No, PbSO4 (lead(II) sulfate) is generally considered insoluble in water. 1 It has a very low solubility in water, resulting in the formation of a white precipitate when lead(II) ions and sulfate ions come together in an aqueous solution.
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Key Takeaways: Is PbSO4 Soluble in Water?
- PbSO4 is generally considered insoluble in water, with very low solubility, resulting in a white precipitate.
- The insolubility of PbSO4 is due to its strong ionic bonding, high lattice energy, inadequate hydration energy, and the size and charge of its ions.
- PbSO4 can dissolve in concentrated acids, such as nitric acid, hydrochloric acid, and sulfuric acid, forming soluble or acidic salts containing lead ions.
Why is PbSO4 insoluble in water?
PbSO4 is primarily considered insoluble in water. The reasons for its insolubility can be explained as follows:
- Ionic Bonding: PbSO4 is made up of lead ions (Pb)2+ and sulfate ions (SO4)2-. These ions are held together by ionic bonds, which are formed by the attraction between positively and negatively charged ions. The strength of these ionic bonds in PbSO4 is significant, leading to a stable crystal lattice structure.
- High Lattice Energy: PbSO4 has a high lattice energy, which is the energy required to break the ionic bonds in the crystal lattice. The strong ionic bonding in PbSO4 results in a high lattice energy, making it difficult for the crystal to dissociate in water. 2
- Hydration Energy: When an ionic compound dissolves in water, the water molecules surround and stabilize the individual ions through hydration. However, in the case of PbSO4, the hydration energy is not sufficient to overcome the strong lattice energy of the crystal. As a result, the crystal remains intact, and PbSO4 does not dissolve appreciably in water.
Overall, the combination of strong ionic bonding, high lattice energy, inadequate hydration energy, and the size and charge of the ions in PbSO4 contribute to its insolubility in water.
Can PbSO4 dissolve in other solvents?
PbSO4 can dissolve in concentrated acids such as nitric acid (HNO3), hydrochloric acid (HCl), and sulfuric acid (H2SO4), forming acidic salts containing lead ions. 3 4 These strong acids can react with PbSO4 and result in the formation of soluble or acidic salts.
Lead(II) sulfate has a strong ionic lattice structure, with ionic bonding between lead and sulfate ions. This lattice is difficult to break, making PbSO4 insoluble in most solvents. Its solubility in water is very low, and it is generally regarded as insoluble.
However, when PbSO4 is exposed to concentrated acids, the strong acid-base interactions can lead to the dissolution of PbSO4 and the formation of soluble or acidic salts.
This dissolution occurs due to the formation of new compounds, such as lead nitrate (Pb(NO3)2), lead chloride (PbCl2), or lead hydrogen sulfate (Pb(HSO4)2). It’s important to note that the solubility of PbSO4 in these acids is significantly higher compared to its solubility in water or other solvents.
Further reading
Why is MgSO4 Soluble in Water?
Why is KCl (Potassium Chloride) Soluble in Water?
Is Benzene Soluble in Water?
Why is CuSO4 (Copper Sulfate) Soluble in Water?
Why is NaOH (Sodium Hydroxide) Soluble in Water?
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References
- Lead(II) sulfate – Wikipedia. (2022, March 4). Lead(II) Sulfate – Wikipedia. https://en.wikipedia.org/wiki/Lead(II)_sulfate
- 7.3: Ionic Bond Formation and Strength. (2018, November 26). Chemistry LibreTexts. https://chem.libretexts.org/Courses/Oregon_Institute_of_Technology/OIT%3A_CHE_202_-_General_Chemistry_II/Unit_7%3A_Intermolecular_and_Intramolecular_Forces_in_Action/7.3%3A_Ionic_Bond_Formation_and_Strength
- P. (n.d.). Lead sulfate. Lead Sulfate | PbSO4 | CID 24008 – PubChem. https://pubchem.ncbi.nlm.nih.gov/compound/24008
- Crockford, H. D., & Addleston, J. A. (1936, March 1). The Solubility of Lead Sulfate in Aqueous Solutions of Sulfuric Acid at High Concentrations. The Journal of Physical Chemistry, 40(3), 303–305. https://doi.org/10.1021/j150372a002
