Final answer:
The solubility of a compound in water can be determined by comparing their respective solubility product constants (Ksp). The larger the Ksp value, the greater the solubility of the compound in water. None of the given compounds has a larger solubility in water based on their respective solubility product constants.
Step-by-step explanation:
The solubility of a compound in water can be determined by comparing their respective solubility product constants (Ksp). Ksp is an equilibrium constant that represents the dissolution of an ionic compound in water. The larger the Ksp value, the greater the solubility of the compound in water.
Based on the given compounds:
- LaF3: It is insoluble in water and has a low solubility product constant.
- CaCO3: It has a low solubility in water and a relatively low solubility product constant.
- Ag2SO4: It has a moderate solubility in water and a moderate solubility product constant.
- Pb(OH)2: It has a high solubility in water and a high solubility product constant.
Therefore, (d) None of the above has a larger solubility in water based on their respective solubility product constants.