Chromic acid
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Template:Chembox image cellTemplate:Chembox AllOtherNamesTemplate:Chembox headerbarTemplate:Chembox IndexlistTemplate:Chembox JmolTemplate:Chembox ChEMBLTemplate:Chembox ECHATemplate:Chembox E numberTemplate:Chembox IUPHAR ligandTemplate:Chembox UNIITemplate:Chembox CompToxTemplate:Chembox headerbarTemplate:Chembox SolubilityInWaterTemplate:Chembox ConjugateAcidBaseTemplate:Chembox headerbarTemplate:Chembox OHS (set)Template:Chembox GHS (set)Template:Chembox Lethal amounts (set)Template:Chembox setHeaderTemplate:Chembox setDatarowTemplate:Chembox setDatarowTemplate:Chembox setDatarowTemplate:Chembox Datapage checkTemplate:Chembox Footer| Template:Longitem | Template:Unbulleted list |
| ChEBI | Template:Unbulleted list |
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| EC Number | Template:Unbulleted list |
| Template:Longitem | 25982 |
| KEGG | Template:Unbulleted list |
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| RTECS number | Template:Unbulleted list |
| UN number | 1755 1463 |
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| Template:Longitem | Template:Chem2 (chromic acid) Template:Chem2 (dichromic acid) |
| Molar mass | 118.008 g/mol (chromic acid) 218.001 g/mol (dichromic acid) |
| Appearance | Dark purplish-red sand-like crystalline solid or powderScript error: No such module "Unsubst". |
| Odor | Odorless |
| Density | 1.201 g/cm3Script error: No such module "Unsubst". |
| Melting point | Template:Chembox CalcTemperatures |
| Boiling point | Template:Chembox CalcTemperatures |
| Acidity (pKa) | −0.8 to 1.6 (chromic acid) |
| NFPA 704 (fire diamond) | Template:NFPA 704 diamond |
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Chromic acid is a chemical compound with the chemical formula Template:Chem2. More generally, it is the name for a solution formed by the addition of sulfuric acid to aqueous solutions of dichromate. It consists at least in part of chromium trioxide.[3]
The term "chromic acid" is usually used for a mixture made by adding concentrated sulfuric acid to a dichromate, which may contain a variety of compounds, including solid chromium trioxide. This kind of chromic acid may be used as a cleaning mixture for glass. Chromic acid may also refer to the molecular species, Template:Chem2 of which the trioxide is the anhydride. Chromic acid features chromium in an oxidation state of +6 (and a valence of VI or 6). It is a strong and corrosive oxidizing agent and a moderate carcinogen.
Molecular chromic acid
Molecular chromic acid, Template:Chem2, in principle, resembles sulfuric acid, Template:Chem2. It would ionize accordingly:
The pKa for the equilibrium is not well characterized. Reported values vary between about −0.8 to 1.6.[4] The structure of the mono anion has been determined by X-ray crystallography. In this tetrahedral oxyanion, three Cr-O bond lengths are 156 pm and the Cr-OH bond is 201 pm[5]
Template:Chem2 condenses to form dichromate:
- Template:Chem2, logKD = 2.05.
Furthermore, the dichromate can be protonated:
- Template:Chem2, pKa = 1.8[6]
Loss of the second proton occurs in the pH range 4–8, making the ion Template:Chem2 a weak acid.Script error: No such module "Unsubst".
Molecular chromic acid could in principle be made by adding chromium trioxide to water (cf. manufacture of sulfuric acid).
In practice, the reverse reaction occurs: molecular chromic acid dehydrates. Some insights can be gleaned from observations on the reaction of dichromate solutions with sulfuric acid. The first colour change from orange to red signals the conversion of dichromate to chromic acid. Under these conditions deep red crystals of chromium trioxide precipitate from the mixture, without further colour change.
Chromium trioxide is the anhydride of molecular chromic acid. It is a Lewis acid and can react with a Lewis base, such as pyridine in a non-aqueous medium such as dichloromethane (Collins reagent).
Higher chromic acids with the formula Template:Chem2 are probable components of concentrated solutions of chromic acid.
