Question:
Arrange the following in increasing order of solubility product:
\[
{Ca(OH)}_2, {AgBr}, {PbS}, {HgS}
\]
Arrange the following in increasing order of solubility product:
\[
{Ca(OH)}_2, {AgBr}, {PbS}, {HgS}
\]
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For solubility products, compounds with lower Ksp values are less soluble. Compare Ksp values to determine the order of solubility.
Updated On: Mar 17, 2025
- HgS<AgBr<PbS<Ca(OH)2
- PbS<HgS<Ca(OH)2<AgBr
- Ca(OH)2<AgBr<HgS<PbS
- HgS<PbS<AgBr<Ca(OH)2
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The Correct Option is C
Solution and Explanation
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.
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