3. A complex of chromium (Cr) was treated with H,SO, and HNO, then converted to dichromate ion Cr,0,2. The sample was then titrated with 0.112 N FeSO, and found that 24.5 mL of FeSO, was required to change the indicator color. Calculate the mass of Cr in the complex sample. [molar mass of Cr = 52.0 g/mol] 3 27 %3D
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![3. A complex of chromium (Cr) was treated with
H,SO, and HNO, then converted to dichromate
ion Cr,0,2. The sample was then titrated with
0.112 N FeSO, and found that 24.5 mL of FeSO,
was required to change the indicator color.
Calculate the mass of Cr in the complex sample.
[molar mass of Cr = 52.0 g/mol]
3
27
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- Ethylenediaminetetraacetate (EDTA4 ) is used as a complexing agent in chemical analysis with the structure shown in Fig. 21.7. Solutions of EDTA4 are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The complex ion virtually prevents the heavy metal ions from reacting with biochemical systems. The reaction of EDTA4 with Pb2+ is Pb2+(aq) + EDTA4(aq) iPbEDTA2(aq) K = 1.1 1018 Consider a solution with 0.010 mol of Pb(NO3)? added to 1.0 L of an aqueous solution buffered at pH = 13.00 and containing 0.050 M Na1EDTA. Does Pb(OH)2 precipitate from this solution? [Ksp for Pb(OH)2 = 1.2 1015.A cyanide solution with a volume of 13.72 mL was treated with 25.00 mL of Ni2+ solution(which contained an excess of Ni(II) ions) to convert the cyanide to the complex ion tetracyanonickelate(II): 4CN- + Ni2+ → 6 Ni(CN)2- The excess Ni 2+ was then titrated with 10.15 mL of 0.01307 M EDTA. One mole of this reagent reacts with one mole of Ni(II) as follows: Ni(CN)42- does not react with EDTA. If 39.35 mL of EDTA was required to react with 30.10 mL of the original Ni 2+ solution, calculate the molarity of CN- in the 13.72 mL cyanide sample.A sample contains Pb2+, Mg2+ and Zn2+. 0.4085 g of the sample is weighed and dissolved. Once dissolved it is with cyanide to form a complex and mask the zinc (Zn2++ 4 CN-→ Zn (CN)4 2-). The Pb2+ and Mg2+ in the solution are titrated with 42.22 mL of EDTA 0.02604 M. Then the Pb complex is treated with another organic ligand that masks Pb and releases EDTA, which is titrated with 19.35 mL of a Mg2+ 0.007657 M solution. For finalize formaldehyde is added to unmask the Zn2+(Zn (CN)4 2- + 4 HCHO + 4 H2O → Zn2+ + 4 HOCH2CN + 4 OH-). The liberated zinc is titrated with EDTA 0.02064 M consuming 28.63 mL. (Data: Pat Pb, 207.22; Pat Mg, 24.31; Pat Zn, 65.4). Find the percentage of the three metals in the sample.
- Write two half-equations for each reaction involved in the preparation of the complex (synthesize potassium tris(oxalato)chromium(III) trihydrate, K3[Cr(C2O4)3].3H2O ) using oxalic acid dihydrate, H2C2O4.2H2O, and potassium dichromate, K2Cr2O7, and a balanced equation for the overall reaction.A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 10.0 mL of a 0.100 M stock solution was added to 90.0 mL of solvent to make 100.0 mL of the first calibration standard solution and, secondly, 80 mL of that first calibration solution plus 20.0 mL of solvent were mixed to make the second calibration standard. What is the concentration of the second calibration standard solution?Complex Ion Formation and Precipitation Reactions i. A 1-L water sample was submitted for determination of chloride ion. 100.00mL the sample was analyzed using the Volhard method. 50.00 mL of 0.0929N AgNO3 was added to the sample and was back titrated with 12.50mL of 0.0510N KSCN solution to reach the end point. Find ppm Cl- in the water sample. ii. Using Mohr method, the chloride content of a mineral water was determined. 50.00mL of the sample was titrated with 10.80mL of 0.05N AgNO3 solution to reach end point. Determine the concentration of Cl- in ppm. iii. Calculate the hardness of a water sample such that 100.00mL of the sample required 35.00mL of 0.1051M EDTA solution to reach the end point.
- A second calibration standard solution of an iron(III) salicylate complex was prepared in two steps. First, 12.9 mL of a 0.481 M stock solution was diluted with solvent to make 100.0 mL of the first calibration standard solution and, secondly, 86.6 mL of that first calibration solution was diluted to 100 mL to make the second calibration standard. What is the molar concentration of the second calibration standard solution? Report your answer to 3 significant figures.A 0.87 g sample containing Ni (Mwt 58.693) was precipitated with dimethylglyoxime as Ni(II)/DMG complex (Mwt 288.91). Find the percentage (%) of Ni in the sample if the precipitate weighed 3.20 g.In complexation volumetry, classify the statements below as true or false.Justify the one(s) that you judge to be “false”.a) When preparing an EDTA solution, to be used as a titrant of Ca2+ ions, it is necessary to add a small amount of Mg2+ in the solution.b) A metallochromic (Ind) indicator is a substance that forms colored complexes with metallic ions. The colors of these complexes are always the same as the colors of the free forms of these indicators.c) In order for the titration of a metal (Me) with EDTA to be carried out, it is necessary that the Me-EDTA complex has a stability constant greater than that of the Me-Ind complex.d) In determining the partial hardness of a hard water sample with EDTA solution, murexide is used as an indicator at pH 10.
- What is the ligand to metal ratio for SCN-1 and Fe+3?a. write the net ionic equation involved in the formation of copper complexes in: Reagent added ligand added 1 control - 2 0.5 mL of 12M NH3 NH3 3 5 drops of 5M HCl Cl- b. starting from the copper (ii) complexes in the table above, write the net ionic equation involved in the ligand substitution reactions as observed in: Reagent added reagent added 1a 0.25 mL of 12 MNH3 1b 0.22g of KCl 2a 0.25 mL H2O 2b 0.22g of KCl 3a 0.25 mL H2O 3b 0.25 mL of 12M NH3An alloy containing Ni, Fe and Cr was analyzed by a complexation titration using EDTA as titrant. A 0.7176 g sample of the alloy was dissolved in HNO3 and diluted to 250 mL in a flask. A 50.00 mL aliquot of the sample, treated with pyrophosphate to mask Fe and Cr, required 26.14 mL of 0.05831 M EDTA to reach the murexide endpoint. A second 50.00 mL aliquot was treated with hexamethylenetetramine to mask Cr and titration with 0.05831 M EDTA required 35.43 mL to reach the murexide endpoint. Finally, a third 50.00 mL aliquot was treated with 50.00 mL of 0.05831 M EDTA and titrated back to the murexide endpoint with 6.21 mL of 0.06316 M Cu(II). the weight percentages of Ni, Fe and Cr in the alloy.
