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# Equilibrium Constants and Precipitation

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108. Consider a solution that is .022M in Fe2+ and .014M in Mg2+
a. if potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?
b. What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate.

109. a 120.0ml sample fo a solution that is 2.8x10^-3M in AgNO3 is mixed with a 225ml sample of a solution that is .1M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) remains?
110. Use the appropriate values of Ksp and Kf to find the equilibrium constant for the following reaction:
PbCl2(s) + 3OH-(aq)  Pb(OH)3-(aq) + 2Cl-(aq)

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The expert examines equilibrium constants and precipitations in solutions.

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108. Consider a solution that is .022M in Fe2+ and .014M in Mg2+
a. if potassium carbonate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?
b. What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate.
109. a 120.0ml sample fo a solution that is 2.8x10^-3M in AgNO3 is mixed with a 225ml sample of a solution that is .1M in NaCN. After the solution reaches equilibrium, what concentration of Ag+(aq) ...

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