I have 250mL of a solution that is 0.100 M Fe(NO3). 0.100 M Cu(NO3)2 and 0.50 M Ca(NO3)2. 1 want to separate the metals. I have solid sodium carbonate (NaCO3), solid Na3PO4, and solid NaOH in the stockroom. a.) Which solid should I add to get the best separation b.) how much of the first ion precipitate is left in solution when the second ion begins to precipitate? please explain and solve

I have 250mL of a solution that is 0.100 M Fe(NO3). 0.100 M Cu(NO3)2 and 0.50 M Ca(NO3)2. 1 want to separate the metals. I have solid sodium carbonate (NaCO3), solid Na3PO4, and solid NaOH in the stockroom. a.) Which solid should I add to get the best separation b.) how much of the first ion precipitate is left in solution when the second ion begins to precipitate? please explain and solve

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter3: Statistical Tests With Excel

Section: Chapter Questions

Problem 6P

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I have 250mL of a solution that is 0.100 M Fe(NO3). 0.100 M Cu(NO3)2 and 0.50 M Ca(NO3)2. I want to separate the metals. I have solid sodium carbonate (NaCO3), solid Na3PO4, and solid NaOH in the stockroom. a.) Which sild should I add to get the best separation b.) how much of the first ion precipitate is left in solution when the second ion begins to precipitate?
A solution is prepared by mixing 50.0 mL of 0.50 M Cu(NO3)2 with 50.0 mL of 0.50 M Co(NO3)2. Sodium hydroxide is added to the mixture. Which hydroxide precipitates first and what concentration of hydroxide ions present in solution will accomplish the separation? Hint : Look up Ksp for Cu(OH)2 and Co(OH)2. Show work, please
the solubility of Ba(IO3)2 in a solution prepared by mixing 300 mL of 0.010 M Ba(NO3)2 with 200 mL of 0.10 M NaIO3 .(K.S.P=1.57X 10-9) is
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5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
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During the experiment, to obtain the Beer's law plot for FeSCN2+ ion at various concentrations, the following solutions are mixed to form a solution of FeSCN2+ through reaction as follows: Fe3+ + SCN- <=> FeSCN2+ 2.9 mL 0.2 M Fe(NO3)3 in 0.50M HNO3 , 1.5 mL 0.50M HNO3, and 1.4 mL 2.00 x 10–2 M KSCN in 0.50M HNO3. Assuming all SCN- ion is converted to product FeSCN2+ , determine the concentration of FeSCN2+ in the reaction mixture.