Lead(II) sulfate
| Lead(II) sulfate | |
|---|---|
_sulfate.jpg) |
|
|
lead(II) sulfate |
|
|
Other names
|
|
| Identifiers | |
| CAS number | 7446-14-2  |
| PubChem | 24008 |
| ChemSpider | 19956579 |
| Jmol-3D images | Image 1 |
|
|
|
|
| Properties | |
| Molecular formula | PbSO4 |
| Molar mass | 303.26 g/mol |
| Appearance | white solid |
| Density | 6.29 g/cm3[1] |
| Melting point |
1087 °C, 1360 K, 1989 °F |
| Solubility in water | 0.0032 g/100 mL (15 °C) 0.00425 g/100 mL (25 °C) |
| Solubility | insoluble in alcohol |
| Refractive index (nD) | 1.877 |
| Structure | |
| Crystal structure | orthorhombic, barite |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−920 kJ·mol−1[2] |
| Standard molar entropy S |
149 J·mol−1·K−1[2] |
| Specific heat capacity, C | 103 J/degree mol |
| Hazards | |
| EU Index | 082-001-00-6 |
| EU classification | Repr. Cat. 1/3 Toxic (T) Harmful (Xn) Dangerous for the environment (N) |
| R-phrases | R61, R20/22, R33, R62, R50/53 |
| S-phrases | S53, S45, S60, S61 |
| NFPA 704 |
 0
3
0
|
| Flash point | Non-flammable |
| Threshold Limit Value | 0.15 mg/m3 |
| Related compounds | |
| Other anions | Lead(II) chloride, Lead(II) bromide, Lead(II) iodide, Lead(II) fluoride |
| Other cations | Tin(II) sulfate, Sodium sulfate, Copper(II) sulfate |
 (verify) (what is:  / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) |
|
| Infobox references | |
Lead(II) sulfate (British English sulphate) (PbSO4) is a white crystal or powder. It is also known as fast white, milk white, sulfuric acid lead salt or anglesite.
It is often seen in the plates/electrodes of car batteries, as it is formed when the battery is discharged (when the battery is recharged, then the lead sulfate is transformed back to metallic lead and sulfuric acid on the negative terminal or lead dioxide and sulfuric acid on the positive terminal). Lead sulfate is poorly soluble in water.
Manufacturing
Lead(II) sulfate is prepared by treating lead oxide, hydroxide or carbonate with warm sulfuric acid, or by treating a soluble lead salt with sulfuric acid.
Alternatively, it may be created by the interaction of solutions of lead nitrate and sodium sulfate.
Toxicology
Lead sulfate is toxic by inhalation, ingestion and skin contact. It is a cumulative poison, and repeated exposure may lead to anemia, kidney damage, eyesight damage or damage to the central nervous system (especially in children). Some lead salts may cause reproductive defects and cardiovascular disturbances. It is also corrosive - contact with the eyes can lead to severe irritation or burns. Typical threshold limit value (above which the substance is harmful) is 0.15 mg/m³.
Mineral
The naturally occurring mineral anglesite, PbSO4, occurs as an oxidation product of primary lead sulfide ore, galena.
Basic and hydrogen lead sulfates
A number of lead basic sulfates are known: PbSO4·PbO; PbSO4·2PbO; PbSO4·3PbO; PbSO4·4PbO. They are used in manufacturing of active paste for lead acid batteries. A related mineral is leadhillite, 2PbCO3·PbSO4·Pb(OH)2. a
At high concentration of sulfuric acid (>80%), hydrogen lead sulfate, Pb(HSO4)2, forms.[3]
References
- ^ "CRC Handbook of Chemistry and Physics", 83rd Edition, CRC Press, 2002.
- ^ a b Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 0-618-94690-X.
- ^ Министерство образования и науки РФ, Реферат "Свинец и его свойства", 2007, http://revolution.allbest.ru/chemistry/00011389_0.html
|
|||||
