Question

Hello, I need help answering these questions:

Write the net ionic equation for sulfuric acid solution reacting with the sodium oxalate solution.

Write and balance the net ionic equation for the oxalic acid reacting with the permanganate ion in acidic solution.

Thank you!

Answer 1

Oxalic acid is a weak acid.

Comment if any problem.

Answer 2

Net Ionic Equations

1. Sulfuric Acid + Sodium Oxalate Reaction

Molecular Equation:

$${\text{H}}_2{\text{SO}}_4(aq)+{\text{Na}}_2{\text{C}}_2{\text{O}}_4(aq)\to 2{\text{Na}}^{+}(aq)+{\text{SO}}_4^{2-}(aq)+{\text{H}}_2{\text{C}}_2{\text{O}}_4(aq)$$

Net Ionic Equation:

$$\boxed{{\displaystyle 2{\text{H}}^{+}(aq)+{\text{C}}_2{\text{O}}_4^{2-}(aq)\to {\text{H}}_2{\text{C}}_2{\text{O}}_4(aq)}}$$

Explanation:

• Spectator ions (${\text{Na}}^{+}$, ${\text{SO}}_4^{2-}$) are removed.

• Oxalate ion (${\text{C}}_2{\text{O}}_4^{2-}$) protonates to form oxalic acid (${\text{H}}_2{\text{C}}_2{\text{O}}_4$).

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2. Oxalic Acid + Permanganate (Acidic Solution) Reaction

Balanced Net Ionic Equation:

$$\boxed{{\displaystyle 5{\text{H}}_2{\text{C}}_2{\text{O}}_4(aq)+2{\text{MnO}}_4^{-}(aq)+6{\text{H}}^{+}(aq)\to 10{\text{CO}}_2(g)+2{\text{Mn}}^{2+}(aq)+8{\text{H}}_2\text{O}(l)}}$$

Explanation:

• Oxidation: ${\text{C}}_2{\text{O}}_4^{2-}\to 2{\text{CO}}_2+2e^{-}$ (×5).

• Reduction: ${\text{MnO}}_4^{-}+8{\text{H}}^{+}+5e^{-}\to {\text{Mn}}^{2+}+4{\text{H}}_2\text{O}$ (×2).

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• Key Features:

• Manganese reduces from $+7$ to $+2$.

• Carbon oxidizes from $+3$ to $+4$.

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Key Notes:

• Acidic Conditions: Essential to balance ${\text{MnO}}_4^{-}$ reactions (provides ${\text{H}}^{+}$ for water formation).

• Gas Formation: ${\text{CO}}_2$ escapes, driving the reaction forward.