Bismuth(III) nitrate
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| Other names
Bismuth trinitrate, Bismuth(III) nitrate pentahydrate
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3D model (JSmol)
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PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| Bi(NO3)3·5H2O | |
| Molar mass | 485.07 g/mol (pentahydrate) |
| Appearance | colorless, white |
| Density | 2.90 g/cm3 (pentahydrate)[1] |
| Decomposes to form bismuth oxynitrate[2] | |
| Solubility | Slightly soluble in acid[2] |
| −91.0·10−6 cm3/mol | |
| Hazards | |
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| Warning | |
| H272, H315, H319, H335, H411 | |
| P210, P220, P221, P261, P264, P271, P273, P280, P302+P352, P304+P340, P305+P351+P338, P312, P321, P332+P313, P337+P313, P362, P370+P378, P391, P403+P233, P405, P501 | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Bismuth(III) nitrate is a salt composed of bismuth in its cationic +3 oxidation state and nitrate anions. The most common solid form is the pentahydrate.[3] It is used in the synthesis of other bismuth compounds.[4] It is available commercially. It is the only nitrate salt formed by a group 15 element, indicative of bismuth's metallic nature.[5]
Preparation and reactions
[edit | edit source]Bismuth nitrate can be prepared by the reaction of bismuth metal and concentrated nitric acid.[6]
- Bi + 4HNO3 → Bi(NO3)3 + 2H2O + NO
It dissolves in nitric acid but is readily hydrolysed to form a range of oxynitrates when the pH increases above 0.[7]
It is also soluble in acetone, acetic acid and glycerol but practically insoluble in ethanol and ethyl acetate.[8]
Some uses in organic synthesis have been reported for example the nitration of aromatic compounds and selective oxidation of sulfides to sulfoxides.[8]
Bismuth nitrate forms insoluble complexes with pyrogallol and cupferron and these have been the basis of gravimetric methods of determining bismuth content.[9]
On heating bismuth nitrate can decompose forming nitrogen dioxide, NO2.[10]
Structure
[edit | edit source]The crystal form is triclinic, and contains 10 coordinate Bi3+, (three bidentate nitrate ions and four water molecules).[1]
References
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- ^ A.I. Vogel,(1951), Quantitative Inorganic analysis, (2d edition), Longmans Green and Co
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