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Solubility Equilibria (McGuire)

Last updated

Oct 26, 2020
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- Solubility and Ionic Strength (Scott)
- Solubility Equilibria (Scott)

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Analytical Sciences Digital Library

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1.) Calculate the Ksp for each of the salts whose solubility is listed below. Show units!

CaSO₄ = 5.0 x 10^-3 mol/L

MgF₂ = 2.7 x 10^-3 mol/L

AgC₂H₃O₂ (silver acetate) = 1.02 g/100 mL

SrF₂ = 12.2 mg/100 mL

2.) Calculate the solubility in moles/L of each of these salts in pure water and the concentration of the cations in ppm in each of the saturated solutions.

salt	Ksp	Solubility (M)	Conc. cation (ppm)
AgCN	2.0 x 10^-12
BaSO₄	1.5 x 10^-9
FeS	3.7 x 10^-19
Mg(OH)₂	9.0 x 10^-12
Ag₂S	1.6 x 10^-49
CaF₂	4.9 x 10^-11

3.) For each of these substances, calculate the milligrams of metallic ion per liter that can remain at equilibrium in a buffered solution at pH = 10.

Cu(OH)₂ Ksp = 1.6 x 10^-9

Fe(OH)₃ Ksp = 6.0 x 10^-38

Mg(OH)₂ Ksp = 6.0 x 10^-12

4.) Which salt — CaCO₃ or Ag₂CO₃ — is more soluble in water in units of moles per liter?

CaCO₃: K_sp = 2.8 x 10^-9

Ag₂CO₃: K_sp = 8.1 x 10^-12

5.) If 55 mg of lead (II) sulfate, PbSO₄, is placed in 250.0 mL of pure water, how much PbSO₄ will remain undissolved? Ksp for PbSO₄ is 2.53 x 10^-8.

6.) Will a precipitate form when 0.150 L of 0.10 M lead (II) nitrate and 0.100 L of 0.20 M NaCl are mixed? For PbCl₂, Ksp = 1.2x10^-5.

7.) What is the molar solubility of Pb(IO₃)₂ in a solution of 0.10 M Pb(NO₃)₂? Ksp for Pb(IO₃)₂ = 3.69 x 10^-13. Justify any approximations you make.

8.) Would it be possible to separate a solution containing 0.0020 M Pb²⁺ and 0.030 M Ag⁺ by adding drops of Na₂CO₃ solution? (K_sp for lead carbonate = 1.5 x 10^-13 and K_sp for silver carbonate = 8.2 x 10^-12)

9.) You wish to separate the metals in 100 mL of a solution of 0.10 M Ag⁺ and 0.10 M Pb²⁺.

Which metal will precipitate first if you add a solution of 0.10 M Br^- is small increments?

AgBr K_sp=3.3 x 10^-13

PbBr₂ K_sp=6.3 x 10^-6

What is the concentration of Br^- when the second metal just begins to precipitate?

What is the concentration of the first metal (identified in part a) that will be left in solution at the point that the second metal begins to precipitate?

Was this a successful separation?

Contributors and Attributions

Molly McGuire, Bucknell University (mmcguire@bucknell.edu)
Sourced from the Analytical Sciences Digital Library

Contributors and Attributions

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