Lead(II) sulfate

Lead(II) sulfate

Names
IUPAC name lead(II) sulfate
Other names Anglesite, fast white, milk white
Identifiers
CAS Number	7446-14-2 Y
3D model (JSmol)	Interactive image
ChemSpider	19956579 Y
ECHA InfoCard	100.028.362
PubChem CID	24008
InChI InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2 Y Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L Y InChI=1S/H2O4S.Pb.4H/c1-5(2,3)4;;;;;/h(H2,1,2,3,4);;;;;/q;+2;;;;/p-2 Key: PIJPYDMVFNTHIP-QKXYEYSFAV Key: PIJPYDMVFNTHIP-UHFFFAOYSA-L
SMILES [O-]S(=O)(=O)[O-].[PbH4+2]
Properties
Chemical formula	PbSO4
Molar mass	303.26 g/mol
Appearance	white solid
Density	6.29 g/cm3[1]
Melting point	1,087 °C (1,989 °F; 1,360 K) decomposes
Solubility in water	0.0032 g/100 mL (15 °C) 0.00443 g/100 mL (20 °C)[2]
Solubility product (Ksp)	2.13 x 10−8 (20 °C)
Solubility	insoluble in alcohol
Magnetic susceptibility (χ)	−69.7·10−6 cm3/mol
Refractive index (nD)	1.877
Structure
Crystal structure	orthorhombic, barite
Thermochemistry
Specific heat capacity (C)	103 J/degree mol
Std molar entropy (So298)	149 J·mol−1·K−1[3]
Std enthalpy of formation (ΔfHo298)	−920 kJ·mol−1[3]
Hazards
EU classification (DSD) (outdated)	Repr. Cat. 1/3 Toxic (T) Harmful (Xn) Dangerous for the environment (N)
R-phrases (outdated)	R61, R20/22, R33, R62, R50/53
S-phrases (outdated)	S53, S45, S60, S61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
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
N verify (what is YN ?)
Infobox references

Lead(II) sulfate (PbSO₄) is a white solid, which appears white in microcrystalline form. 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 can be produced 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). 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.

At high concentration of sulfuric acid (>80%), lead hydrogensulfate, Pb(HSO₄)₂, forms.^[4]

Chemical properties

Lead(II) sulfate can be dissolved in concentrated HNO₃, HCl, H₂SO₄ producing acidic salts or complex compounds, and in concentrated alkali giving soluble hexahydroxidoplumbate(II) [Pb(OH)₆]²⁻ complexes.

PbSO₄(s) + H₂SO₄(conc.) <=> Pb(HSO₄)₂(aq)

PbSO₄(s) + 4NaOH(aq) → Na₂[Pb(OH)₆](aq) + Na₂SO₄(aq)

Lead(II) sulfate decomposes when heated above 1000 °C:

PbSO₄(s) → PbO(s) + SO₃(g)

External links

Wikimedia Commons has media related to Lead(II) sulfate.

• Case Studies in Environmental Medicine (CSEM): Lead Toxicity
• ToxFAQs: Lead
• National Pollutant Inventory - Lead and Lead Compounds Fact Sheet

References