solubilityproducts

solubilityproducts - • Ksp = c x(2c)2 = 4c3 • 1.6 x...

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solubility product  - Ksp   equals product of ion concentrations raised to the power of their coefficients can be used to calculate solubility (g/L) Find the Ksp for a saturated solution of Mg(OH)2 if the pH is 10.17   assume that Mg(OH)2, a strong base, dissociates completely Mg(OH)2 >> Mg2+ + 2OH- pOH = 14 - pH = 14 - 10.17 = 3.83 [OH-] = 10-pOH = 10-3.83 = 1.48 x 10-4 [Mg2+] = [OH-] / 2 = 7.4 x 10-5 Ksp = [Mg2+] [OH-]2 = 1.62 x 10-12 Find the molar solubility of Mn(OH)2 if the Ksp is 1.6 x 10-13   Mn(OH)2 >> Mn2+ + 2OH- Ksp = [Mn2+] [OH-]2 let c = molar solubility, concentration of Mn
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Unformatted text preview: • Ksp = c x (2c)2 = 4c3 • 1.6 x 10-13 = 4c3 • c = 3.4 x 10-5 Find the molar solubility of Ba(IO3)2 in a solution of 0.010 M NaIO3 • Given: o Ksp = 6 x 10-10 • [IO3-] = [NaIO3] = 0.010 • Ksp = [Ba2+] [IO3-]2 • 6 x 10-10 = [Ba2+] (0.010)2 • [Ba2+] = molar solubility = 6 x 10-6 Find the molar solubility of Ba(IO3)2 in a solution of 0.01 M NaNO3 • Given: o Ksp = 6 x 10-10 • NaNO3 has no effect on the solubility of Ba(IO3)2 • Ksp = [Ba2+] [IO3-]2 • let c = molar solubility, concentration of Ba • Ksp = c x (2c)2 = 4c3 • 6 x 10-10 = 4c3 • c = 5.3 x 10-4...
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