Which of the following is true at the equivalence point in the titration of Fe³+ with EDTA? Select one: O [Fe³+] = Cy O [Fe³+] = Cy- [FeY] O [Fe³+] = [FeY] O [FeY] = Cy
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no 11
![Which of the following is true at the equivalence point in the titration of Fe³+ with EDTA?
Select one:
O [Fe³+] = Cy
O [Fe³+] = Cy- [FeY-]
O [Fe³+] = [FeY]
O [FeY] = Cy](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F73f501d7-87bd-47c0-8a85-010e22bb107b%2F0e736264-032a-4c15-a360-7cee649ee6cf%2Fc4034o_processed.png&w=3840&q=75)
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- The titration of Zn+2 and EDTA is carried out in the same manner as the Mg+2-EDTA titration. In this case, the ammonia in the EDTA buffer serves an additional purpose, what is it?At pH 7, what metal ions can be titrated by EDTA?Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?
- 0.8153 g of a sample containing Pb(NO3)2 was taken, dissolved in water, and 40.20 mL of 0.06 M EDTA was added. What is the percentage of Pb(NO3)2 since the excess EDTA is back-titrated with 23.10 mL of 0.02 M EDTA? (Pb(NO3)2: 331 g/mol, Pb: 207 g/mol)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.Hardness in groundwater is due to the presence of metal ions, primarily Mg2+and Ca2+. Hardness is generally reported asppm (mg/L) CaCO3or mmol/L Ca2+. To measure water hardness, a sample of groundwater is titrated with EDTA, a chelating agent, in the presence of the indicator eriochrome black T, symbolized here as In. Eriochrome black T, a weaker chelating agent than EDTA, is red in the presence of Ca2+and turns blue when Ca2+is removed. A 50.00-mL sample of groundwater is titrated with 0.0850M EDTA. Assume that Ca2+accounts for all of the hardness in the groundwater. If 10.10 mL of EDTA is required to titrate the 50.00-mL sample, what is the hardness of the groundwater in molarity Ca2+and in ppm CaCO3?
- As part of a geological team that studied a local cave, you brought with you a bunch of 1.00 g rock samples to be studied. Each rock was prepared and titrated against 0.050 M EDTA. a. Calculate the percent calcite (CaCO3) content of rock A if it was titrated with 48.0 mL EDTAThe hardness of a water sample may be determined by titrating a 100-mL sample of water with 0.010 M EDTA. If the Eriochrome Black T (EBT) end point occurs after 12.3 mL of the EDTA solution is added, calculate the water hardness in terms of (1) ppm CaCO3 and (2) mM Ca2+.Would tris(2,29-bipyridine)iron be a useful indicator for the titration of Sn21 in 1 M HCl with Mn(EDTA)2? (Hint: The potential at the equivalence point must be between the potentials for each redox couple.)
- A 0.5745 g sample of an alloy containing principally bismuth and lead is dissolved in nitric acid and diluted to 250.0 mL in a volumetric flask. A 50.00 mL aliquot is withdrawn, the pH adjusted to 1.5, and the bismuth titrated with 30.26 mL of 0.01024 M EDTA. The pH of the solution is then increased to 5.0 and the lead titrated with 20.42 mL of the same EDTA solution. Calculate the percentages of lead and bismuth in the alloy.Calamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?Calculate the potential in the solution in the titration of 50.0 mL of 0.100 M Fe2+ in 1.00 M HCl4 with 0.0167 M Cr2O7 2- at 10.0, 25.0, 50.0 and 60.0 titrant added.