Lead(II) sulfate

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.

Lead(II) sulfate
Names
IUPAC name
lead(II) sulfate
Other names
Anglesite, fast white, milk white, plumbous sulfate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.028.362
UNII
Properties
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
0.0032 g/100 mL (15 °C)
0.00443 g/100 mL (20 °C)[2]
2.13 x 10−8 (20 °C)
Solubility insoluble in alcohol

soluble in ammonium acetate (>6M)

soluble in ammonium tartrate in presence of ammonium chloride and ammonia

−69.7·10−6 cm3/mol
1.877
Structure
orthorhombic, barite
Thermochemistry
103 J/degree mol
149 J·mol−1·K−1[3]
−920 kJ·mol−1[3]
Hazards
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R-phrases (outdated) R61, R20/22, R33, R62, R50/53
S-phrases (outdated) S53, S45, S60, S61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 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasReactivity code 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
0
3
0
Flash point Non-flammable
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

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 made 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 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 tetrahydroxidoplumbate(II) [Pb(OH)4]2− complexes.

PbSO4(s) + H2SO4(l) ⇌ Pb(HSO4)2(aq)
PbSO4(s) + 4NaOH(aq) → Na2[Pb(OH)4](aq) + Na2SO4(aq)

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

PbSO4(s) → PbO(s) + SO3(g)

References
  1. "CRC Handbook of Chemistry and Physics", 83rd Edition, CRC Press, 2002.
  2. NIST-data review 1980
  3. Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A22. ISBN 978-0-618-94690-7.
  4. Министерство образования и науки РФ, Реферат "Свинец и его свойства", 2007, http://revolution.allbest.ru/chemistry/00011389_0.html Archived 2007-12-21 at the Wayback Machine
Compounds containing the sulfate group (SO2−
4)
H2SO4 He
Li2SO4 BeSO4 B2S2O9 esters
ROSO3−
(RO)2SO2		 (NH4)2SO4
[N2H5]HSO4
(NH3OH)2SO4
NOHSO4		 HOSO4 F Ne
Na2SO4
NaHSO4		 MgSO4 Al2(SO4)3
Al2SO4(OAc)4		 Si P SO42−
HSO3HSO4
(HSO4)2		 Cl Ar
K2SO4
KHSO4		 CaSO4 Sc2(SO4)3 TiOSO4 VSO4
V2(SO4)3
VOSO4		 CrSO4
Cr2(SO4)3		 MnSO4 FeSO4
Fe2(SO4)3		 CoSO4
Co2(SO4)3		 NiSO4
Ni2(SO4)3		 CuSO4
Cu2SO4
[Cu(NH3)4(H2O)]SO4		 ZnSO4 Ga2(SO4)3 Ge As Se Br Kr
RbHSO4
Rb2SO4		 SrSO4 Y2(SO4)3 Zr(SO4)2 Nb MoSO4
Mo2(SO4)3
Mo(SO4)2
Mo(SO4)2
Mo(SO4)3		 Tc Ru(SO4)2 RhSO4
Rh2(SO4)3		 PdSO4 Ag2SO4
AgSO4		 CdSO4 In2(SO4)3 SnSO4
Sn(SO4)2		 Sb2(SO4)3 Te I Xe
Cs2SO4
CsHSO4		 BaSO4   Hf Ta W Re OsSO4
Os2(SO4)3
Os(SO4)2		 IrSO4
Ir2(SO4)3		 PtSO4
Pt(SO4)2		 AuSO4
Au2(SO4)3		 Hg2SO4
HgSO4		 Tl2SO4
Tl2(SO4)3		 PbSO4
Pb(SO4)2		 Bi2(SO4)3 PoSO4
Po(SO4)2		 At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La2(SO4)3 Ce2(SO4)3
Ce(SO4)2		 Pr2(SO4)3 Nd2(SO4)3 Pm2(SO4)3 Sm2(SO4)3 Eu2(SO4)3 Gd2(SO4)3 Tb2(SO4)3 Dy2(SO4)3 Ho2(SO4)3 Er2(SO4)3 Tm2(SO4)3 Yb2(SO4)3 Lu2(SO4)3
Ac2(SO4)3 Th(SO4)2 Pa U2(SO4)3
U(SO4)2
UO2SO4		 Np(SO4)2 Pu(SO4)2 Am2(SO4)3 Cm2(SO4)3 Bk Cf Es Fm Md No Lr
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