO}_{4}^{3-} + 2\mathrm{H}_2\mathrm{O} + 2e^{-} \]
Reduction Half-Reaction: \[ \mathrm{ClO}_{2}^{-} + 4\mathrm{e}^{-} + 4\mathrm{OH}^{-} \rightarrow \mathrm{Cl}^{-} + 2\mathrm{H}_2\mathrm{O} \]

Step 7: Equalize Electrons and Combine Half-Reactions

Multiply the oxidation half-reaction by 2 to equalize the electrons and then add the half-reactions.

Oxidation Half-Reaction (multiplied by 2): \[ 2\mathrm{HPO}_{3}^{2-} + 4\mathrm{OH}^{-} \rightarrow 2\mathrm{PO}_{4}^{3-} + 4\mathrm{H}_2\mathrm{O} + 4e^{-} \]
Combined Reaction: \[ 2\mathrm{HPO}_{3}^{2-} + \mathrm{ClO}_{2}^{-} + 4\mathrm{OH}^{-} \rightarrow 2\mathrm{PO}_{4}^{3-} + \mathrm{Cl}^{-} + 4\mathrm{H}_2\mathrm{O} \]

Final Answer

The balanced reaction with coefficients is:

\[ \boxed{4 \ \mathrm{OH}^{-} + 1 \ \mathrm{ClO}_{2}^{-} + 2 \ \mathrm{HPO}_{3}^{2-} \rightarrow 1 \ \mathrm{Cl}^{-} + 2 \ \mathrm{PO}_{4}^{3-} + 2 \ \mathrm{H}_{2}\mathrm{O}} \]

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