I need to complete concentration of EDTA CHM-202 Lab 4 Calcium ion Rev 1 G6-2022Preparation of EDTA solution (show calculations below)250mL of 2.5 X 103mm= n/m 0.0025m=250 MLn = 0.625 mmides = on = 0.625 x 10²³ molesGrams of EDTA RequiredMass of EDTA [2.61Analytical Balance182.3Moles of EDTA10.000 625Mass of water in solutionMolarityMolalitymiligram.Mole FractionPercentage (m/v)292.24MWEota g/mol0.182 105.TareWeightMass of Solution [2.4, 2.7]Top Loading Balance102.04 mg5/8GrossWeight 351.520249 2977Concentration of EDTA [2.8] Use both correct units and significant figuresmg.NetWeight 249 480 mg. 3.13.23.33.42.22.32.12.42.72.82.52.6CHM-202 Lab 4 Calcium ion Rev 1 G6-2022commandToptionYou will need the following materials to prepare an EDTA solution of known concentration:1) Solid EDTA (Formula weight of EDTA: 292.24 g/mol).2) A 250 mL volumetric flaskSolution specifications:3) An analytical balance, weighing paper, top-loading balance4) Distilled water3/8250 mL of 2.5 x 10 M EDTA solutionSolution concentration should be reported to the appropriate number of significant figures.Calculate the required amount of EDTA needed to fulfill the solution specifications.Record the mass of your empty 250 mL volumetric flask with stopper or cap on using a top-loading balancewhich can measure up to 400 grams (contact your instructor if the balances with this capacity are clearlyidentified).Weigh out the required amount of EDTA on the analytical balance recording gross and tare weight towithin 0.1 mg. Transfer this amount to the 250 mL volumetric flask and combine with 10 mL of ammoniapH 10 buffer (this can be an approximate volume transferred with a graduated cylinder)3. Qualitative examination of titration reaction.You will examine the titration reaction in a qualitative manner prior to running the titrations. To do thistake a clean dry test tube and add 1.0 mL of ammonia buffer and 10 drops of the Mg-EDTA solution. Tothis sample add a few drops of Eriochrome Black T (EBT) indicator. Add 1.0 mL of one of the commercialwater samples on the list of hard (high calcium concentration) water. You should observe a pink or purplesolution after the addition of the indicator and water sample.Add 150-200 mL of distilled water and stir the solution until all of the EDTA has dissolved. Fill withdistilled water until the meniscus of the solution is even with the mark in the neck of the volumetric flask.Shake the solution with the cap on until uniform. Record the mass of the volumetric flask containing thesolution on the top-loading balance (with the cap on) and record this mass to the appropriate number ofsignificant figures.Calculate the concentration of the EDTA solution in molarity to the appropriate number of significantfigures. Using the other data recorded report the concentration of EDTA in the following units: molality,mole fraction and percentage (m/v). You can assume that the buffer added is pure water for calculationpurposes.Using the EDTA solution that you prepared in part 2 add the EDTA solution to the test tube drop wise withsome stirring. As you add the EDTA solution you should see a color change from the original pink color toa definite blue color. Note that the transition between pink and blue may not be as obvious as was observedin a typical acid-base titration using phenolphthalein.Once a blue solution has been obtained add more of the commercial water sample until the pink colorreturns.Repeat 3.2 more carefully to observe the transition of the EBT indicator as it turns from pink to blue.

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Molarity is defined as number of gram moles of a solute in one litre solution.
M = nV (L) = w (g)MW…

Molarity Molality Concentration of EDTA [2.8 Mole Fraction Percentage (m/v)