clearly solved full solution is required ASAP. The stability contact values of M1-EDTA, M2-EDTA, M3-EDTA, M4-EDTAcomplexes are 2.1 x 10", 7.8 x 10", 9.7 x 10 and 1.1 x 10, respecctively.You are estimating unknown concentrations of these four metal ions (M,M2, M3 and M.) by titration against standard EDTA, which mctal ion willallow you the sharpest end point detection(a) M1(b) M2(c) M3(d) M4

In EDTA Titration,larger stability constant indicates that the reaction is more complete and larger…

The stability contact values of M1-EDTA, M2-EDTA, M3-EDTA, M-EDTA complexes are 2.1 x 10", 7.8 x 10", 9.7 x 10° and 1.1 x 102, respectively. You are estimating unknown concentrations of these four metal ions (M. M2, M3 and M.) by titration against standard EDTA, which mctal ion will allow you the sharpest end point detection

The stability contact values of M1-EDTA, M2-EDTA, M3-EDTA, M-EDTA complexes are 2.1 x 10", 7.8 x 10", 9.7 x 10° and 1.1 x 102, respectively. You are estimating unknown concentrations of these four metal ions (M. M2, M3 and M.) by titration against standard EDTA, which mctal ion will allow you the sharpest end point detection

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter31: Introduction To Analytical Separations

Section: Chapter Questions

Problem 31.18QAP

See similar textbooks

Similar questions

Calculate the pZn2+ for solutions prepared by adding 0.00, 5.00, 10.00, 15.00, 20.00, 25.00 and 30.00 mL of 0.0100 M EDTA to 25.00 mL of 0.00250 M Zn2+. Assume that both the Zn2+ and EDTA are 0.0100 M in NH3 to provide a constant pH of 9.0
Consider the titration of 25.0ml 0.0100M Sn2+ by 0.0500M Tl3+ in 1M HCl using Pt and saturated calomel electrodes , calculate E at following volumes of Tl3+ : 1, 5 and 10ml
You are asked to titrate a Mn3+ solution with EDTA at pH 9.00. The overall ionic strength of the solution is 0.10 M. Mn3+ +EDTA4- ⇌ MnEDTA- log K = 25.2 a. Calculate the conditional formation constant for MnEDTA- at pH 9.00 b. Calculate the equilibrium [Mn3+] at pH 9.00 for total Mn3+ = 2.0 mM i) total EDTA = 0.50 mM ii) total EDTA = 5.00 mM
What is the rationale of maintaining the analyte solution at high pH (~10) in the titration process with EDTA? At this pH, EDTA is at its fully deprotonated form, Y-4. At this pH, EDTA is partially deprotonated with 1 ionizable H+. At this pH, EDTA is at its fully protonated form, H4Y. At this pH, EDTA is partially deprotonated with 2 ionizable H+.
(i) You have been provided with a sample collected from a water pool beside a slag heap at the iron ore mine. 35 uL of the sample is added to 1165 uL of buffered ferrozine (excess). If the %T recorded at 562 nm in a 2 mm cuvette is found to be 25%, calculate the concentration of Fe(II) in the sample in mol L−1 and ppm. Comment on the contamination level. (ii) Comment on a possible contaminant that could interfere with the assay and suggest an approach that could be used to account for its presence.
An EDTA solution was allowed to react with Pb²⁺ to produce 0.25 M PbY²⁻, 2.67×10⁻⁸ M Pb²⁺ and an excess of 0.10 M at equilibrium (K = 1.1×10⁸). What will be the α₄ value under these conditions?
b. 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.
A 1.509-g samle of a Pb/Cd alloy was dissolved in acid and diluted to exactly 250.0 mL in a volumetric flask. A 50.00-mL aliquot of the diluted solution was brought to a pH of 10.0 with an HCN/NaCN buffer, which also served to mask the Cd2+; 11.56mL of the EDTA solution were needed to titrate the Pb2+. Calculate the percentage of Pb and Cd in the sample.
50 mL of a solution of 0.0200 M Zn2+ will be titrated with 0.0100 M EDTA in 0.0100 M NH3 at pH 6.0. Ethylenediaminetetraacetic acid (EDTA) can be considered as a tetraprotic acid (H4Y). The stepwise acid dissociation constants are: K1 = 1.02 x 10-2, K2= 2.14 x 10-3, K3 = 6.92 x 10-7 and K4 = 5.50 x 10-11. The alplia value of the un-deprotonated species in a solution buffered to a certain pH is given by the following equation: a0 = [H+]4/([H+]4 + K1[H+]3 + K1K2[H+]2 + K1 K2K3[H+] + K1 K2K3K4) Calculate the alpha value of the fully deprotonated species (Y4- ) in a solution buffered to a pH of 6.0.
When using ion-selective electrodes, to comensate for a complex or unknown matrix, the __________ method can be used to determine the analyte concentration. a) least-squares analysis b) standardization c)standard addition d)dilution e)calibration curve
A 25.00 mL sample containing Fe3+ was treated with 10.00 mL of 0.03676 M EDTA to complex all the Fe3+ and leave excess EDTA in solution. The excess EDTA was then back-titrated, requiring 2.37 mL of 0.04615 M Mg2+. What was the concentration of Fe3+ in the original solution in ppm Fe3+?
A 40.00-mL aliquot of 0.05000 M HNO2 is diluted to 75.00 mL and titrated with 0.0800 M Ce4+. The pH of the solution is maintained at 1.00 throughout the titration; the formal potential of the cerium system is 1.44V a. Calculate the potential of the indicator electrode with respect to a saturated calomel reference electrode after the addition of 5.00, 10.00, 15.00, 25.00, 40.00, 49.00, 49.50, 49.60, 49.70, 49.80, 49.90, 49.95, 49.99, 50.00, 50.01, 50.05, 50.10, 50.20, 50.30, 50.40, 50.50, 51.00, 60.00, 75.00 and 90.00 mL of Cerium (IV). b. Draw a titration curve for these data. c. Generate a first- and second-derivative curve for these data. Does the volume at which the second-derivative curve crosses zero correspond to the theoretical equivalence point? Why or why not?