|Jmol-3D images||Image 1|
|Molar mass||241.21 g/mol|
|Appearance||white amorphous powder|
|Density||7.41 g/cm3 |
|Melting point||135 °C (275 °F; 408 K) (decomposes)|
|Solubility in water||1.55 g/100 mL (20 °C)|
|Solubility product, Ksp||1.42 x 10−20|
|Solubility||soluble in dilute acid and alkalis;
insoluble in acetone and acetic acid
|EU classification||Toxic (T)|
|S-phrases||(S1/2) S20/21 S29/56 S45|
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Lead(II) hydroxide, Pb(OH)2, is a hydroxide of lead, with lead in oxidation state +2. Although it appears a fundamentally simple compound, it is doubtful if lead hydroxide is stable as a solid phase. Lead basic carbonate (PbCO3·2Pb(OH)2) or lead(II) oxide (PbO) is encountered in practice where lead hydroxide is expected. This has been a subject of considerable confusion in the past.
When an alkali hydroxide is added to a solution of a lead(II) salt, then a hydrated lead oxide PbO·xH2O (with x < 1) is obtained. Careful hydrolysis of lead(II) acetate solution yields a crystalline product with a formula 6PbO·2H2O = Pb6O4(OH)4.
In solution, lead(II) hydroxide is a somewhat weak base, forming lead(II) ion, Pb2+, under weakly acidic conditions. This cation hydrolyzes and, under progressively increasing alkaline conditions, forms Pb(OH)+, Pb(OH)2(aqueous), Pb(OH)3−, and other species, including several polynuclear species, e.g., Pb4(OH)44+, Pb3(OH)42+, Pb6O(OH)64+.
- Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- G. Todd and E. Parry (1964). "Character of Lead Hydroxide and Basic Lead Carbonate". Nature 202 (4930): 386–387. doi:10.1038/202386a0.
- Von Egon Wiberg, Nils Wiberg, Arnold Frederick Holleman, "Inorganic Chemistry", Academic Press, 2001 (Google books).
- Case Studies in Environmental Medicine - Lead Toxicity
- ToxFAQs: Lead
- National Pollutant Inventory - Lead and Lead Compounds Fact Sheet