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

Solution & Explanation

### Related Formula The solubility product constant (K_sp) reflects the equilibrium position of a sparingly soluble salt in water. ### Core Logic Based on standard literature K_sp values at 298text K: - HgS: approx 4 times 10^-53 (extremely insoluble, Group IIB cation analysis) - PbS: approx 8 times 10^-28 (highly insoluble, Group IIA cation analysis) - AgBr: approx 5 times 10^-13 (sparingly soluble halide salt) - Ca(OH)_2: approx 5.5 times 10^-6 (moderately soluble base) ### Step 1: Arrangement Comparing these K_sp orders: 4 times 10^-53 < 8 times 10^-28 < 5 times 10^-13 < 5.5 times 10^-6 Hence, the correct increasing sequence is: HgS < PbS < AgBr < Ca(OH)_2. ### Pattern Recognition Sulphides of heavy transition metals like Hg^2+ and Pb^2+ have exceptionally small K_sp values compared to halides or hydroxides. Among sulphides, HgS is famously known to have one of the lowest solubility products found in inorganic qualitative analysis. ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 11 Chemistry: Equilibrium

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Equilibrium

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Q62 jee_main_2024_31_jan_morning Equilibrium Constant
For the given reaction, choose the correct expression of K_C from the following :- Fe_(aq)^3+ + SCN_(aq)^- rightleftharpoons (FeSCN)_(aq)^2+
  • A. K_C = frac[FeSCN^2+][Fe^3+][SCN^-]
  • B. K_C = frac[Fe^3+][SCN^-][FeSCN^2+]
  • C. K_C = frac[FeSCN^2+][Fe^3+]^2[SCN^-]^2
  • D. K_C = frac[FeSCN^2+]^2[Fe^3+][SCN^-]

Solution

### Related Formula K_C = frac[textProducts][textReactants] ### Core Logic K_C = fractextProducts ion conc.textReactants ion conc. K_C = frac[FeSCN^2+][Fe^3+][SCN^-] ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 11 Chemistry: Equilibrium

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