Potassium chromate

Two crystalline forms are known, both being very similar to the corresponding potassium sulfate. Orthorhombic β-K₂CrO₄ is the common form, but it converts to an α-form above 66 °C.^[1] These structures are complex, although the chromate ion adopts the typical tetrahedral geometry.^[2]

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  Structure of β-K₂CrO₄.
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  Coordination sphere of one of two types of K⁺ site.
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  The environment about the tetrahedral CrO₄²⁻ center in β-K₂CrO₄.

It is prepared by treating potassium dichromate with potassium hydroxide:

${\displaystyle {\ce {K2Cr2O7(aq) + 2KOH -> 2K2CrO4 + H2O}}}$ 

Or, the fusion of potassium hydroxide and chromium trioxide:

${\displaystyle {\ce {2KOH + CrO3 -> K2CrO4 + H2O}}}$ 

In solution, the behavior of potassium and sodium dichromates are very similar. When treated with lead(II) nitrate, it gives an orange-yellow precipitate, lead(II) chromate.

Unlike the less expensive sodium salt, potassium salt is mainly used for laboratory work in situations where an anhydrous salt is required.^[1] It is as an oxidizing agent in organic synthesis. It is used in qualitative inorganic analysis, e.g. as a colorimetric test for silver ion. It is also used as an indicator in precipitation titrations with silver nitrate and sodium chloride (they can be used as standard as well as titrant for each other) as potassium chromate turns red in the presence of excess of silver ions.

Tarapacaite is the natural, mineral form of potassium chromate. It occurs very rarely and until now is known from only few localities on Atacama Desert.^{[citation needed]}

As with other Cr(VI) compounds, potassium chromate is carcinogenic.^[3] The compound is also corrosive and exposure may produce severe eye damage or blindness.^[4] Human exposure further encompasses impaired fertility, heritable genetic damage and harm to unborn children.