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Pb 2 (OH) 2 (NO 3) 2 is the predominant species formed at low pH. At higher pH Pb 6 (OH) 5 (NO 3) is formed. [17] The cation [Pb 6 O(OH) 6] 4+ is unusual in having an oxide ion inside a cluster of 3 face-sharing PbO 4 tetrahedra. [18] There is no evidence for the formation of the hydroxide, Pb(OH) 2, in aqueous solution below pH 12.
Lead(II) azide Pb(N 3) 2 is an inorganic compound. More so than other azides, it is explosive. It is used in detonators to initiate secondary explosives. [5]
When mixed, as the lead from one solution and the iodide from the other combine to form lead(II) iodide (PbI 2), which is insoluble at low temperature and has a bright golden-yellow color. Although this is a reaction solely of the dissociated ions in solution, it is sometimes referred to as a double displacement reaction : [ 1 ]
It dissolves in nitric acid with the evolution of nitric oxide gas to form dissolved Pb(NO 3) 2. [8] It is a well-soluble solid in water; it is thus a key to receive the precipitates of halide, sulfate, chromate, carbonate, and basic carbonate Pb 3 (OH) 2 (CO 3) 2 salts of lead. [3]
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.
2 is commonly synthesized via a precipitation reaction between potassium iodide KI and lead(II) nitrate Pb (NO 3) 2 in water solution: Pb(NO 3) 2 + 2 KI → PbI 2 + 2 KNO 3. While the potassium nitrate KNO 3 is soluble, the lead iodide PbI 2 is nearly insoluble at room temperature, and thus precipitates out. [17]
2 Pb(NO 3) 2 → 2 PbO + 4 NO 2 + O 2 PbCO 3 → PbO + CO 2. PbO is produced on a large scale as an intermediate product in refining raw lead ores into metallic lead. The usual lead ore is galena (lead(II) sulfide). At a temperature of around 1,000 °C (1,800 °F) the sulfide is converted to the oxide: [5] 2 PbS + 3 O 2 → 2 PbO + 2 SO 2
Aqueous KSCN reacts almost quantitatively with Pb(NO 3) 2 to give Pb(SCN) 2, which has been used to convert acyl chlorides to isothiocyanates. [2] KSCN converts ethylene carbonate to ethylene sulfide. [3] For this purpose, the KSCN is first melted under vacuum to remove water.