Consider a solution that is 2.0 x 10^-2 M in Fe^2+ and 1.4 x 10^-2 M in Mg^2+. P
ID: 974791 • Letter: C
Question
Consider a solution that is 2.0 x 10^-2 M in Fe^2+ and 1.4 x 10^-2 M in Mg^2+.Part 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?
A.) Fe^2+ B.) Mg^2+
Part B
What minimum concentration of K_2CO_3 is required to cause the precipitation of the cation that precipitates first?
Express your answer using two significant figures.
[K_2CO_3] = ? Consider a solution that is 2.0 x 10^-2 M in Fe^2+ and 1.4 x 10^-2 M in Mg^2+.
Part 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?
A.) Fe^2+ B.) Mg^2+
Part B
What minimum concentration of K_2CO_3 is required to cause the precipitation of the cation that precipitates first?
Express your answer using two significant figures.
[K_2CO_3] = ?
Part 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?
A.) Fe^2+ B.) Mg^2+
Part B Part 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?
A.) Fe^2+ B.) Mg^2+
Part B
What minimum concentration of K_2CO_3 is required to cause the precipitation of the cation that precipitates first?
Express your answer using two significant figures.
[K_2CO_3] = ?
Explanation / Answer
the data on KSP is
FeCO3= 1.5*10-11 and that of MgCO3=6.8*10-6
since KSp of MgCO3> Ksp of FeCO3
Fe+2 has to get precipitated first.
Part B :
FeCO3----> Fe+2 +CO3-2
Ksp = [Fe+2] [CO3-2]
1.5*10-11= x2, where x is solubility of K2CO3
x= 3.87*10-6 M