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
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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?11. A 0.8000-g sample of iron ore containing 21.00% Fe is analyzed gravimetrically. If the final precipitate (assumed to be Fe,03) contains 20.0 mg of Al,03 by mistake, what percentage of Fe does the analyst find?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
- 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, pleaseThe concentration of ammonia in a cleaning product was determined by back titration.Firstly, 10.00 cm3 of the cleaning product was pipetted into a large conical flask,containing 250.00cm3 of 0.50 mol/l HCl to give Solution A.Following a period of reaction and shaking, 50.00cm3 of Solution A was removed anddiluted to 250 cm3 with water in a volumetric flask to give Solution B.20 cm3 samples of Solution B were titrated against 0.05 mol/l Na2CO3 solution, givingan average titre of 12.45 cm3. i) Write equations for the reactions that have taken place.ii) Determine the concentration of NH3 in the original cleaning product in mol/l,g/l, ppm, and % w/v.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.
- Potassium thiocyanate, KSCN, is often used to detect thepresence of Fe³⁺ ions in solution through the formation of thered Fe(H₂O)₅SCN²⁺(or, more simply, FeSCN²⁺). What is[Fe³⁺] when 0.50 L each of 0.0015 MFe(NO₃)₃ and 0.20 MKSCN are mixed? Kfof FeSCN²⁺=8.9X10².A solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by slowly adding Na2CO3 aq solution? Assume that for successful separation 99% of the metal ion must be precipitated before the other metal ion begins to precipitate, and assume no volume change on addition of Na2CO3 solution. Pls show step by step. Ksp of CuCO3 = 1.4 x10-10 Ksp of NiCO3 = 1.42X 10-7 B. If you need to redissolve the salt that was first precipitated, what pH will you use and why ?5) 3 L contaminated air 50 mL 0.0116 M in an air pollution analysis Carbon dioxide (CO2) BaCO3 is passed through Ba (OH) 2 solution. as precipitated. Excess of base, next to phenol phthalate (f.f.) indicator It is titrated with 23.6 mL of 0.0108 M HCl. CO2 in this air sample Calculate its concentration in ppm. (Density of CO2 Take it as 1.98 g / L. C = 12, O = 16 g / mol).
- What concentration of K4Fe(CN)6 should be in a suspension of solid Zn₂ Fe(CN)6 in water to give [Zn²+] = 5.0 x 10-7 M? Ksp for zinc ferrocyanide is 2.1 x 10-16. What concentration of Fe(CN)64+ (ferrocyanide) is in equilibrium with 1.0 μM Ag+ and Ag4 Fe(CN)6(s)? Ksp for silver ferrocyanide can be found in appendix A.Directions: Solve the problem with a complete step-by-step solution. A 100.0-mL sample of brackish water was made ammoniacal, and the sulfide it contained was titrated with 16.47 mL of 0.02310 M AgNO3. The analytical reaction is 2Ag+ + S2- ---> Ag2S (s)Calculate the concentration of H2S in the water in parts per million, cppm.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.