Lead(II) sulfate

Lead(II) sulfate (PbSO₄) is an ionic compound made of lead(II) cations and sulfate anions. It is sparingly soluble in water and occurs as the mineral anglesite.

Lead(II) ion: The Pb²⁺ cation formed when a lead atom loses two electrons. Pb²⁺ supplies the positively charged ion in PbSO₄.
Precipitation reaction: A chemical reaction in solution that produces an insoluble or sparingly soluble solid. Mixing soluble sources of Pb²⁺ and SO₄²⁻ can precipitate PbSO₄.
Battery discharge: The conversion of stored chemical energy into electrical energy by an electrochemical cell. During discharge, both lead–acid battery electrodes form PbSO₄.
Lead(II) chloride: An ionic lead compound with formula PbCl₂ that is sparingly soluble in cold water. Its chloride anions give it different solubility and temperature behavior from PbSO₄.
Sulfate: The polyatomic anion SO₄²⁻, with sulfur bonded to four oxygen atoms. SO₄²⁻ supplies the negatively charged ion in PbSO₄.
Common-ion effect: The reduction in a salt’s solubility when a solution already contains one of its ions. Added sulfate or lead ions shift PbSO₄ dissolution toward the solid.
Battery charging: The use of external electrical energy to reverse a rechargeable battery’s discharge reactions. Charging converts electrode PbSO₄ back into lead and lead dioxide.
Lead(II) carbonate: A sparingly soluble lead compound with formula PbCO₃, occurring as the mineral cerussite. Carbonate forms a distinct lead precipitate and mineral rather than sulfate.
Ionic compound: A substance composed of oppositely charged ions held together by electrostatic attraction. PbSO₄ is an electrically neutral lattice of Pb²⁺ and SO₄²⁻ ions.
Dissolution: The process by which particles of a substance disperse into a solvent. Only a small fraction of PbSO₄ enters water as dissolved ions.

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