|Jmol-3D images||Image 1|
|Molar mass||294.185 g/mol|
|Appearance||red-orange crystalline solid|
|Density||2.676 g/cm3, solid|
|Melting point||398 °C (748 °F; 671 K)|
|Boiling point||500 °C (932 °F; 773 K) decomposes|
|Solubility in water||4.9 g/100 mL (0 °C)
102 g/100 mL (100 °C)
|Solubility||insoluble in alcohol|
Refractive index (nD)
|Crystal structure||Triclinic (α-form, <241.6 °C)|
|Tetrahedral (for Cr)|
|291.2 J K−1 mol−1|
Std enthalpy of
|EU classification||Oxidant (O)
Carc. Cat. 2
Muta. Cat. 2
Repr. Cat. 2
Highly toxic (T+)
Dangerous for the environment (N)
|R-phrases||R45, R46, R60, R61, R8, R21, R25, R26, R34, R42/43, R48/23, R50/53|
|S-phrases||S53, S45, S60, S61|
|LD50||25 mg/kg (oral, rat)|
|Other anions||Potassium chromate
|Other cations||Ammonium dichromate
|Related compounds||Potassium permanganate|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Potassium dichromate, K2Cr2O7, is a common inorganic chemical reagent, most commonly used as an oxidizing agent in various laboratory and industrial applications. As with all hexavalent chromium compounds, it is acutely and chronically harmful to health. It is a crystalline ionic solid with a very bright, red-orange color. The salt is popular in the laboratory because it is not deliquescent, in contrast to the more industrially relevant salt sodium dichromate.
Potassium dichromate is usually prepared by the reaction of potassium chloride on sodium dichromate. Alternatively, it can be obtained from potassium chromate by roasting chrome ore with potassium hydroxide. It is soluble in water and in the dissolution process it ionizes:
- K2Cr2O7 → 2 K+ + Cr2O72−
- Cr2O72− + H2O ⇌ 2 CrO42− + 2 H+
Potassium dichromate is an oxidizing agent in organic chemistry, and is milder than potassium permanganate. It is used to oxidize alcohols. It converts primary alcohols into aldehydes and, under more forcing conditions, into carboxylic acids. In contrast, potassium permanganate tends to give carboxylic acids as the sole products. Secondary alcohols are converted into ketones. For example, menthone may be prepared by oxidation of menthol with acidified dichromate. Tertiary alcohols cannot be oxidized.
In an aqueous solution the color change exhibited can be used to test for distinguishing aldehydes from ketones. Aldehydes reduce dichromate from the +6 to the +3 oxidation state, changing color from orange to green. This color change arises because the aldehyde can be oxidized to the corresponding carboxylic acid. A ketone will show no such change because it cannot be oxidized further, and so the solution will remain orange.
When heated strongly, it decomposes with the evolution of oxygen.
- 4K2Cr2O7 → 4K2CrO4 + 2Cr2O3 + 3O2
When an alkali is added to an orange red solution containing dichromate ions, a yellow solution is obtained due to the formation of chromate ions. For example, potassium chromate is produced industrially using potash:
- K2Cr2O7 + K2CO3 → 2 K2CrO4 + CO2
The reaction is reversible.
Treatment with cold sulphuric acid gives red crystals of chromic anhydride (CrO3):
- K2Cr2O7 + 2H2SO4 → 2CrO3 + 2 KHSO4 + H2O
On heating with concentrated acid, oxygen is evolved:
- 2 K2Cr2O7 + 8H2SO4 → 2 K2SO4 + 2 Cr2(SO4)3 + 8 H2O + 3O2
Like other chromium(VI) compounds (chromium trioxide, sodium dichromate), potassium dichromate has been used to prepare "chromic acid" for cleaning glassware and etching materials. Because of safety concerns associated with hexavalent chromium, this practice has been largely discontinued.
Gum bichromate printing was one of the very first stable photographic printing processes, dating back to about 1850. A solution of gum arabic and potassium dichromate, once applied to paper and dried, will harden when exposed to ultraviolet light.
Chromium intensification or Photochromos uses potassium dichromate together with equal parts of concentrated hydrochloric acid diluted down to approximately 10% v/v to treat weak and thin negatives of black and white photograph roll. This solution reconverts the elemental silver particles in the film to silver chloride. After thorough washing and exposure to actinic light, the film can be redeveloped to its end-point yielding a stronger negative which is able to produce a more satisfactory print.
