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Titanium Extraction

As far as I can see there is only one UK-based Exam Board that wants the extraction of titanium, and that is AQA. They only want the conditions and equations for the reactions involved, and that is all you will find on this page together with a few comments related to method used.

If you want more details, you can find them on a useful page from The Essential Chemistry Industry from the University of York.

Titanium Extraction

The overall process

Titanium is extracted from its ore, rutile – TiO2. It is first converted into titanium(IV) chloride, which is then reduced to titanium using either magnesium or sodium.

Conversion of TiO2 into TiCl4

The ore rutile (impure titanium(IV) oxide) is heated with chlorine and coke at a temperature of about 1000°C.

Note: There are other reactions occurring as well in which the other product is either carbon dioxide or carbonyl chloride, COCl2. AQA give the one producing carbon monoxide as their first choice, but will also accept one producing carbon dioxide.

{\underset{m.p.~1,843\degree{C}}{\text{Ti}\text{O}_{2(s)}}} + 2\text{Cl}_{2(g)} + {\underset{m.p.~3.642\degree{\text{C}}}{2\text{C}_{(s)}}} \longrightarrow {\underset{b.p.~136\degree{C}}{\text{TiCl}_{4(g)}}} + 2\text{CO}_{(g)}

Other metal chlorides are formed as well because of other metal compounds in the ore. Very pure liquid titanium(IV) chloride can be separated from the other chlorides by fractional distillation under an argon or nitrogen atmosphere, and is stored in totally dry tanks.

Note: Titanium(IV) chloride is a typical covalent chloride. It is a colourless liquid which fumes in moist air due to reaction with water to give titanium(IV) oxide and fumes of hydrogen chloride. Everything has to be kept very dry to stop this happening.

Reduction of the titanium(IV) chloride

TiCl4 can be reduced using either magnesium or sodium. AQA will accept either, and so I am just giving the magnesium one.

Titanium(IV) chloride vapour is passed into a reaction vessel containing molten magnesium in an argon atmosphere, and the temperature is increased to about 1000°C. The reduction process is very slow, taking about 2 days, followed by several more days of cooling.

\text{TiCl}_{4(g)} + {\underset{m.p.~650\degree{C}}{2\text{Mg}_{(l)}}} \longrightarrow {\underset{m.p.~1,668\degree{C}}{\text{Ti}_{(s)}}} + {\underset{m.p.~1,714\degree{C}}{2\text{MgCl}_{2(l)}}}

When it is cool, the reaction mixture is crushed, and dilute hydrochloric acid is added to react with any excess magnesium to form more magnesium chloride. All the magnesium chloride dissolves in the water present, and the remaining titanium is processed further to purify it.

Other Thoughts

Why is this extraction process used?

Titanium can't be extracted by reducing the ore using carbon as a cheap reducing agent. The problem is that titanium forms a carbide, TiC, if it is heated with carbon, so you don't get the pure metal that you need. The presence of the carbide makes the metal very brittle.

That means that you have to use an alternative reducing agent. In the case of titanium, the reducing agent is either sodium or magnesium. Both of these would, of course, first have to be extracted from their ores by expensive processes.

Other problems

Note: If you follow the link at the top of the page, you will find that there is now a continuous flow method involving sodium, and even a method of producing titanium electrolytically.

Questions to test your understanding

Questions on titanium extraction