Is Aluminium Chloride (AlCl3) Hazardous?

Anhydrous aluminium chloride or AlCl3 is a neutral and white or yellow coloured crystalline substance. It interacts vigorously when it comes in contact with fluids like water to release hydrogen chloride or HCL gas. At 178 degrees Celsius, AlCl3 effortlessly sublimes to produce hydrogen chloride gas. Thus, solid and gaseous by-products are highly damaging to the eyes and mucous membranes. Although AlCl3 is not flammable, typical ABC or BC extinguishers should not be used.

This paper will cover the fundamental question, ‘Is Aluminium Chloride Hazardous?’ Along with that, it will also cover aluminium chloride’s definition, structure, and its hazardous examples and the basic idea of the hardness of aluminium chloride. 

What is aluminium chloride?

Aluminium chloride is a Lewis acid that is soluble in alcohol. Aluminium chloride in diglyme with sodium borohydride in a molar ratio produces a combination that has strong reducing capabilities. It facilitates the ‘Friedel-Crafts acylation’ reaction and or aromatic halogenation process.

Hydrogen’s vapour-phase co-reductions of other metal halides result in finely separated intermetallics with desirable thermoelectric, magnetic, and oxidation-resistance properties for use as structural materials or compounds. Aluminium nitride can be manufactured from the elements with the addition of AlCl3 to aid in crystallisation. Aluminium chloride (AlCl3) compounds, often referred to as aluminium trichloride compounds, have the formula AlCl3(H2O) n. They are made up of aluminium and chloride molecules in a 1:3 ratio, or one version also contains six hydration fluids.

Commercially, anhydrous material is significant. It does have a low melting point and a high boiling point. It is primarily manufactured and utilised in the production of ‘aluminium metal,’ although, it is also utilised extensively in other sectors of the chemical industry. The chemical is frequently referred to as a Lewis acid. It is an example of an ‘inorganic chemical’ that, at low temperatures, reversibly converts from polymers to monomers.

Usage of aluminium chloride

Hans Oersted created metallic aluminium in 1825 by heating aluminium chloride and elemental potassium. When aluminium sulphate and lime are combined in water, colloidal aluminium hydroxide is formed, which can precipitate and remove waterborne organic debris. This water clarity process is commonly utilised. Aluminium-containing additives can also be found in a variety of food products. They are employed as emulsifying agents in the processing of processed cheese, baking powder, crispy texture agents in pickles, and various food colourings. Cosmetics also contain aluminium-containing chemicals. Significant levels of metal can be found in commercial infant formula mixes.

The juices produced by cooking acidic fruits in aluminium cookware contain high quantities of soluble Al. The aluminium content of urban water sources varies, although quantities as high as ‘0.4–1 mg/L’ have occasionally been found in drinking water. Although the health effects of these metal levels on humans are unknown, the “Joint Food and Agriculture Organisation” or “World Health Organisation Expert Committee on Food Additives in 2007” suggested a weekly Al intake of less than 1 mg/kg body weight. For a 140-pound adult, this equates to 63 milligrams per week. Some industrial pastry products include up to 28 mg of aluminium sulphate and sodium aluminium phosphate in typical muffins or other baked products by using baking powder.

How to handle aluminium chloride hazards

Because anhydrous AlCl3 reacts violently with bases, appropriate precautions must be taken. If inhaled or coming in contact with it, it can irritate the skin, eyes, and the respiratory system.

Some basic precautions when working with AlCl3 include: 

• Wearing waterproof gloves, protective goggles, and a fire-retardant workshop coat. 
• Controlling the sources of ignition and avoiding the creation of dust. 
• Maintaining supplies of dry sand in the working area and making a class D chemical or fire extinguisher readily available. 
• When working with high amounts of AlCl3, work in a dry environment, such as a fume hood or glove box. Avoid coming into contact with fluids like water or being in humid settings. 
• AlCl3 is not compatible with many compounds, including powerful oxidants and caustics, sodium oxide, alcohols, hydrated reagents, nitromethane, ethylene oxide, and many other materials. AlCl3 corrodes with the majority of transition metals.
• Do not heat AlCl3 unless the resulting HCl vapours are adequately contained. When AlCl3 comes into contact with fluids like water or heat, it undergoes an exothermic reaction that produces hydrogen chloride gas.
• When AlCl3 is applied to the skin, it might irritate it depending on the chemical form or species of aluminium. According to an animal study, 10% aluminium chloride and nitrate caused epidermal alterations and damage; however, aluminium chlorohydrate, as used in antiperspirants, sulphates, hydroxide suspensions, or basic acetate suspension, do not cause any damage or irritation to the skin. 
• It should be kept in sealed containers in a cold, dry location away from combustible items. If a storage container becomes polluted with water, it may become compressed. Wastes should be kept in sealed containers and disposed of as hazardous trash.

Conclusion

In several practices, aluminium chloride has taken the position of Monsel solution. It is most frequently used following shave or blow biopsies. Formulations with concentrations ranging from 20% to 40% are made in alcohol, water, ether, or glycerol or as a pencil applicator. Its mode of action is hydrolysis with hydrochloric acid, which causes vasoconstriction, tissue clotting, or stimulation of the tissue factor found in the section. Though AlCl3 is hazardous enough in several cases, it has many practical applications as well.