A potassium dichromate solution in sulfuric acid can be used to produce a reversal negative (i.e., a positive transparency from a negative film). This is effected by developing a black and white film but allowing the development to proceed more or less to the end point. The development is then stopped by copious washing and the film then treated in the acid dichromate solution. This converts the silver metal to silver sulfate, a compound that is insensitive to light. After thorough washing and exposure to actinic light, the film is developed again allowing the previously unexposed silver halide to be reduced to silver metal.
The results obtained can be unpredictable, but sometimes excellent results are obtained producing images that would otherwise be unobtainable. This process can be coupled with solarisation so that the end product resembles a negative and is suitable for printing in the normal way.
In screen-printing a fine screen of bolting silk or similar material is stretched taut onto a frame similar to the way canvas is prepared before painting. A colloid sensitized with a dichromate is applied evenly to the taut screen. Once the dichromate mixture is dry, a full-size photographic negative is attached securely onto the surface of the screen, and the whole assembly exposed to strong light – typically about half an hour in bright sunlight – hardening the exposed colloid. When the negative is removed, the unexposed mixture on the screen can be washed off with warm water, leaving the hardened mixture intact, acting as a precise mask of the desired pattern, which can then be printed with the usual screen-printing process.
As an analytical reagent
Because it is non-hygroscopic, potassium dichromate is a common reagent in classical "wet tests" in analytical chemistry.
The concentration of ethanol in a sample can be determined by back titration with acidified potassium dichromate. Reacting the sample with an excess of potassium dichromate, all ethanol is oxidized to acetic acid:
- CH3CH2OH + 2[O] → CH3COOH + H2O
The excess dichromate is determined by titration against sodium thiosulfate. Subtracting the amount of excess dichromate from the initial amount, gives the amount of ethanol present. Accuracy can be improved by calibrating the dichromate solution against a blank.
One major application for this reaction is in old police breathalyzer tests. When alcohol vapor makes contact with the orange dichromate-coated crystals, the color changes from orange to green. The degree of the color change is directly related to the level of alcohol in the suspect's breath.
When dissolved in an approximately 35% nitric acid solution it is called Schwerter's solution and is used to test for the presence of various metals, notably for determination of silver purity. Pure silver will turn the solution bright red, sterling silver will turn it dark red, low grade coin silver (0.800 fine) will turn brown (largely due to the presence of copper which turns the solution brown) and even green for 0.500 silver. Brass turns dark brown, copper turns brown, lead and tin both turn yellow while gold and palladium do not change.
Sulfur dioxide test
Potassium dichromate paper can be used to test for sulfur dioxide, as it turns distinctively from orange to green. This is typical of all redox reactions where hexavalent chromium is reduced to trivalent chromium. Therefore, it is not a conclusive test for sulfur dioxide. The final product formed is Cr2(SO4)3.
Potassium dichromate is used to stain certain types of wood by darkening the tannins in the wood. It produces deep, rich browns that cannot be achieved with modern color dyes. It is a particularly effective treatment on mahogany.
Potassium dichromate occurs naturally as the rare mineral lopezite. It has only been reported as vug fillings in the nitrate deposits of the Atacama desert of Chile and in the Bushveld igneous complex of South Africa.
Potassium dichromate is one of the most common causes of chromium dermatitis; chromium is highly likely to induce sensitization leading to dermatitis, especially of the hand and fore-arms, which is chronic and difficult to treat. Toxicological studies have further illustrated its highly toxic nature. With rabbits and rodents, concentrations as low as 14 mg/kg have shown a 50% fatality rate amongst test groups.  Aquatic organisms are especially vulnerable if exposed, and hence responsible disposal according local environmental regulations is advised.
As with other CrVI compounds, potassium dichromate is carcinogenic and should be handled with gloves and appropriate health and safety protection. The compound is also corrosive and exposure may produce severe eye damage or blindness. Human exposure further encompasses impaired fertility, heritable genetic damage and harm to unborn children.
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- "Potassium dichromate MSDS". Sigma-Aldrich. Retrieved 2011-07-20.
- "Potassium dichromate MSDS". JT Baker.
- Potassium Dichromate at The Periodic Table of Videos (University of Nottingham)
- International Chemical Safety Card 1371
- National Pollutant Inventory – Chromium VI and compounds fact sheet
- NIOSH Pocket Guide to Chemical Hazards
- IARC Monograph "Chromium and Chromium compounds"
- Gold refining article listing color change when testing metals with Schwerter's Solution