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Chapter 20: Problem 35

Oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), is sometimes used to clean rust stains from sinks and bathtubs. Explain the chemistry underlying this cleaning action.

Short Answer

Expert verified
Oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), is used to clean rust since it reacts with iron(III) oxide (rust) in a redox reaction to form a soluble iron(III) oxalate complex, which is easily rinsed away with water, removing the rust stain.

Step by step solution

01

Rust Composition

Rust is essentially iron(III) oxide \(\mathrm{Fe}_{2} \mathrm{O}_{3}\). This reddish-brown compound typically forms on iron or steel when it comes into contact with water and oxygen.
02

Oxalic Acid Properties

Oxalic acid \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), is a powerful acid that is capable of reducing other substances. This reduction potential allows it to react with rust.
03

Reaction between Rust and Oxalic Acid

When oxalic acid comes into contact with rust (iron(III) oxide), it reacts to form a soluble complex. This reaction can be represented by the chemical equation: \[ 6 \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4} + 2 \mathrm{Fe}_{2} \mathrm{O}_{3} \longrightarrow 2 \mathrm{Fe}_{2} (\mathrm{C}_{2} \mathrm{O}_{4})_{3}.\mathrm{H}_{2} \mathrm{O} + 6 \mathrm{H}_{2} \mathrm{O} \] This soluble iron(III) oxalate complex is easily washed away, leaving the surface clean of rust.
04

Final Cleaning Process

The iron(III) oxalate complex is then washed away with water, leaving a clean surface. It is important to fully rinse off all oxalic acid, as its strong acidic nature can be corrosive, thereby damaging the surface if left in contact for long periods.

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Most popular questions from this chapter

Write the formulas for each of these ions and compounds: (a) tetrahydroxozincate(II), (b) pentaaquochlorochromium(III) chloride, (c) tetrabromocuprate(II), (d) ethylenediaminetetraacetatoferrate(II).

Give the oxidation numbers of the metals in these species: (a) \(\mathrm{K}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{K}_{3}\left[\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (c) \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\)

Briefly describe the crystal field theory. Define the following terms: crystal field splitting, high-spin complex, low-spin complex, spectrochemical series.

The \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) ion, which has a square planar geometry, is diamagnetic, whereas the \(\left[\mathrm{NiCl}_{4}\right]^{2-}\) ion, which has a tetrahedral geometry, is paramagnetic. Show the crystal field splitting diagrams for those two complexes.

Compounds containing the \(\mathrm{Sc}^{3+}\) ion are colorless, whereas those containing the \(\mathrm{Ti}^{3+}\) ion are colored. Explain.
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