An accurately weighed chelometric standard calcium carbonate of 200 mgwas used to standardize Disodium Ethylenediaminetetraacetate, using thesame procedures set by the monograph. If the molarity of the DisodiumEDTA was found to be 0.054 M, what is the final volume (mL) of the titrantused?

Disodium ethylenediaminetetraacetate, also known as disodium EDTA, has the following structure: In…

using the An accurately weighed chelometric standard calcium carbonate of 200 mg was used to standardize Disodium Ethylenediaminetetraacetate, same procedures set by the monograph. If the molarity of the Disodium EDTA was found to be 0.054 M, what is the final volume (mL) of the titrant used?

using the An accurately weighed chelometric standard calcium carbonate of 200 mg was used to standardize Disodium Ethylenediaminetetraacetate, same procedures set by the monograph. If the molarity of the Disodium EDTA was found to be 0.054 M, what is the final volume (mL) of the titrant used?

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.40QAP

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An accurately weighed chelometric standard calcium carbonate of 200 mg was used to standardize Disodium Ethylenediaminetetraacetate, using the same procedures set by the monograph. If the molarity of the Disodium EDTA was found to be 0.054 M, what is the final volume of the titrant used?
A solution containing Mg2+ was buffered to pH 9.81 and titrated with EDTA. Eriochrome black T, with p?a1 = 6.3 and p?a2 = 11.6 was used as the indicator. It is a diprotic acid, H2E What is the fraction of the predominant form of eriochrome black T in solution at this pH? (To answer this, report the alpha fraction of the indicator’s most prevalent species at this pH)
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.
3. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation ofthe end point was equal to 13.03 mL. Based on this information,a) Outline the two steps involved, representing the related reactions./5b) Calculate the concentrations of CaCO3 and MgCO3 present in the initialsolution./6c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6d) Calculate the…
An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask. and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, (a) Outline the two steps involved, representing the related reactions. (b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution. (c) Calculate the masses of CaCO3 and MgCO3 present in the pellet. (d) Calculate the…
. An antacid tablet, weighing 1.25 g, was dissolved in a 1.0 L volumetric flask to allow for determination of calcium carbonate and magnesium carbonate contents. After preparing the solution, an aliquot of 10.0 ml was transferred to an Erlenmeyer flask containing a buffer solution with pH = 10. This aliquot was then titrated with EDTA 0.0040 mol/L and the average volume spent was 15.01 mL. To measure calcium after precipitation. After the magnesium was fractionated, a second 10.00 mL aliquot of the stock solution was transferred to an Erlenmeyer flask, and the pH of the present solution was adjusted to a value of approximately 13. In EDTA titration, the volume consumed for observation of the end point was equal to 13.03 mL. Based on this information, a) Outline the two steps involved, representing the related reactions./5 b) Calculate the concentrations of CaCO3 and MgCO3 present in the initial solution./6 c) Calculate the masses of CaCO3 and MgCO3 present in the pellet./6 d) Calculate…
An antihistamine sample, brompheniramine maleate, weighing 5.01234 g was dissolved in alcohol and decomposed with metallic sodium. The resulting solution was treated with 12.00mL of 0.3121M AgNO3 to precipitate all of the liberated bromide ions as AgBr. The excess AgNO3 remaining in the solution was titrated with 9.123mL of 0.2181M KSCN to reach the endpoint. What is the %Br in the sample? Br- + Ag+ --> AgBr(s) Ag+ + SCN- --> AgSCN(s) Br = 79.904 g/mol
1. an accurately weighed chelometric standard calcium carbonate of 150 mg was used to standardize Disodium ethylenediaminetetraacetate, using the same procedure set by the monograph. The total volume of EDTA consumed was 37.5 ml . Calculate the molarity and normality of the standard solution. 2. A 0.62L of 0.072N silver nitrate was used to titrate three samples of sodium lauryl sulfate with 2500 mg,5000mg, and 6750 mg respectively. Tabulate its data, calculate the %NaCl in each sample , did any sample conformed to the official requirement?
A student has a sea water sample which contains Ca2+ ions . Describe briefly how he willdetermine the concentration of Ca2+ ion in the sample using a simple titration. Explain the colourchanges at the endpoint. Which medium is suitable for performing the titration, acidic or basic medium and why?
Explain brieflyWhat would happen to the total hardness if the solution was buffered to pH 13.00? What is done to the soda ash solution when the pre-equivalence point of the methyl orange endpoint is reached? What compound is trying to be removed?
In determination of mixed alkali, does adding H2O to the analyte can afect the process of titration?
A 25.00 ml of Ni2+ solution was diluted in HCl and treated with 25.00 ml of 0.05283 MNa2EDTA. The solution was neutralized with NaOH followed by addition of acetate buffer untilthe pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator.Back titration using standard 0.022 MZn2+ at pH 5.5 requires 17.61 ml until end point, onwhich the solution will turn red. Calculate for the molarity of the unknown.