Lead(II) sulfate, commonly represented as PbSO4, is not soluble in water. This characteristic can be understood by examining the nature of its ionic bonds and the overall solubility rules for sulfates.
Most sulfate salts are soluble in water, but there are key exceptions. Lead(II) sulfate falls into this category due to the strong ionic bonds formed between lead ions (Pb2+) and sulfate ions (SO42-). The greater the ionic bond strength, the less likely the compound will dissolve in a polar solvent like water.
When lead(II) sulfate is placed in water, the water molecules, which are polar, do not effectively break apart the strong bonds between Pb2+ and SO42- ions. This inability to overcome the ionic attractions means that PbSO4 remains largely in a solid state despite being surrounded by water.
Furthermore, the low solubility of PbSO4 can lead to its precipitation in situations where lead and sulfate ions are present in a solution, which is significant in various chemical and environmental contexts. Thus, when considering whether PbSO4 dissolves in water, the answer is a definitive no, primarily due to the strong ionic interactions holding the compound together.