I have 2.00 L of a solution that is 0.022 M in Fe2+ and 0.014 M...
I have 2.00 L of a solution that is 0.022 M in Fe2+ and 0.014 M in Pb2+. I start to gradually dissolve sodium carbonate (Na2CO3) in the solution to selectively precipitate the two metals. What mass of sodium carbonate must be added to cause the first cation to precipitate? What is that cation?
What is the remaining concentration of the cation that precipitate first when the other cation has just begun to precipitate?
Homework Answers
![22 me puring con entrations of Fete psta are- [feet)= 0.022M (PL+2]; O.olum. Now when we add Mazeos to the solutor, he cation](http://img.homeworklib.com/questions/18de4ac0-4b10-11eb-a4f5-8b9556ffb629.png?x-oss-process=image/resize,w_560)
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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...
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...
A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and...
A solution of Na2CO3 is added dropwise to a solution that contains 1.00×10-2 M Fe2+ and 1.49×10-2 M Cd2+. What concentration of CO32- is need to initiate precipitation? Neglect any volume changes during the addition. Ksp value: FeCO3: 2.10*10-11 Ksp value: CdCO3: 1.80*10-14 Which cation precipitates first? What is the concentration of CO32- when the second cation begins to precipitate?
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...
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...
A solution of NaOH is added dropwise to a solution that is 0.0224 M in Fe2+ and 3.60e-15 M in Ga3+. The Ksp of Fe(OH)2 i...
A solution of NaOH is added dropwise to a solution that is 0.0224 M in Fe2+ and 3.60e-15 M in Ga3+. The Ksp of Fe(OH)2 is 4.87e-17. The Ksp of Ga(OH)3 is 7.28e-36. (a) What concentration of OH- is necessary to begin precipitation? (Neglect volume changes.) [OH-] = M (b) Which cation precipitates first? Fe2+ Ga3+ (c) What is the concentration of OH- when the second cation begins to precipitate? [OH-] = M
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is diss...
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is dissolved in 1.00 grams of Nal can be dissolved in this solution without a precipitate 4.) (Modified from Chemistry: A Molecular Approach, 1" Ed. by Tro) Consider a solution that is 0.024 M in Cu and 0.017 M in Fe (a) If sodium hydroxide is used to selectively...
Suppose you slowly add solid sodium carbonate (Na2CO3) to a solution that contains 0.030 M Pb2+...
Suppose you slowly add solid sodium carbonate (Na2CO3) to a solution that contains 0.030 M Pb2+ and 0.030 M Ni2+. What is the minimum concentration of CO32– that would cause a precipitate to form? (Assume no volume change; for PbCO3, Ksp = 7.4x10–11, and for NiCO3, Ksp = 1.3x10–7)
2. A solution is 0.01 M in Ba2+ and 0.01 M in Cal. Sodium sulfate is added to selectively precipitate one of the ca...
2. A solution is 0.01 M in Ba2+ and 0.01 M in Cal. Sodium sulfate is added to selectively precipitate one of the cations, while leaving the other in solution. a) Given that BaSO4 and CaSO4 have kse values of 1.07 x 10-10 and 7.10 x 105 respectively, which cation will precipitate first? Explain why. b) What is the minimum concentration of S0,2" that will trigger the precipitation of the cation that precipitates first?
A) A solution of Na2CO3 is added dropwise to a solution that contains 1.23×10−2 M Fe2+...
A) A solution of Na2CO3 is added dropwise to a solution that contains 1.23×10−2 M Fe2+ and 1.59×10−2 M Cd2+. What concentration of CO32− is need to initiate precipitation? Neglect any volume changes during the addition. Answer is = [CO32−] = 1.13×10−12 M B) In the solution from Part A, what will the concentration of CO32− be at the moment before Fe2+ begins to precipitate?
A solution contains 0.0100 M Ca2+ and 0.0500 M Sr2+. Can 99% of the first cation...
A solution contains 0.0100 M Ca2+ and 0.0500 M Sr2+. Can 99% of the first cation be precipitated before the second cation starts to precipitate as Na2CO3 is added to the solution? Find Ksp values in the table of solubility-product constants. For CaCO3, use the aragonite Ksp value. yes not enough information no What is the concentration of the first cation when the second cation starts to precipitate? concentration of the first cation:
A solution of Na2CO3 is added dropwise to a solution that is 0.0852 M in Y3+...
A solution of Na2CO3 is added dropwise to a solution that is 0.0852 M in Y3+ and 0.0413 M in Cd2+. The Ksp of Y2(CO3)3 is 1.03e-31. The Ksp of CdCO3 is 1e-12. (a) What concentration of CO32- is necessary to begin precipitation? (Neglect volume changes.) [CO32-] = M. (b) Which cation precipitates first? Y3+ Cd2+ (c) What is the concentration of CO32- when the second cation begins to precipitate? [CO32-] = M.
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...
3.) (Taken from General Chemistry: Principals and Modern Applications(8 Ed.) by Petrucci, Harwood L of 1.00 M NH,. How many of AgI(s) forming? and Herring) A 0.10 mol sample of AgNO,(s) is dissolved in 1.00 grams of Nal can be dissolved in this solution without a precipitate 4.) (Modified from Chemistry: A Molecular Approach, 1" Ed. by Tro) Consider a solution that is 0.024 M in Cu and 0.017 M in Fe (a) If sodium hydroxide is used to selectively...
2. A solution is 0.01 M in Ba2+ and 0.01 M in Cal. Sodium sulfate is added to selectively precipitate one of the cations, while leaving the other in solution. a) Given that BaSO4 and CaSO4 have kse values of 1.07 x 10-10 and 7.10 x 105 respectively, which cation will precipitate first? Explain why. b) What is the minimum concentration of S0,2" that will trigger the precipitation of the cation that precipitates first?
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