Search results
Results From The WOW.Com Content Network
Lead(II) sulfate (PbSO 4) 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 ...
Lead(II) oxide is also soluble in alkali hydroxide solutions to form the corresponding plumbite salt. [2] PbO + 2 OH − + H 2 O → Pb(OH) 2− 4. Chlorination of plumbite solutions causes the formation of lead's +4 oxidation state. Pb(OH) 2− 4 + Cl 2 → PbO 2 + 2 Cl − + 2 H 2 O. Lead dioxide is representative of the +4 oxidation state ...
Lead(II) hydroxide: Pb(OH) 2: 1.615×10 −4: Lead(II) iodate: Pb(IO 3) 2: ... Lead(II) sulfate: PbSO 4: 0.00443: Lead(II) sulfide: PbS: 6.767×10 −13: Lead(II ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
In aqueous solution, lead(II) hydroxide is a somewhat weak base, forming lead(II) ion, Pb 2+, under weakly acidic conditions. This cation hydrolyzes and, under progressively increasing alkaline conditions, it becomes somewhat weak acid, and it forms Pb(OH) +, Pb(OH) 2 (aqueous), Pb(OH) − 3, and other species, including several polynuclear species, e.g., Pb 4 (OH) 4+ 4, Pb 3 (OH) 2+ 4, Pb 6 O ...
Lead(II) azide – Pb(N 3) 2; Lead(II) bromide – PbBr 2; Lead(II) carbonate – Pb(CO 3) Lead(II) chloride – PbCl 2; Lead(II) fluoride – PbF 2; Lead(II) hydroxide – Pb(OH) 2; Lead(II) iodide – PbI 2; Lead(II) nitrate – Pb(NO 3) 2; Lead(II) oxide – PbO; Lead(II) phosphate – Pb 3 (PO 4) 2; Lead(II) sulfate – Pb(SO 4) Lead(II ...
lead(II) cyanide: 592–05–2 PbCO 3: lead(II) carbonate: 598–63–0 Pb(C 2 H 3 O 2) 2: lead(II) acetate: 301–04–2 Pb(C 2 H 3 O 2) 2: lead(III) acetate: 546–67–8 PbC 2 O 4: lead(II) oxalate: 814–93–7 Pb(C 3 H 5 O 2) 2: lead(II) lactate: 18917–82–3 Pb(C 4 H 7 O 2) 2: lead(II) butanoate: 819–73–8 Pb(C 18 H 33 O 2) 2: lead ...
Litharge is the most commonly used inorganic compound of lead. [68] There is no lead(II) hydroxide; increasing the pH of solutions of lead(II) salts leads to hydrolysis and condensation. [69] Lead commonly reacts with heavier chalcogens. Lead sulfide is a semiconductor, a photoconductor, and an extremely sensitive infrared radiation detector.