Question

Arrange the following in increasing order of solubility product: 
\[ {Ca(OH)}_2, {AgBr}, {PbS}, {HgS} \]

• A. HgS<AgBr<PbS<Ca(OH)2
• B. PbS<HgS<Ca(OH)2<AgBr
• C. Ca(OH)2<AgBr<HgS<PbS
• D. HgS<PbS<AgBr<Ca(OH)2

Hint:

For solubility products, compounds with lower Ksp values are less soluble. Compare Ksp values to determine the order of solubility.

Answer 1

The Correct Option is C

The solubility product (Ksp) quantifies a compound's solubility in water; a higher Ksp indicates greater solubility. To determine the order of solubility, we compare the Ksp values of the given compounds:
- Ca(OH)2 exhibits a high Ksp due to facile dissociation.
- AgBr possesses a lower Ksp than Ca(OH)2.
- HgS demonstrates a Ksp lower than AgBr, signifying reduced solubility.
- PbS has the lowest Ksp among these compounds, indicating it is the least soluble.
Therefore, the compounds ordered by increasing solubility product are: \( {Ca(OH)}_2<{AgBr}<{HgS}<{PbS} \).