Missing image Potassium_chloride.jpg Potassium chloride Potassium chloride
IUPAC name potassium chloride
General
Molecular formula	KCl
Molecular weight	74.55 amu
Appearance	white crystalline solid
CAS number	[7447-40-7]
MSDS	Potassium chloride MSDS
Other names
sylvite (mineral form) muriate of potash
Bulk Properties
Density	1.987 g/cm3
Solubility	water_(molecule): 34.4 g/ cm3 (cold) ethanol: 0.4 g/ cm3 acetone: insoluble
Melting point	776 °C (1049 K)
boiling (sublimation) point	1500 °C (1770 K)
Hazards:	see text
Structure
Crystal structure	Face-centred cubic
Hydrates	none believed known
Related Compounds
potassium fluoride potassium bromide potassium iodide	sodium chloride rubidium chloride

Contents

1 Overview 2 Chemical Properties 3 Manufacture/Extraction 4 Uses 5 Biological/Medical Properties 6 Precautions 7 Suppliers/Manufacturers 8 References

Overview

The chemical compound potassium chloride (KCl) is a metal halide composed of potassium and chlorine. In a pure state it is odourless, with a white to colourless vitreous crystal, with a face-centred cubic structure that cleaves easily in three directions. KCl is used in medicine, scientific applications, food processing and in judicial execution through lethal injection. It occurs naturally as the mineral sylvite and in combination with sodium chloride as sylvinite.

Chemical Properties

Potassium chloride can react as a source of chloride ion. As with any other soluble ionic chloride, it will precipitate insoluble chlorides when added to a solution of an appropriate metal salt such as silver nitrate:

KCl(aq) + Ag(NO₃)(aq) -----> AgCl(s) + KNO₃(aq)

Although potassium is more electropositive than sodium, KCl can be reduced to the metal by reaction with metallic sodium if the potassium is removed by distillation, due to Le Chatelier's principle:

Missing image
Potassium_prep.gif

This method is the main method for producing metallic potassium. Electrolysis (used for sodium) fails because of the high solubility of potassium in molten KCl.

Manufacture/Extraction

Potassium chloride occurs naturally as sylvite, and it can be extracted from sylvinite. It is also extracted from salt water and can be manufactured by crystallization from solution, flotation or electrostatic separation from suitable minerals. It is a by-product of the making of nitric acid from potassium nitrate and hydrochloric acid.

Uses

The majority of the potassium chloride produced is used for making fertilizer^[2], since the growth of many plants is limited by their potassium intake. As a chemical feedstock it is used for the manufacture of potassium hydroxide and potassium metal. It is also used in medicine, scientific applications, food processing and in judicial execution through lethal injection.

Biological/Medical Properties

Potassium is vital in the human body and oral potassium chloride is the common means to replenish it, although it can also be diluted and given intravenously. Medically it is used in the treatment of hypokalemia and associated conditions, for digitalis poisoning, and as an electrolyte replenisher. Side effects can include gastrointestinal discomfort including nausea and vomiting, diarrhea and bleeding of the gut. Overdoses cause hyperkalemia which can lead to paresthesia, cardiac conduction blocks, fibrillation and arrhythmias, also sclerotic effects.

Orally it is toxic, but the LD₅₀ is around 2500 mg/kg. Intravenously this is reduced to just over 100 mg/kg but of more concern are its severe effects on cardiac muscles; high doses can cause cardiac arrest and rapid death.

Precautions

See previous section.

Suppliers/Manufacturers

Aldrich: http://www.sigmaaldrich.com Alfa: http://www.alfa.com/alf/index.htm VWR: http://www.vwr.com/index.htm or Fisher: https://www1.fishersci.com/index.jsp

de:Kaliumchlorid ja:塩化カリウム nl:Kaliumchloride pl:chlorek potasu

References

1. Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
2. N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, Pergamon Press, 1984.