13. A sample contained Cr(III) species. A 25.00 mL portion of this sample is combined with 10.00 mL of a 0.0875 M solution that contains a complexing agent, CDTA. This mixture is heated to boiling for several minutes to allow the CDTA to complex with Cr(III) species. The mixture is then cooled, and the excess CDTA is measured by a back titration using 0.0258 M Bi³+, required 4.20 mL to reach end point. Determine the original concentration of Cr(III) species in the sample [Molar ratio of CDTA:Cr(III):Bi³+ = 1:1:1]
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- Chromel is an alloy composed of nickel, iron and chromium.A 0.6472 g sample was dissolved and diluted to 250 mL. When a50 mL aliquot of 0.05182 M EDTA was mixed with an equal volumeof the diluted sample and all the three ions were chelated, a 5.11 mLback titration with 0.06241 M copper (II) was required.The chromium in a second 50 mL aliquot was masked through theaddition of hexamethylenetetramine, titration of the Fe and Nirequired 36.28 mL of 0.05182 M EDTA.Iron and chromium were masked with pyrophosphate in a third50 mL aliquot and the nickel was titrated with 25.91 mL of theEDTA solution.Calculate the percentage of nickel, chromium and iron in thealloy.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 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?
- 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.You are given a table of [CN-] standard solutions of different concentration. A 25 mL aliquot of each standard solution was added with Fe(NO3)3 to form a colored complex[Fe(CN)6]3-(aq). Each standard solution was then diluted to a total volume of50.0 mL. [CN–] prior to dilution, M [CN-] final M 0 0 0.04 0.1 0.16 0.24 0.32 0.4 What are the new concentrations for the standard solutions? Please show solutions.The brine solution has a significant amount of chloride, and it is determined by the Volhard method. A 10.0-aliquot of the solution is treated with 15.25 mL of standard 0.1163 M AgNO3 solution. The excess silver is titrated with standard 0.101 M KSCN solution, requiring 3.28 mL to reach the red Fe(SCN)2+ end point. Calculate the concentration of chloride in the brine solution in mg/L and g/L.
- Janine's research focuses on the ability of quercetin, a flavonoid and natural dye, to detect the presence of Co2+ in wastewater samples. She prepared a set of calibration standard solutions by adding an excess of quercetin to solutions of varying Co2+ concentration and maintaining it at pH 6.4 using a Tris-HCl buffer. The reaction yields a colored complex solution that has a maximum absorbance at 440 nm:Co2+ + 2 Quercetin --> Co(Quercetin)22+ The absorbance measurements for the calibration solutions prepared are shown in the tables; a cuvette with a 2.50 cm path length was used. [Co2+], in M Absorbance Color Wavelength range (nm) 0.05 0.100 Red 625-740 0.10 0.166 Orange 590-625 0.20 0.285 Yellow 565-590 0.30 0.367 Green 490-565 0.40 0.454 Blue 440-490 0.50 0.571 Violet 380-440 Part of her research is to determine the extent of Co2+ pollution in a stream near a pharmaceutical company. She obtained a 50.0-mL sample of the stream water and buffered it to pH 6.4. She…A cyanide solution with a volume of 10.33 mL was treated with 22.00 mL of Ni2+ solution (containing excess Ni2+) to convert the cyanide into tetracyanonickelate(II): 4CN−+Ni2+⟶Ni(CN)(2−)/4 The excess Ni2+ was then titrated with 11.85 mL of 0.01303 M ethylenediaminetetraacetic acid (EDTA): Ni2++EDTA4−⟶Ni(EDTA)2− Ni(CN)(2−)/4 does not react with EDTA. If 38.80 mL of EDTA were required to react with 30.47 mL of the original Ni2+ solution, calculate the molarity of CN− in the 10.33 mL cyanide sample. [CN-] = ________________________________Mb. EDTA cannot be used as a primary standard always. When can EDTA be used as a primarystandard ? Give reason why EDTA is used in complexometric titrations.
- The bismuth (AW 208.98) in 0.7405 g of an alloy was precipitated as BiOCl (FW 260.43) and separated from the solution by filtration. The washed precipitate was dissolved in nitric acid and treated with 18.25 mL of 0.1498 M AgNO3, causing the precipitation of AgCl. The excess AgNO3 required 13.98 mL of 0.1008 M KSCN for titration. Calculate the % Bi in the sample.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 solution containing chloride ion was analyzed by the Volhard method. A 50.00 mL sample containing chloride ion was treated with 25.00 mL of 0.2500 M silver nitrate. The precipitated AgCl was removed from the solution by filtration, and 1.00 mL of 0.1000 M Fe3+ was added to the filtrate. This new solution was then titrated with 10.67 mL of 0.2380 M KSCN. What is the concentration of chloride ion in the original solution?