Potassium dichromate

Not to be confused with Potassium chromate.
Potassium dichromate
Names
IUPAC name
Potassium dichromate(VI)
Other names
potassium bichromate

bichromate of potash
dipotassium dichromate
dichromic acid, dipotassium salt
chromic acid, dipotassium salt

lopezite[1]
Identifiers
7778-50-9 YesY
ChEMBL ChEMBL1374101
ChemSpider 22910 YesY
EC Number 231-906-6
Jmol 3D image Interactive graph
PubChem 24502
RTECS number HX7680000
UN number 3288
Properties
K2Cr2O7
Molar mass 294.185 g/mol
Appearance red-orange crystalline solid
Odor odorless
Density 2.676 g/cm3, solid
Melting point 398 °C (748 °F; 671 K)
Boiling point 500 °C (932 °F; 773 K) decomposes
4.9 g/100 mL (0 °C)
102 g/100 mL (100 °C)
Solubility insoluble in alcohol
1.738
Structure
Triclinic (α-form, <241.6 °C)
Tetrahedral (for Cr)
Thermochemistry
291.2 JK−1mol−1
-2033 kJ/mol
Hazards
Safety data sheet ICSC 1371
Oxidant (O)
Carc. Cat. 2
Muta. Cat. 2
Repr. Cat. 2
Highly toxic (T+)
Harmful (Xn)
Corrosive (C)
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
NFPA 704
Flash point non-flammable
Lethal dose or concentration (LD, LC):
25 mg/kg (oral, rat)[2]
Related compounds
Other anions
Potassium chromate
Potassium molybdate
Potassium tungstate
Other cations
Ammonium dichromate
Sodium dichromate
Related compounds
Potassium permanganate
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
YesY verify (what is YesYN ?)
Infobox references

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.[3]

Chemistry

Production

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+

Reactions

Potassium dichromate is an oxidising 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.[4] 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

Uses

Potassium dichromate has few major applications, as the sodium salt is dominant industrially. The main use is as a precursor to potassium chrome alum, used in leather tanning.[3][5]

Cleaning

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.

Construction

It is used as an ingredient in cement in which it retards the setting of the mixture and improves its density and texture. This usage commonly causes contact dermatitis in construction workers.[6]

Photography

Potassium dichromate has uses in photography and in photographic screen printing, where it is used as an oxidizing agent together with a strong mineral acid.

In 1839, Mungo Ponton discovered that paper treated with a solution of potassium dichromate was visibly tanned by exposure to sunlight, the discoloration remaining after the potassium dichromate had been rinsed out. In 1852, Henry Fox Talbot discovered that exposure to ultraviolet light in the presence of potassium dichromate hardened organic colloids such as gelatin and gum arabic, making them less soluble.

These discoveries soon led to the carbon print, gum bichromate, and other photographic printing processes based on differential hardening. Typically, after exposure, the unhardened portion was rinsed away with warm water, leaving a thin relief that either contained a pigment included during manufacture or was subsequently stained with a dye. Some processes depended on the hardening only, in combination with the differential absorption of certain dyes by the hardened or unhardened areas. Because some of these processes allowed the use of highly stable dyes and pigments, such as carbon black, prints with an extremely high degree of archival permanence and resistance to fading from prolonged exposure to light could be produced.

Dichromated colloids were also used as photoresists in various industrial applications, most widely in the creation of metal printing plates for use in photomechanical printing processes.

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.

CrVI compounds have the property of tanning animal proteins when exposed to strong light. This quality is used in photographic screen-printing.

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.

Ethanol determination

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

Full reaction of converting ethanol to acetic acid:

3C2H5OH + 2K2Cr2O7 + 8H2SO4 → 3CH3COOH + 2Cr2(SO4)3 + 2K2SO4 + 11H2O

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.

Silver test

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.

Wood treatment

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.[7]

Natural occurrence

A ~10 mm crystal of potassium dichromate in the same form as the mineral lopezite

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.[8]

Safety

In 2005–06, potassium dichromate was the 11th-most-prevalent allergen in patch tests (4.8%).[9]

Potassium dichromate is one of the most common causes of chromium dermatitis;[10] 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. [11] 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.[12] Human exposure further encompasses impaired fertility, heritable genetic damage and harm to unborn children.

References

  1. "POTASSIUM DICHROMATE LISTING" (PDF). US EPA.
  2. http://chem.sis.nlm.nih.gov/chemidplus/rn/7778-50-9
  3. 1 2 Gerd Anger, Jost Halstenberg, Klaus Hochgeschwender, Christoph Scherhag, Ulrich Korallus, Herbert Knopf, Peter Schmidt, Manfred Ohlinger, "Chromium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, Wiley-VCH, Weinheim, 2005. doi:10.1002/14356007.a07_067
  4. L. T. Sandborn. "l-Menthone". Org. Synth.; Coll. Vol. 1, p. 340
  5. M. Saha, C. R. Srinivas, S. D. Shenoy, C. Balachandran (May 1993). "Footwear dermatitis". Contact Dermatitis 28 (5): 260–264. doi:10.1111/j.1600-0536.1993.tb03428.x. PMID 8365123.
  6. Pekka Roto, Hannele Sainio, Timo Reunala, Pekka Laippala (January 1996). "Addition of ferrous sulfate to cement and risk of chromium dermatitis among construction workers". Contact Dermatitis 34 (1): 43–50. doi:10.1111/j.1600-0536.1996.tb02111.x. PMID 8789225.
  7. Jewitt, Jeff (1997). Hand-Applied Finishes. Newtown, CT USA: The Taunton Press, Inc. ISBN 1-56158-154-2.
  8. Mindat
  9. Zug KA, Warshaw EM, Fowler JF Jr, Maibach HI, Belsito DL, Pratt MD, Sasseville D, Storrs FJ, Taylor JS, Mathias CG, Deleo VA, Rietschel RL, Marks J. Patch-test results of the North American Contact Dermatitis Group 2005–2006. Dermatitis. 2009 May–Jun;20(3):149-60.
  10. Farokh J. Master (2003). Diseases of Skin. New Delhi: B Jain Pub Pvt Ltd. p. 223. ISBN 81-7021-136-0.
  11. "Potassium dichromate MSDS". Sigma-Aldrich. Retrieved 2011-07-20.
  12. "Potassium dichromate MSDS". JT Baker.

External links

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