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Solubility Equilibria and Calculations

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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









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