You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and each at a concentration of 0.010 M. You will accomplish this by titrating (adding slowly) sodium sulfate (Na2SO4). (Ksp for CaSO4 = 4.9 x 10^-5; Ksp for PbSO4 = 1.3 x 10^-8 at 25 degrees C). a. Which will be the first salt to precipitate b. What will be the concentration of the first ion to precipitate (Ca2+ or Pb2+) be when the second salt begins to precipitate?
You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and each at a concentration of 0.010 M. You will accomplish this by titrating (adding slowly) sodium sulfate (Na2SO4). (Ksp for CaSO4 = 4.9 x 10^-5; Ksp for PbSO4 = 1.3 x 10^-8 at 25 degrees C). a. Which will be the first salt to precipitate b. What will be the concentration of the first ion to precipitate (Ca2+ or Pb2+) be when the second salt begins to precipitate?
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and each at a concentration of 0.010 M. You will accomplish this by titrating (adding slowly) sodium sulfate (Na2SO4). (Ksp for CaSO4 = 4.9 x 10^-5; Ksp for PbSO4 = 1.3 x 10^-8 at 25 degrees C).
a. Which will be the first salt to precipitate
b. What will be the concentration of the first ion to precipitate (Ca2+ or Pb2+) be when the second salt begins to precipitate?
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