Solubility Equilibria and Calculations

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Analytical Sciences Digital Library

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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 CrO₄^2-. 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 = K_sp, solution is saturated; if Q < K_sp, undersaturated; if Q > K_sp, 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 K_a 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 K_sp 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