Difference between revisions of "Chromic acid"
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==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Chromic acid is a powerful oxidizer. Solutions of chromic acid are used to oxidize primary alcohols to aldehydes and secondary alcohols to ketones. | + | Chromic acid is a powerful oxidizer. Solutions of chromic acid are used to oxidize primary alcohols to aldehydes and secondary alcohols to ketones. |
| + | |||
| + | Addition of a reducing agent, such as [[ascorbic acid]] will reduce it to Cr(III). | ||
===Physical=== | ===Physical=== | ||
Revision as of 20:31, 26 February 2017
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| Names | |
|---|---|
| IUPAC name
Chromic acid
| |
| Systematic IUPAC name
Dihydroxidodioxidochromium | |
| Other names
Chromic(VI) acid
Tetraoxochromic acid | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| H2CrO4 | |
| Molar mass | 118.01 g/mol |
| Appearance | Dark red/reddish-brown viscous liquid |
| Density | 1.201 g/cm3 |
| Melting point | 197 °C (387 °F; 470 K) |
| Boiling point | 250 °C (482 °F; 523 K) |
| 169 g/100 mL | |
| Solubility | Soluble in acetone |
| Acidity (pKa) | -0.8 to 1.6 |
| Hazards | |
| Safety data sheet | ScienceLab |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
51.9 mg/kg (H2CrO4·2Na, rat, oral) |
| Related compounds | |
| Related compounds
|
Chromium trioxide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Chromic acid is the name given to the compound resulted from the addition of concentrated sulfuric acid to a dichromate salt, such as potassium dichromate. The resulting product however is impure, and also tends to contain other compounds such as chromium trioxide or dichromic acid. The generally recognized formula for chromic acid is H2CrO4.
Contents
Properties
Chemical
Chromic acid is a powerful oxidizer. Solutions of chromic acid are used to oxidize primary alcohols to aldehydes and secondary alcohols to ketones.
Addition of a reducing agent, such as ascorbic acid will reduce it to Cr(III).
Physical
Chromic acid is a dark red to red-brownish viscous liquid, that decomposes on boiling.
Availability
Chromic acid is generally not sold, and has to be prepared in situ.
Preparation
Chromic acid can be prepared by adding concentrated sulfuric acid to a cooled aqueous solution of a dichromate salt:
- H2SO4 + K2Cr2O7 → H2CrO4 + K2SO4
Very pure chromic acid can be made by adding chromium trioxide to pure water.
- CrO3 + H2O ⇋ H2CrO4
Derivations
Chromosulfuric acid
Made by adding an excess of sulfuric acid to a supersaturated solution of potassium dichromate. One standard recipe involves adding 93 ml of concentrated (95-98%) sulfuric acid to a cooled 7 ml solution of supersaturated K2Cr2O7. If the solution is not cooled, chromium trioxide will precipitate. The resulting liquid has a red-brownish color, it is viscous and has a weak unpleasant rotten eggs smell (though it's best not to inhale chromic solution vapors).
It is also known as sulfochromic mixture.
Chromonitric acid
This special mixture is made by adding concentrated nitric acid to a dichromate salt. It is/was widely used in the countries of the Soviet bloc, instead of the more common piranha solution. May release nitrogen oxides fumes during preparation.
Chromonitric acid is known to ignite organic materials and pose an explosion hazard.[1]
Diluted mixtures of chromic and nitric acids can be used to test for silver.
Dichromic acid
Can be obtained by adding excess chromium trioxide to chromic acid. It's generally encountered as a side product in the preparation of chromic acid solutions, rather than a desired compound.
Projects
- Clean glassware
- Jones oxidation
- Make chromyl chloride
- Identify silver (chromonitric)
- Destroy small samples of hazardous organic compounds/alkaloids
Handling
Safety
Chromic acid and its derivatives are extremely corrosive to flesh. Contact with bare skin causes an intense heating sensation and, if not washed immediately, the acid will cause severe burns. Hexavalent chromium ions are carcinogenic and proper protection must be worn when handling the product. However, when the chromic acid is neutralized with a base, it immediately converts to the less harmful Cr(III), though traces of Cr(VI) may still be in the final product.
Storage
Chrmic acid should be stored in glass bottles, away from any organic material.
Disposal
Chromic acid can be neutralized with a reducing agent. Sodium/potassium metabisulfite, sodium thiosulfate or sodium sulfite are excellent neutralizing agents.
Sodium bicarbonate will also neutralize the acid to Cr(III), however there might still be traces of Cr(IV) in the product, so this might not be a suitable disposal agent.
References
- ↑ http://booksonchemistry.com/index.php?id1=3&category=laborotor-tech&author=zaharov-ln&book=1991&page=26
Relevant Sciencemadness threads
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- Chemical compounds
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