Iodic acid: Difference between revisions
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{{ | {{DISPLAYTITLE:Iodic acid}} | ||
[[File:Iodic_acid.svg|thumb|right|150px|Structural formula of iodic acid]] | |||
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'''Iodic acid''' is a chemical compound with the formula ''' | '''Iodic acid''' is a chemical compound with the formula '''HIO_'''. It is a white crystalline solid and is one of the most important [[oxides of iodine]]. Iodic acid is a strong [[acid]] and is used in various chemical reactions and industrial applications. | ||
== Chemical Properties == | ==Chemical Properties== | ||
Iodic acid is a strong acid | Iodic acid is a strong acid, comparable in strength to [[sulfuric acid]]. It is highly soluble in water, forming a colorless solution. The acid dissociates in water to form [[hydronium ions]] and iodate ions: | ||
: HIO_ + H_O _ H_O_ + IO__ | |||
Iodic acid is a powerful oxidizing agent and can oxidize [[sulfur dioxide]] to [[sulfuric acid]] and [[hydrogen sulfide]] to [[sulfur]]. | |||
Iodic acid is | |||
== | ==Preparation== | ||
Iodic acid | Iodic acid can be prepared by oxidizing [[iodine]] with strong oxidizing agents such as [[nitric acid]] or [[chlorine]] in the presence of water: | ||
== Related | : I_ + 5 HNO_ _ 2 HIO_ + 5 NO_ + H_O | ||
Alternatively, it can be produced by the reaction of [[iodine pentoxide]] with water: | |||
: I_O_ + H_O _ 2 HIO_ | |||
==Uses== | |||
Iodic acid is used in analytical chemistry as a reagent for the determination of [[arsenic]] and [[antimony]]. It is also used in the synthesis of [[iodates]], which are salts of iodic acid. These iodates are used in the food industry as a source of iodine in [[iodized salt]]. | |||
==Safety== | |||
Iodic acid is a strong oxidizer and should be handled with care. It can cause burns upon contact with skin and is harmful if ingested. Proper safety precautions, including the use of [[personal protective equipment]], should be taken when handling iodic acid. | |||
==Related pages== | |||
* [[Iodine]] | * [[Iodine]] | ||
* [[Iodine pentoxide]] | * [[Iodine pentoxide]] | ||
* [[Iodate]] | * [[Iodate]] | ||
* [[Oxidizing agent]] | |||
* [[Oxidizing | |||
[[Category:Acids]] | [[Category:Acids]] | ||
[[Category:Iodine compounds]] | |||
[[Category:Oxidizing agents]] | [[Category:Oxidizing agents]] | ||
Latest revision as of 04:03, 13 February 2025
Iodic acid is a chemical compound with the formula HIO_. It is a white crystalline solid and is one of the most important oxides of iodine. Iodic acid is a strong acid and is used in various chemical reactions and industrial applications.
Chemical Properties[edit]
Iodic acid is a strong acid, comparable in strength to sulfuric acid. It is highly soluble in water, forming a colorless solution. The acid dissociates in water to form hydronium ions and iodate ions:
- HIO_ + H_O _ H_O_ + IO__
Iodic acid is a powerful oxidizing agent and can oxidize sulfur dioxide to sulfuric acid and hydrogen sulfide to sulfur.
Preparation[edit]
Iodic acid can be prepared by oxidizing iodine with strong oxidizing agents such as nitric acid or chlorine in the presence of water:
- I_ + 5 HNO_ _ 2 HIO_ + 5 NO_ + H_O
Alternatively, it can be produced by the reaction of iodine pentoxide with water:
- I_O_ + H_O _ 2 HIO_
Uses[edit]
Iodic acid is used in analytical chemistry as a reagent for the determination of arsenic and antimony. It is also used in the synthesis of iodates, which are salts of iodic acid. These iodates are used in the food industry as a source of iodine in iodized salt.
Safety[edit]
Iodic acid is a strong oxidizer and should be handled with care. It can cause burns upon contact with skin and is harmful if ingested. Proper safety precautions, including the use of personal protective equipment, should be taken when handling iodic acid.
