Potassium chromate

Potassium chromate
IUPAC name	Potassium chromate
Other names	Chromic acid, (H2CrO4), dipotassium salt
Identifiers
CAS number	7789-00-6 Y
PubChem	24597
EC number	232-140-5
RTECS number	GB2940000
Properties
Molecular formula	CrK2O4
Molar mass	194.19 g mol−1
Appearance	Yellow odorless powder
Odor	odorless
Density	2.7320 g/cm3
Melting point	968 °C, 1241 K, 1774 °F
Boiling point	1000 °C, 1273 K, 1832 °F
Solubility in water	63 g/100 mL (20 °C)
Solubility	insoluble in alcohol
Hazards
MSDS	Chemical Safety Data
EU Index	024-006-00-8
EU classification	Carc. Cat. 2 Muta. Cat. 2 Toxic (T) Irritant (Xi) Dangerous for the environment (N)
R-phrases	R49, R46, R36/37/38, R43, R50/53
S-phrases	S53, S45, S60, S61
NFPA 704	0 3 1 OX
Related compounds
Other anions	Potassium dichromate Potassium molybdate Potassium tungstate
Other cations	Sodium chromate Calcium chromate Barium chromate
Y (what is this?)  (verify) Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Potassium chromate (K₂CrO₄) is a yellow chemical indicator used for identifying concentrations of chloride ions in a salt solution with silver nitrate (AgNO₃). It is a class two carcinogen and can cause cancer on inhalation.^[1]

General information

Physical properties

Potassium Chromate is a lemon yellow compound that is in the form of a crystalline solid, and it is very stable.^{[citation needed]}

Reactions

When reacted with Lead(II) Nitrate, it creates an orange-yellow precipitate, Lead(II) Chromate, Silver Nitrate, and Potassium Nitrate. All ions hydrolyze in solution.

Occurrence

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]}

Dangers/Hazards

Potassium Chromate is very toxic and may be fatal if swallowed. It may also act as a carcinogen, and can create reproductive defects if inhaled or swallowed. It also is a strong oxidizing agent if in the presence of H⁺ to produce the dichromate ion. It may react rapidly, or violently. It is also possible that it may react explosively with other reducing agents and flammable objects.

References

1. ^ Potassium chromate information URL last accessed 15 March 2007

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