Solubility product
- Find out the solubility of Ni(OH)_2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)_2 is 2×10^-15. Answer: 1. 2×10⁻¹³ M In 0.1 M NaOH the common ion OH^- is already present, so the OH^- from Ni(OH)₂ can be ignored. mathrmNi(OH)₂ ⇌ Ni²⁺ + 2... 1
- pH of a saturated solution of Ca(OH)_2 is 9. The solubility product (K_sp) of Ca(OH)_2 is : Answer: 1. 0.5×10⁻¹⁵ Use pH to get [OH^-] , then write K_sp . pH = 9 so pOH = 5 and [OH^-] = 10⁻⁵ M. mathrmCa(OH)₂ ⇌ Ca²⁺ + 2OH^- , so [math... 1
- The solubility of BaSO_4 in water is 2.42×10^-3 gL^-1 at 298 K. The value of its solubility product (K_sp) will be(Given molar mass of BaSO_4 = 233 g mol^-1) Answer: 1. 1.08×10⁻¹⁰ mol ² L ⁻² Convert solubility to mol/L, then use K_sp=s² for a 1:1 salt. s=dfrac2.42×10⁻³233=1.04×10⁻⁵\ mathrmmol L⁻¹... 1
- Concentration of the Ag^+ ions in a saturated solution of Ag_2C_2O_4 is 2.2 × 10^-4 mol L^-1. Solubility product of Ag_2C_2O_4 is : Answer: 3. 5.3 × 10⁻¹² Key idea: Ag₂C₂O₄ ⇌ 2Ag^+ + C₂O₄²⁻ , K_sp=[Ag^+]²[C₂O₄²⁻] . [C₂O₄²⁻]=1/2[Ag^+]=1.1×10⁻⁴ M. K_sp=(2.2×10⁻⁴)²×1.1×10⁻⁴=... 1
- The solubility of AgCl (s) with solubility product 1.6×10^-10 in 0.1 M NaCl solution would be Answer: 1. 1.6×10⁻⁹ M Key idea: the common ion Cl^- from NaCl suppresses the solubility of AgCl. Let solubility be s . [Ag^+]=s , [Cl^-]≈ 0.... 1
- MY and NY_3, two nearly insoluble salts, have the same K_sp values of 6.2×10^-13 at room temperature. Which statement would be true in regard to MY and NY_3 ? Answer: 2. The molar solubility of MY in water is less than that of NY₃ . Key idea: compare solubilities from the K_sp expression for each s... 1