Ksp for Cr(OH)_3 is 1.6times10^-30. What is the molar solubility of this salt in water ?

Solution & Explanation

### Related Formula K_sp = x^x y^y s^x+y ### Core Logic The dissolution equilibrium for chromium hydroxide is written as: Cr(OH)_3(s) rightleftharpoons Cr^3+(aq) + 3OH^-(aq) If the molar solubility is denoted by s: [Cr^3+] = s quad textand quad [OH^-] = 3s Substituting values into the expressions: K_sp = (s) cdot (3s)^3 = 27s^4 Given K_sp = 1.6 times 10^-30: 27s^4 = 1.6 times 10^-30 s = left( frac1.6 times 10^-3027 right)^1/4 ### Pattern Recognition For a binary-quaternary salt of type AB_3, the relationship simplifies strictly to K_sp = 27s^4. ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 11 Chemistry: Equilibrium

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Equilibrium

More Equilibrium Previous-Year Questions — Page 6

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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