A 25.00 mL sample containing an unknown amount of Al3+ and Pb2+ required 20.51 mL of 0.04633 M EDTA to reach the endpoint. A 50.00 mL sample of the unknown was then treated with F to mask the Al³+. To the 50.00 mL sample, 25.00 mL of0.04633 M EDTA was added. The excess EDTA was then titrated with 0.02353 M Mn²+. A total of 14.2 mL was required toreach the methylthymol blue end point. Determine pAl3+ and pPb2+ in the unknown sample.PA3+ ;pPb²+II

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Answered: A 25.00 mL sample containing an unknown…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.29QAP

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A 25.00 mL sample containing an unknown amount of AI* and Pb+ required 15.40 mL of 0.05788 M EDTA to reach the end point. A 50.00 mL sample of the unknown was then treated with F to mask the Al+. To the 50.00 mL sample, 25.00 mL of 0.05788 M EDTA was added. The excess EDTA was then titrated with 0.02329 M Mn2+. A total of 27.5 mL was required to reach the methylthymol blue end point. Determine pAl+ and pPh?+ in the unknown sample. PAI+
A 15.00 mL urine specimen containing Ca2+ and Mg2+ was diluted to 2.000 L. A 10.00 mL sample was taken and buffered to a pH of 10 and required 27.32 mL of 0.003960 M EDTA to react with 'all' the Ca²+ and Mg2+. A second 10.00 mL sample was taken and all the Ca²+ was precipitated as Ca(C204)(s). The Ca(C2O4) (s) precipitate was then taken and dissolved in 18.00 mL of water, buffered to a pH of 10, and required 12.21 mL of 0.003960 M EDTA solution to react with all the Ca2+. Calculate the concentration of Ca²+ and Mg2+ in the original urine specimen.
3. A water sample was tested for water hardness. A 50.00 mL sample, prepared and buffered to pH 10, required 23.55 mL of 0.0250 M EDTA. A second 50.00 mL aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA solution. Calculate the total hardness of the water sample, express in ppm CaCO3 Calculate the concentration of CaCO3 in the sample in ppm Calculate the concentration of MgCO3 in the sample in ppm а. b. С.
A solution is prepared by mixed 50.0 mL of 0.0400 M Ni2+ with 50.00 mL of 0.0400 M EDTA.Calculate the concentration of Ni 2+ after mixing. The mixture is buffered to a pH of 3.0. KNiY =4.2x1018, alpha4 =2.5x10 -11.
A 50.00 mL sample of hard water is titrated with 0.0102 M EDTA solution (volume of blank titration= 1.5 mL) and the volume of EDTA required is 22.44mL. What is the water hardness in ppm CaCO3?
C- Al is determined by titrating with EDTA:- Al" +H;Y * AIY +2H 0.5 mg sample required 20.5 ml. EDTA for titration. The EDTA was standardized by titrating 25 ml. of 0.01M CaCl, solution, requiring 30 ml. EDTA. Calculate Al:0, in the sample.
In the titration of 50 mL 0.02 M Sr² with 0.02 M EDTA in a buffered medium at titrated pH 11, calculate the psr value for the addition of 10 mL EDTA
a. A 40.0 mL sample containing 0.0400 M Ni2+ was titrated with 0.0400 M EDTA at pH 11.0. Given pKNiY = 18.62 and α = 0.85. Calculate pNi at 0, 10, 100 and 110% of the titration.
a. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. b. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L.
The concentration of CA2+ in an unknown solution was determined by titration with the EDTA solution standardized with a molarity of 0.000085 M. 25 mL of the unknown solution was diluted to 250 mL with deionized water. A 25 mL aliquot of the diluted solution was then titrated with the EDTA solution. The titration required 35.54 mL of the EDTA solution to each the end point. What is the molarity of calcium in the original unknown solution?
A 50.00 ml aliquot of a solution containing Ca2+ and Mg2+ was buffered at pH 10 and titrated with 0.0493 M EDTA. The endpoint volume was 42.15 ml. A second aliquot of the same mixture was made strongly basic by the addition of NaOH – this causes the Mg2+ to precipitate as Mg(OH)2. The solution was then titrated with the 0.0493 M EDTA and the endpoint volume was found to be 35.65 ml. Calculate the molar concentration of Mg
A 25.00 mL sample of water, buffered at a pH of 10, is titrated with 0.008989 M EDTA using the Calmagite indicator. A volume of 8.15 mL of EDTA is required. Determine the hardness of the water sample in ppm.

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