Write the net ionic equation for the reaction of citric acid and sodium hydroxide. NG 1 Info Mouse over the picture above to view the 4 components of a reactant or product that are needed to write chemical equations.
Write the balanced net ionic equation for the reaction between citric acid and sodium hydroxide Mouse over the grey boxes for information on 2 NH4 coefficients, formulas, charges and states of matter. The coefficient and formula are required components – the components of a chemical equation. H + ——- Work Problem
The Correct Answer and Explanation is :
Net Ionic Equation for the Reaction of Citric Acid and Sodium Hydroxide:
Balanced Net Ionic Equation:
[
\text{C}_6\text{H}_5\text{O}_7^{3-} + 3 \text{OH}^- \rightarrow \text{C}_6\text{H}_5\text{O}_7^{3-} + 3 \text{H}_2\text{O}
]
Explanation (300 words)
1. Understanding the Reactants:
Citric acid (C₆H₈O₇) is a weak, triprotic acid, meaning it can donate up to three hydrogen ions (H⁺). It ionizes in water as follows:
[
\text{C}_6\text{H}_8\text{O}_7 \rightleftharpoons \text{C}_6\text{H}_7\text{O}_7^- + H^+
]
[
\text{C}_6\text{H}_7\text{O}_7^- \rightleftharpoons \text{C}_6\text{H}_6\text{O}_7^{2-} + H^+
]
[
\text{C}_6\text{H}_6\text{O}_7^{2-} \rightleftharpoons \text{C}_6\text{H}_5\text{O}_7^{3-} + H^+
]
Since citric acid has three acidic protons, it reacts with three hydroxide ions (OH⁻) from sodium hydroxide (NaOH) in a neutralization reaction.
2. Understanding the Reaction with NaOH:
Sodium hydroxide is a strong base that completely dissociates in water:
[
\text{NaOH} \rightarrow \text{Na}^+ + \text{OH}^-
]
Each hydroxide ion neutralizes a hydrogen ion from citric acid:
[
\text{H}^+ + \text{OH}^- \rightarrow \text{H}_2\text{O}
]
Since citric acid donates three protons, it requires three hydroxide ions for complete neutralization.
3. Writing the Net Ionic Equation:
Since sodium ions (Na⁺) are spectator ions and do not participate in the actual reaction, we remove them from the full equation, leaving only the reacting species:
[
\text{C}_6\text{H}_8\text{O}_7 + 3 \text{OH}^- \rightarrow \text{C}_6\text{H}_5\text{O}_7^{3-} + 3 \text{H}_2\text{O}
]
This net ionic equation represents the neutralization of citric acid by sodium hydroxide, forming citrate ions and water.
4. Summary:
This reaction is a classic acid-base neutralization. The citric acid donates its hydrogen ions, while hydroxide ions neutralize them, forming water. The final product is the citrate ion (C₆H₅O₇³⁻) and water molecules, indicating the complete neutralization of citric acid.