Sulfuric acid’s effects are due to its strong acidity and dehydrating properties. It corrodes metals and chars organic materials like wood and paper. It can cause burns and permanent scarring on skin. Dilution with water is necessary, and protective gear should be worn. Inhaling sulfuric acid mist can damage the respiratory system and pose a cancer risk. Reactions with other materials can produce dangerous products.
Most of sulfuric acid’s effects come from its strong acidity and its great affinity for water. Corrosion of metals by sulfuric acid is caused by its acidity. The effects of sulfuric acid on organic materials, including human tissue, are largely the result of its dehydrating properties. Materials such as wood, paper and cotton are rapidly charred in contact with acid.
The effects of sulfuric acid on metals are typical of a strong acid: it will react with those metals that are more reactive than hydrogen to form a metal sulfate salt and release hydrogen gas. It will react this way with many common metals, including iron, zinc, and aluminum. The reaction is more vigorous with dilute acid than with concentrated acid. This limits the materials that can be used to store the acid, although in concentrated form it can be stored in stainless steel tanks. The release of hydrogen gas presents a potential explosion hazard in the event of a spill or leak if the acid contacts metals.
Sulfuric acid is a very powerful dehydrating agent and a large amount of heat is released when the concentrated acid comes into contact with water. If water is added to an excess of acid, the heat produced immediately boils the water, which can cause the acid to be sprayed over a large area. For this reason concentrated sulfuric acid must always be diluted by adding it — slowly — to the water; the process should never be reversed.
The dehydrating effects of sulfuric acid explain its reactions with many common organic materials. It will remove hydrogen and oxygen from molecules containing these elements in the 2:1 ratio found in the water (H2O) molecule – for example carbohydrates – which include sugars, starch and cellulose. The sulfuric acid will react with the carbohydrates to remove the hydrogen and oxygen, leaving the carbon. A well-known laboratory demonstration illustrates this; concentrated sulfuric acid is added to sucrose table sugar in a glass and quickly converts it into a lump of charcoal, with a fair amount of heat produced. This is why sulfuric acid chars wood and paper, substances which consist mainly of carbohydrates.
The effects of sulfuric acid on the skin are well documented and are still due to the dehydrating properties of the acid rather than its acidity. Skin contact with the concentrated acid causes pain and tissue swelling within seconds. If the contact is prolonged enough, deep burns can occur and there may be some charring, resulting in brown discoloration. Because of the swelling caused, sulfuric acid burns often result in permanent scarring.
When using sulfuric acid, protective gloves and suitable safety goggles should always be worn; a visor and protective apron are also recommended. Small spills on unprotected skin can be treated by prompt washing with plenty of water. Larger spills pose a risk of acid splashing if water is applied immediately – it’s best to quickly remove as much acid as possible before washing.
Sulfuric acid is not volatile at room temperature and therefore does not normally represent an inhalation hazard; however, if this acid or its industrial precursor, sulfur dioxide, comes into contact with water, the violence of the reaction can produce a fine mist of sulfuric acid droplets. This can damage the eyes, respiratory tract and lungs if inhaled. Chronic exposure to sulfuric acid mist, for example in a sulfuric acid plant, can have long-term health effects and can pose a cancer risk to workers.
Reactions of sulfuric acid with other materials can give rise to dangerous products. For example, it will release toxic and corrosive vapors when in contact with halides, such as chlorides, fluorides and bromides. Contact with chlorates and permanganates produces strong oxidizing compounds which pose a risk of fire or explosion.
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