He chloric acid Is an inorganic compound of the formula HCLO 3, Composed of an oxacid acid where the chlorine has oxidation state +5 with a structure analogous to Bromic acid or Iodic acid . AND S a strong acid capable of donating a hydrogen to an acceptor or Bronsted base.
The acid was first discovered in the seventeenth century, for Johann Rudolf Glauber Of Karlstadt am Main, Germany, in which it used sodium chloride and sulfuric acid For the preparation of sodium sulfate in the Mannheim process, releasing hydrogen chloride gas, harmful to humans.
The compound is obtained with barium chlorate (barite chlorate) with sulfuric acid to produce barium sulfate (Jacob Green, 1829) insoluble in water according to the following reaction:
Ba (ClO 3 ) 2 + H 2 SW 4 → 2HClO 3 + BaSO 4
Another method of obtaining is heating Hypochlorous acid To obtain chloric acid and hydrogen chloride according to the reaction:
3HClO → HClO 3 + 2HCl
Cloric acid (HClO3) is a powerful oxidant given that it is able to be reduced to oxidation states +3, +1 and -1. It is used for the manufacture of chlorate salts.
Decomposes in concentrations higher than 30%. It also decomposes on heating, for this reason it should be kept cold all the time and all glass jars used to handle must be pre-cooled.
Physical and chemical properties of chloric acid
Chloric acid exists only in solution. It is a colorless liquid with no characteristic aroma (National Center for Biotechnology Information, 2017) its appearance is shown in figure 2.
Figure 2: appearance of chloric acid.
The compound has a molecular weight of 84.459 g / mol and a density of 1 g / ml at about 25 ° C. It has a boiling point higher than 100 ° C (CHLORIC ACID, S.F.) and a water solubility of 40 g per 100 ml of this solvent at 25 ° C (Royal Society of Chemistry, 2015).
Chloric acid will accelerate the burning of combustible materials and can ignite most in contact. The compound is corrosive to metals and fabrics.
Self-reactive
- Concentrations of chloric acid above 40% are decomposed.
- The antimony sulfide and the concentrated solutions of chloric acid react with incandescence.
- Arsenic sulfide and concentrated solutions of chloric acid react with incandescence.
- Reacts vigorously even explodes with other metal sulfides, ie, copper sulphide.
- In contact with oxidizable materials, including ammonia, the reactions can be extremely violent.
- The filter paper is switched on after submerging it in hydrochloric acid.
- The explosions have been recorded by mixtures of chloric acid solution with metals such as: antimony, bismuth and iron. This is due to the formation of explosive compounds including hydrogen (CHLORIC ACID, 2016).
Reactivity and hazards
Chloric acid is an unstable compound. Being a strong acid, it is extremely dangerous in case of contact with the skin (it is corrosive and irritant), contact with the eyes (irritant) and in case of ingestion. Also very dangerous in case of inhalation.
Severe overexposure may result in lung damage, asphyxia, loss of consciousness or death. Prolonged exposure may cause skin burns and ulcerations.
Overexposure by inhalation may cause respiratory irritation. Inflammation of the eye is characterized by redness, watering and itching. Inflammation of the skin is characterized by itching, peeling, redness and occasionally, blistering.
The substance is toxic to the kidneys, lungs and mucous membranes. Repeated or prolonged exposure to the substance may cause damage to these organs.
In case of contact with the eyes, it is necessary to check if they are wearing contact lenses and to remove them immediately. Flush eyes with running water for at least 15 minutes, keeping eyelids open. Cold water can be used. Eye ointment should not be used.
If the chemical comes into contact with clothing, remove it as quickly as possible, protecting your own hands and body. Place the victim under a safety shower.
If the chemical accumulates on the victim's exposed skin, such as the hands, gently and thoroughly wash contaminated skin with running water and non-abrasive soap.
The acid can also be neutralized with dilute sodium hydroxide or with a weak base as sodium bicarbonate . If irritation persists, seek medical attention. Wash the contaminated clothing before using it again.
If contact with the skin is severe, it should be washed with a disinfectant soap and cover the skin contaminated with an anti-bacterial cream.
In case of inhalation, the victim should be allowed to stand in a well-ventilated area. If the inhalation is severe, the victim should be evacuated to a safe area as soon as possible.
Loosen tight clothing such as a shirt collar, belts, or tie. If it is difficult for the victim to breathe, oxygen should be administered. If the victim is not breathing, a mouth-to-mouth resuscitation is performed.
Always taking into account that it can be dangerous for the person providing help give mouth-to-mouth resuscitation when the inhaled material is toxic, infectious or corrosive.
If swallowed, do not induce vomiting. Loosen tight clothing such as shirt collars, belts or ties. If the victim is not breathing, perform mouth-to-mouth resuscitation. In all cases seek immediate medical attention.
Applications
Chloric acid is mainly used for the formation of chlorate salts such as sodium, calcium, magnesium, strontium, lead, copper and silver chlorate, as well as protochlorate and mercury perchlorate are prepared using chloric acid as a reagent.
Stable precursor of chlorine dioxide, is used in the electrochemical production of high purity ammonium perchlorate (Dotson, 1993).
The main production of chloric acid was initiated during the Industrial Revolution In Europe and was used to manufacture vinyl chloride for PVC pipes.
Another use for acid is numerous small scale applications, including household cleaning, production of gelatine and other food additives, descaling and processing of leather (chloric acid, S.F.).
References
- CHLORIC ACID . (2016). Recovered from cameochemicals: cameochemicals.noaa.gov.
- Chloric acid . (S.F.). Retrieved from weebly: http://chloricacid.weebly.com/
- CHLORIC ACID . (S.F.). Recovered from chemicalbook: chemicalbook.com.
- Dotson, R. (1993). A novel electrochemical process for the production of ammonium perchlorate. Journal of Applied Electrochemistry Volume 23, Issue 9, , 897-904. Link.springer.com.
- EMBL-EBI. (2014, July 28). Chloric acid . Retrieved from ebi.ac.uk: ebi.ac.uk.
- Jacob Green, E. T. (1829). A text book of chemical philosophy. Philadelphia: Russell & Martien.
- National Center for Biotechnology Information. . (2017, April 15). PubChem Compound Database; CID = 19654 . Recovered from pubchem:.pubchem.ncbi.nlm.nih.gov.
- Royal Society of Chemistry. (2015). CHLORIC ACID . Recovered from chemspider: chemspider.com.