1. Complete and turn in the Data and Calculations page for this experiment. Include calculations for the determination of the exact concentration of your group’s EDTA solution, and the Ca2+ ion concentration (in M) and the hardness (in ppm CaCO3) of yourunknown water sample. Organize and label your calculations and report all measurementsand calculations with the correct number of significant figures.2. How would you characterize the precision of your experimental measurements in this lab?Is the level of precision reasonable or unreasonable? Explain your answer.Data and Calculations PageRecord all of your group’s experimental data below. Carry out and include all of the calculations needed to determine the Ca2+ ion concentration (in M) and the hardness of your unknown water sample (in ppm CaCO3). Attach additional pages as needed. Part 1: Preparation of the EDTA SolutionStep 2: Calculate the mass (in g) of disodium elhylenediaminetetraacetale, NaCHO,N; 2H,0.requirad lo pepare a 100.0 m. solution with a concentration of 0.00800 M. Inclade hiscalculation on the Data and Calcalations page.Preparing the EDTA solution and calculating its concentration (sleps 3-7):2539220ma of boatand EDTA solule100.0 ml.mass of emptyweigh boatvolumetrie flaskPart 2: Performing a Blank Titration of the Eriochrome Black TIndicatorPreparing the blank analyte olution (steps 4-5)volume of DI water usod: 250 ml.volume of pH 10 buffer solution added: 50 ml.volume of 0.030 M MgC1, solution addel: 100 mil.amount of Eriochrome Black Tindicator: enough so that color of Mg-indicator complex is visibleCarrying out the blank titration and determining the blank volume (steps 6-7)blank solutioninitial buretfinal buretblank solution cadbefoee titrationvolume readingvolume readingpoint of titratioPart 3: Determination of the Hardnes of an Unknown Water SampleUnknowa water sample snalyaed: 1Preparing the unknowa water sample analyte solutions for cach trial (steps 2-3):volume of sample used: 250 ml.volume of pH 10 buffer solution sdided: S0 ml.volume of 0.030 M MgCl, solution added: 10D0 ml.amount of Eriochrome Black Tindicator: enough so that color of Mg-indicator complex is visible1020initial realingfor trial Ifinal readingfinal eadingfinal readingfor trial 3for trial 1for trial 2and initial readingfor trial 2and initial seadingfor trial 3

Hii there, As there are multiple question posted. we are answering first question. If you need…

Complete and turn in the Data and Calculations page for this experiment. Include calculations for the determination of the exact concentration of your group’s EDTA solution, and the Ca2+ ion concentration (in M) and the hardness (in ppm CaCO3) of your unknown water sample. Organize and label your calculations and report all measurements and calculations with the correct number of significant figures.

Complete and turn in the Data and Calculations page for this experiment. Include calculations for the determination of the exact concentration of your group’s EDTA solution, and the Ca2+ ion concentration (in M) and the hardness (in ppm CaCO3) of your unknown water sample. Organize and label your calculations and report all measurements and calculations with the correct number of significant figures.

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.34QAP

See similar textbooks

Similar questions

Calculate the mass of disodium EDTA (FW 372.25) needed to make 500-mL 0.015 M solution of EDTA. What is the equilibrium concentration of Y4- if the pH is (1) 7.00, and (2) 9.00?
Consider an F M solution of Fe2(SO4)3. Besides H+ and OH−, the known species are Fe3+, Fe(OH)2+, Fe(OH)2+, Fe2(OH)24+, FeSO4+, SO42−, and HSO4−. a) Write the charge balance equation for this solution. b) Which species must be an ion pair, and which comes from acid hydrolysis of Fe3+? Write the balanced acid hydrolysis reaction for the hexa-aquo complex of Fe3+ and report its pKa c) Write two mass balance equations for this solution, one for total iron and one for total sulfate. [How do you think you should handle the species that includes two iron atoms?] Give numerical values for these equations in terms of F.
A 0.9352g sample of ore containing Fe³+, Al³+ and Sr²+ was dissolved and made up to 500.00 mL. The analysis of metals was performed using complexation volumetry. Initially, an aliquot of 50.00 mL had its pH adjusted to 1.0 and titrated with a standard 0.03145 mol/L EDTA solution, requiring 6.95 mL to reach the end point. Subsequently, another 25.00 mL aliquot was buffered at pH=5 and titrated with the same EDTA solution, requiring 6.24 mL to reach the end point. Finally, a third aliquot of 25.00 mL was titrated at pH=11, requiring 11.10 mL of the same EDTA solution to complete the titration. Given the molar masses: Fe=55.845 g/mol; Al-26.982 g/mol and Sr-87.620 g/mol. a) Determine the percentage of each of the metals in the sample. b) Explain why the change in pH allows the determination of the three ions in this sample.
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…
A 20 ml aliquot of malonic acid solution was treated with 10.0 ml of 0.25M Ce4+ leading to the reaction CH2(COOH)2 + 6Ce4+ + 2H2O ® HCOOH + 2CO2 + 6Ce3+ + 6H+ After standing for 10 minutes at 60oC, the solution was cooled and the x’ss Ce4+ was titrated with 0.1M Fe2+, requiring 14.4 ml to reach the ferroin end point. Calculate the M of the malonic in the sample.
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.
When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80X 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?
A mixture containing only KCl and NaBr is analyzed by the Mohr method. A 0.2125- g sample is dissolved in 25 mL of water and titrated to the Ag2CrO4 end point, requiring 25.63 mL of 0.1110 M AgNO3. A blank titration requires 1.15 mL of titrant to reach the same end point. Report the %w/w KCl and NaBr in the sample.KCl = 74.551 NaBr = 102.89
To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.
Given that the Ksp for silver chloride is 1.76 x 10-10, and the Kf of silver(I) diammine cation [Ag(NH3)2 +] is 1.7 x 107, calculate the maximum number of grams of silver chloride that will dissolve in 250.0 mL of a 3.25 M solution of ammonia.
Given: You weigh out exactly 0.200 g of Fe(NH4)2(SO4)2·6H2O and dissolve it in the 100.00 mL volumetric flask. You then pipette 2.00 mL of this solution into the 50.00 mL volumetric flask to prepare the stock standard tris-bipyridyl-iron(II) solution. a. Calculate the molar concentration of iron(II) in this solution in the 50.00 mL volumetric flask. (The MW of Fe(NH4)2(SO4)2·6H2O is 392.14 g/mol) (answer a given the information above)