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Potassium chromate is the inorganic compound with the formula K 2 CrO 4. This yellow solid is the potassium salt of the chromate anion. It is a common laboratory chemical, whereas sodium chromate is important industrially.
2 CrO 2− 4 + 2 H + ⇌ Cr 2 O 2− 7 + H 2 O The predominance diagram shows that the position of the equilibrium depends on both pH and the analytical concentration of chromium. [ notes 1 ] The chromate ion is the predominant species in alkaline solutions, but dichromate can become the predominant ion in acidic solutions.
Chromium(VI) compounds in solution can be detected by adding an acidic hydrogen peroxide solution. The unstable dark blue chromium(VI) peroxide (CrO 5) is formed, which can be stabilized as an ether adduct CrO 5 ·OR 2. [6] Chromic acid has the hypothetical formula H 2 CrO 4. It is a vaguely described chemical, despite many well-defined ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Chrome alum. Chromium alum is produced from chromate salts or from ferrochromium alloys. Concentrated aqueous solutions of potassium dichromate can be reduced, usually with sulfur dioxide but also with alcohols or formaldehyde, in the presence of sulfuric acid at temperatures <40 °C.
Hydrogen peroxide is a chemical compound with the formula H 2 O 2.In its pure form, it is a very pale blue [5] liquid that is slightly more viscous than water.It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution (3%–6% by weight) in water for consumer use and in higher concentrations for industrial use.
Chromium(VI) oxide peroxide is the name given to a collection of chromium coordination complexes. They have the formula CrO(O 2) 2 L where L is a ligand. These species are dark blue and often labile. They all feature oxo ligand and two peroxo ligands, with the remaining coordination sites occupied by water, hydroxide, ether, or other Lewis ...
Many industrial peroxides are produced using hydrogen peroxide. Reactions with aldehydes and ketones yield a series of compounds depending on conditions. Specific reactions include addition of hydrogen peroxide across the C=O double bond: R 2 C=O + H 2 O 2 → R 2 C(OH)OOH. In some cases, these hydroperoxides convert to give cyclic diperoxides: