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

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

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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I need to complete concentration of EDTA
CHM-202 Lab 4 Calcium ion Rev 1 G6-2022 Preparation of EDTA solution (show calculations below) 250mL of 2.5 X 103m m= n/ m 0.0025m= 250 ML n = 0.625 mmides = on = 0.625 x 10²³ moles Grams of EDTA Required Mass of EDTA [2.61 Analytical Balance 182.3 Moles of EDTA 10.000 625 Mass of water in solution Molarity Molality miligram. Mole Fraction Percentage (m/v) 292.24 MWEota g/mol 0.182 105. Tare Weight Mass of Solution [2.4, 2.7] Top Loading Balance 102.04 mg 5/8 Gross Weight 351.520 249 2977 Concentration of EDTA [2.8] Use both correct units and significant figures mg. Net Weight 249 480 mg.
Transcribed Image Text:CHM-202 Lab 4 Calcium ion Rev 1 G6-2022 Preparation of EDTA solution (show calculations below) 250mL of 2.5 X 103m m= n/ m 0.0025m= 250 ML n = 0.625 mmides = on = 0.625 x 10²³ moles Grams of EDTA Required Mass of EDTA [2.61 Analytical Balance 182.3 Moles of EDTA 10.000 625 Mass of water in solution Molarity Molality miligram. Mole Fraction Percentage (m/v) 292.24 MWEota g/mol 0.182 105. Tare Weight Mass of Solution [2.4, 2.7] Top Loading Balance 102.04 mg 5/8 Gross Weight 351.520 249 2977 Concentration of EDTA [2.8] Use both correct units and significant figures mg. Net Weight 249 480 mg.
3.1 3.2 3.3 3.4 2.2 2.3 2.1 2.4 2.7 2.8 2.5 2.6 CHM-202 Lab 4 Calcium ion Rev 1 G6-2022 command T option You 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 flask Solution specifications: 3) An analytical balance, weighing paper, top-loading balance 4) Distilled water 3/8 250 mL of 2.5 x 10 M EDTA solution Solution 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 balance which can measure up to 400 grams (contact your instructor if the balances with this capacity are clearly identified). Weigh out the required amount of EDTA on the analytical balance recording gross and tare weight to within 0.1 mg. Transfer this amount to the 250 mL volumetric flask and combine with 10 mL of ammonia pH 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 this take a clean dry test tube and add 1.0 mL of ammonia buffer and 10 drops of the Mg-EDTA solution. To this sample add a few drops of Eriochrome Black T (EBT) indicator. Add 1.0 mL of one of the commercial water samples on the list of hard (high calcium concentration) water. You should observe a pink or purple solution 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 with distilled 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 the solution on the top-loading balance (with the cap on) and record this mass to the appropriate number of significant figures. Calculate the concentration of the EDTA solution in molarity to the appropriate number of significant figures. 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 calculation purposes. Using the EDTA solution that you prepared in part 2 add the EDTA solution to the test tube drop wise with some stirring. As you add the EDTA solution you should see a color change from the original pink color to a definite blue color. Note that the transition between pink and blue may not be as obvious as was observed in a typical acid-base titration using phenolphthalein. Once a blue solution has been obtained add more of the commercial water sample until the pink color returns. Repeat 3.2 more carefully to observe the transition of the EBT indicator as it turns from pink to blue.
Transcribed Image Text:3.1 3.2 3.3 3.4 2.2 2.3 2.1 2.4 2.7 2.8 2.5 2.6 CHM-202 Lab 4 Calcium ion Rev 1 G6-2022 command T option You 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 flask Solution specifications: 3) An analytical balance, weighing paper, top-loading balance 4) Distilled water 3/8 250 mL of 2.5 x 10 M EDTA solution Solution 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 balance which can measure up to 400 grams (contact your instructor if the balances with this capacity are clearly identified). Weigh out the required amount of EDTA on the analytical balance recording gross and tare weight to within 0.1 mg. Transfer this amount to the 250 mL volumetric flask and combine with 10 mL of ammonia pH 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 this take a clean dry test tube and add 1.0 mL of ammonia buffer and 10 drops of the Mg-EDTA solution. To this sample add a few drops of Eriochrome Black T (EBT) indicator. Add 1.0 mL of one of the commercial water samples on the list of hard (high calcium concentration) water. You should observe a pink or purple solution 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 with distilled 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 the solution on the top-loading balance (with the cap on) and record this mass to the appropriate number of significant figures. Calculate the concentration of the EDTA solution in molarity to the appropriate number of significant figures. 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 calculation purposes. Using the EDTA solution that you prepared in part 2 add the EDTA solution to the test tube drop wise with some stirring. As you add the EDTA solution you should see a color change from the original pink color to a definite blue color. Note that the transition between pink and blue may not be as obvious as was observed in a typical acid-base titration using phenolphthalein. Once a blue solution has been obtained add more of the commercial water sample until the pink color returns. Repeat 3.2 more carefully to observe the transition of the EBT indicator as it turns from pink to blue.
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