Uses
Chromic acid is an intermediate in chromium plating, and is also used in ceramic glazes, and colored glass. Because a solution of chromic acid in sulfuric acid (also known as a sulfochromic mixture or chromosulfuric acid) is a powerful oxidizing agent, it can be used to clean laboratory glassware, particularly of otherwise insoluble organic residues. This application has declined due to environmental concerns.[8] Furthermore, the acid leaves trace amounts of paramagnetic chromic ions (Template:Chem2) that can interfere with certain applications, such as NMR spectroscopy. This is especially the case for NMR tubes.[9] Piranha solution can be used for the same task, without leaving metallic residues behind.
Chromic acid was widely used in the musical instrument repair industry, due to its ability to "brighten" raw brass. A chromic acid dip leaves behind a bright yellow patina on the brass. Due to growing health and environmental concerns, many have discontinued use of this chemical in their repair shops.
It was used in hair dye in the 1940s, under the name Melereon.[10]
It is used as a bleach in processing black and white photographic reversal film.[11]
Reactions
Chromic acid is capable of oxidizing many kinds of organic compounds and many variations on this reagent have been developed:
- Chromic acid in aqueous sulfuric acid and acetone is known as the Jones reagent, which will oxidize primary and secondary alcohols to carboxylic acids and ketones respectively, while rarely affecting unsaturated bonds.[12]
- Pyridinium chlorochromate is generated from chromium trioxide and pyridinium chloride. This reagent converts primary alcohols to the corresponding aldehydes (R–CHO).[12]
- Collins reagent is an adduct of chromium trioxide and pyridine used for diverse oxidations.
- Chromyl chloride, Template:Chem2 is a well-defined molecular compound that is generated from chromic acid.
Illustrative transformations
- Oxidation of methylbenzenes to benzoic acids.[13]
- Oxidative scission of indene to homophthalic acid.[14]
- Oxidation of secondary alcohol to ketone (cyclooctanone)[15] and Template:Chem name.[16]
Use in qualitative organic analysis
In organic chemistry, dilute solutions of chromic acid can be used to oxidize primary or secondary alcohols to the corresponding aldehydes and ketones. Similarly, it can also be used to oxidize an aldehyde to its corresponding carboxylic acid. Tertiary alcohols and ketones are unaffected. However, in acidic conditions, some tertiary alcohols may isomerize to an oxidizable alcohol, though such an isomerization is usually not of concern. Because the oxidation is signaled by a color change from orange to brownish green (indicating chromium being reduced from oxidation state +6 to +3), chromic acid is commonly used as a lab reagent in high school or undergraduate college chemistry as a qualitative analytical test for the presence of primary or secondary alcohols, or aldehydes.[12]
Alternative reagents
In oxidations of alcohols or aldehydes into carboxylic acids, chromic acid is one of several reagents, including several that are catalytic. For example, nickel(II) salts catalyze oxidations by bleach (hypochlorite).[17] Aldehydes are relatively easily oxidized to carboxylic acids, and mild oxidizing agents are sufficient. Silver(I) compounds have been used for this purpose. Each oxidant offers advantages and disadvantages. Instead of using chemical oxidants, electrochemical oxidation is often possible.
Safety
Hexavalent chromium compounds (including chromium trioxide, chromic acids, chromates, chlorochromates) are toxic and carcinogenic. Chromium trioxide and chromic acids are strong oxidizers and may react violently if mixed with easily oxidizable organic substances.
Chromic acid burns are treated with a dilute sodium thiosulfate solution.[18]
Notes
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- ↑ IUPAC SC-Database A comprehensive database of published data on equilibrium constants of metal complexes and ligands
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- ↑ a b c Freeman, F. "Chromic Acid" Encyclopedia of Reagents for Organic Synthesis (2001) John Wiley & Sons, Script error: No such module "CS1 identifiers".
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References
- Alcohols from Carbonyl Compounds: Oxidation-Reduction and Organometallic CompoundsScript error: No such module "Unsubst". (PDF)
External links
- International Chemical Safety Card 1194
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- IARC Monograph "Chromium and Chromium compounds"
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