BaSO4 Ksp = 1.1*10^-10
CaSO4 KSp = 2.4*10^-5
first to precipitate is BaSO4
so
Ksp = [Ba+2][SO4-2]
1.1*10^-10 = (10^-2)(M)
M =(1.1*10^-10)/(10^-2) = 1.1*10^-8 M of Na2SO4
Consider a solution that is 1 0 times 10^-2 M in Ba^2+ and 1 9 times...
Consider a solution that is 2.4×10−2 M in Fe2+ and 1.8×10−2 M in Mg2+. [K2CO3] = 1.3×10−9 M is the minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? Express your answer using two significant...
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
2002 - Review Constants Periodic Consider a solution that is 1.3x10-2 Min Ba? and 20x10-2 Min Cat - Part A sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? Ba? О саа Submit Request Answer Part B What minimum concentration of N, 80, is required to cause the precipitation of the cation that precipitate Express your answer using two significant figures. ? AERO? Na,80 Submit Request...
Part B is finished. Part C is the question: What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitates? This is a complete question. Part B simply gives background information needed. Please answer. Edit: I do not completely understand what you mean by solution information. The only other information given would be which cation will precipitate first, which would be Ba 2+, the concentration of the cation is 1.3 x 10^-2,...
Consider a solution that is 2.4×10−2 M in Fe2+and 1.1×10−2 M in Mg2+. a) What minimum concentration of K2CO3 is required to cause the precipitation of the cation that precipitates first?
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