Solubility Equilibria and Calculations
- Page ID
- 283090
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Name: _________________________
1) Given the following reactions and equilibrium constants:
\[\ce{SnO2 (s) + 2 H2 (g) ⇆ Sn (s) + 2 H2O (g)} \hspace{30px} \mathrm{K_1 = 8.12}\nonumber\]
\[\ce{H2 (g) + CO2 (g) ⇆ H2O (g) + CO (g)} \hspace{30px} \mathrm{K_2 = 0.771}\nonumber\]
Calculate K3 for the reaction:
\[\ce{SnO2 (s) + 2 CO (g) ↔ Sn (s) + 2 CO2 (g)}\nonumber\]
2) Consider a solution that is to be made 0.01 M in each of the following ions: Ba2+ and CrO42-. We assume these are concentrations present initially, before any reaction has occurred. Calculate the reaction quotient (Q) to determine whether or not BaCrO4 will precipitate out of the solution.
\[\ce{BaCrO4(s) ↔ Ba^2+ + CrO4^2-}\nonumber\]
If Q = Ksp, solution is saturated; if Q < Ksp, undersaturated; if Q > Ksp, supersaturated.
3) Calculate the solubility (in deionized water) of the following compound. Express the solubility of CuN3, copper(I) azide in mol/L.
\[\ce{CuN3 (s) ↔ Cu+(aq) + N3- (aq)} \hspace{30px} \mathrm{K_{sp} = 4.9 \times 10^{-9}}\nonumber\]
Name: _________________________
1) Use the systematic treatment of equilibrium to determine [Zn2+] in a saturated solution of Zn(CN)2 with a fixed pH of 3.110. The Ka for HCN is 6.2x10-10
Name: _________________________
1) Find the relative error introduced by neglecting activity in calculating the solubility of Ba(IO3)2 in a 500 mL solution that is 0.033M CaCl2. The Ksp of Ba(IO3)2 = 1.57x10-9
Contributors and Attributions
- Sarah Gray, Stockton University (sarah.gray@stockton.edu)
- Sourced from the Analytical Sciences Digital Library