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) determines how soluble a compound is in water. The larger the Ksp, the more soluble the compound. In this case, we need to compare the solubility products for the compounds. 
- Ca(OH)2 has a relatively high Ksp as it dissociates readily. 
- AgBr has a lower Ksp compared to Ca(OH)2. 
- HgS has an even lower Ksp, meaning it is less soluble than AgBr. 
- PbS has the lowest Ksp among these compounds, making it the least soluble. 
Thus, the increasing order of solubility products is: \( {Ca(OH)}_2<{AgBr}<{HgS}<{PbS} \).