Potassium DiChromate 250g 99%

Potassium DiChromate 250g 99%

Potassium DiChromate 250g 99%

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.

Chemistry

Production

Potassium dichromate is usually prepared by the reaction of potassium chloride on sodium dichromate. Alternatively, it can be also obtained from potassium chromate by roasting chromite ore with potassium hydroxide. It is soluble in water and in the dissolution process it ionizes:

K₂Cr₂O₇ → 2 K⁺ + Cr₂O²⁻₇Cr₂O²⁻₇ + H₂O ⇌ 2 CrO²⁻₄ + 2 H⁺

Reaction

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. 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.

4 K₂Cr₂O₇ → 4 K₂CrO₄ + 2 Cr₂O₃ + 3 O₂

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 (CrO2−4). For example, potassium chromate is produced industrially using potash:

K₂Cr₂O₇ + K₂CO₃ → 2 K₂CrO₄ + CO₂

The reaction is reversible.

Treatment with cold sulfuric acid gives red crystals of chromic anhydride (chromium trioxide, CrO₃):

K₂Cr₂O₇ + 2 H₂SO₄ → 2 CrO₃ + 2 KHSO₄ + H₂O

On heating with concentrated acid, oxygen is evolved:

2 K₂Cr₂O₇ + 8 H₂SO₄ → 2 K₂SO₄ + 2 Cr₂(SO₄)₃ + 8 H₂O + 3 O₂

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.

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.

Natural occurrence

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.

Safety

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

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 to the local environmental regulations is advised.

As with other Cr(VI) compounds, potassium dichromate is carcinogenic. 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.