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Chapter 21: Problem 9

Oxalic acid is often used to remove rust stains. What properties of oxalic acid allow it to do this?

Short Answer

Expert verified
Oxalic acid's ability to remove rust stains comes from its property of forming soluble complexes with iron(III) ions. It reacts with hydrated iron(III) oxide (rust) to form a soluble iron(III) oxalate complex that can be easily washed away. The chemical equation representing this reaction is: \[ 6 \text{Fe}_2\text{O}_3\cdot x\text{H}_2\text{O} + 6\text{C}_2\text{H}_2\text{O}_4 \rightarrow 2\text{Fe}_3\text{C}_6\text{H}_2\textit{O}_11 + 3\text{H}_2\text{O} \]

Step by step solution

01

Introduction: What is Oxalic Acid?

Oxalic acid is a simple dicarboxylic acid with the chemical formula C2H2O4. It is a strong organic acid that naturally occurs in many fruits and vegetables. It's commonly used as a cleaning agent for various purposes, including rust removal.
02

Iron Oxide and Rust

Rust is a reddish-brown flaky substance that forms on the surface of iron and steel when they react with oxygen and moisture in the environment. The main chemical component of rust is hydrated iron(III) oxide (Fe2O3 路 xH2O). Over time, rust can weaken the metal and cause structural damage.
03

Oxalic Acid and Rust Removal

One of the main properties of oxalic acid that allows it to remove rust is its ability to form soluble complexes with iron(III) ions. When oxalic acid comes into contact with rust, it forms a soluble iron(III) oxalate complex, which can be easily washed away with water. The overall reaction can be represented by the following chemical equation: \[ 6 \text{Fe}_2\text{O}_3\cdot x\text{H}_2\text{O} + 6\text{C}_2\text{H}_2\text{O}_4 \rightarrow 2\text{Fe}_3\text{C}_6\text{H}_2\textit{O}_11 + 3\text{H}_2\text{O} \] Here, hydrated iron(III) oxide reacts with oxalic acid to form iron(III) oxalate complex and water.
04

Safety Considerations with Oxalic Acid

While oxalic acid is effective at removing rust, it is important to handle it with care due to its hazardous properties. It is a strong acid and can cause skin irritation, and its solutions can be toxic if ingested. It's important to wear gloves and protective eyewear when using oxalic acid, and to use it in a well-ventilated area. In conclusion, the key property of oxalic acid that allows it to remove rust is its ability to form soluble iron(III) oxalate complexes, which can be easily washed away. This makes it an effective cleaning agent for removing rust stains and restoring the appearance and strength of iron and steel surfaces.

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Most popular questions from this chapter

Consider the pseudo-octahedral complex ion of \(\mathrm{Cr}^{3+}\) , where A and \(\mathrm{B}\) represent ligands. Ligand A produces a stronger crystal field than ligand B. Draw an appropriate crystal field diagram for this complex ion (assume the A ligands are on the \(z\) -axis).

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The ferrate ion, \(\mathrm{FeO}_{4}^{2-}\) , is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in FeO \(_{4}^{2-},\) and what is the electron configuration of iron in this polyatomic ion? b. If 25.0 \(\mathrm{mL}\) of a 0.243 \(\mathrm{M} \mathrm{FeO}_{4}^{2-}\) solution is allowed to react with 55.0 \(\mathrm{mL}\) of 1.45 \(\mathrm{M}\) aqueous ammonia, what volume of nitrogen gas can form at \(25^{\circ} \mathrm{C}\) and 1.50 \(\mathrm{atm}\) ?
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