4. A standard solution of EDTA (0.100 M) is being used to titrate 25.00 mL of a 0.1O M Zn? solution (buffered at pH 8.0). Calculate the value of pZn2: a) before the addition of EDTA solution b) after the addition of 10.00 mL of EDTA solution c) at volume V = } Ver (Veq = volume at equivalence point) d) at volume = Veg (at the equivalence point) e) at volume V = 2,0 Veg

4. A standard solution of EDTA (0.100 M) is being used to titrate 25.00 mL of a 0.1O M Zn? solution (buffered at pH 8.0). Calculate the value of pZn2: a) before the addition of EDTA solution b) after the addition of 10.00 mL of EDTA solution c) at volume V = } Ver (Veq = volume at equivalence point) d) at volume = Veg (at the equivalence point) e) at volume V = 2,0 Veg

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.28QAP

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A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg2 is added as previously, and the volume of EDTA required is 31.84 mL. a. What volume of EDTA is used in titrating the Ca2 in the hard water? _____________mL b. How many moles of EDTA are there in that volume? _____________ moles c. How many moles of Ca2 are there in the 100 mL of water? _____________ moles d. If the Ca2 comes from CaCO3, how many moles of CaCO3 are there in one liter of the water? How many grams of CaCO3 are present per liter of the water? _____________ mol / L _____________ g / L e. If 1 ppm CaCO3 = 1 mg per liter, what is the water hardness in ppm CaCO3? _____________ ppm CaCO3
For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. What is the value of the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol)
For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g, necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 27.4mL of 0.0097 M EDTA solution. Calculate the amount of calcium in the sample in terms of% CaCO3. (Ca = 40 g / mol, CaCO3 = 100g / mol)
For complexometric titration of Ca (II) ions in the shell of an egg sample weighing 59,427 g, the necessary processes were applied to the egg shells and a sample of 100 mL was prepared. From the prepared sample, 1 mL was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dripped on it. The prepared solution was titrated with 27.4 mL of EDTA solution set at 0.0097 M. Calculate the amount of calcium in the sample in CaCO3%. (Ca = 40g / mol, CaCO3= 100g / mol)
Chemistry A 20 mL solution containing both Ca2+ and Mg2+ cations is diluted in to 100 mL. When 10 mL of this solution is taken and titrated with 0.05 M EDTA at pH = 10 in the presence of Erio – T indicator, the consumption is found as 12 mL. A new 10 mL was taken from the same solution and (NH4)2C2O4 is added on it and then formed the precipitate is filtered. The filtered solution is titrated with the same EDTA solution and the consumption is found as 3 mL. So find the Ca2+ and Mg2+ amounts in the main sample solution in terms of mg/L.
For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 23.6 mL of 0.0095 M EDTA solution. Which of the following is the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol) A. 5.83B. 10.96C. 3.58D. 7.42
For the complexometric titration of Ca (II) ions in the shell of the egg sample weighing 59.427 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL was taken from the prepared sample, diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The solution prepared was titrated with 27.4mL of 0.0097 M EDTA solution. Calculate the amount of calcium in the sample in terms of% CaCO3. (Ca = 40 g / mol, CaCO3 = 100g / mol) A. 4.47 B. 8.95 C. 3.58 D. 5.83
A 0.4071-g sample of CaCO3 (MM: 100.09 g/mole) is transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. A 50.00-mL aliqout of this solution was mixed with 5 mL of a pH 10 NH3-NH4Cl buffer that contains a small amount of Mg2+--EDTA to adjust the pH to 10. After adding calmagite as an indicator, the solution is titrated with the EDTA, requiring 42.63 mL to reach the end point. Report the molar concentration of EDTA in the titrant. 9.543 x 10-3 M 5.748 x 10-3 M 3.266 x 10-4 M 1.018 x 10-4 M
For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62.576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. Which of the following is the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol)
In order to adjust the EDTA solution, 10 mL of 0.01M Ca + 2 sample was taken and 10 mL of pH 10 buffer was added on it and it was completed to 100 mL. Then, two drops of EBT indicator were added and titrated with EDTA. Since the consumption is 13 mL, what is the concentration of EDTA solution in terms of molarity?
A 100 mL sample of drinking water was buffered at pH 10 and after a ddition of Eriochrome Black T required 1 1 mL of 0.00499 M EDTA for titration. Identify the color at the end point.
a 20 ml portion of a deep well water sample was diluted to 250 ml solution. a 50 ml aliquot of this diluted sample water was buffered at ph 10 and required 8. 50 ml of a standard EDTA.the titrant was standardized using 100ml containing 0.8622 mg primary standard calcium carbonate , which required 15.45 ml for titration.(a) identify a possible indicator and its endpoint color (b) calculate the molarity of the EDTA solution. (c) calculate the total hardness of the water as ppm CaCO3 (d) identify the quality of the water sample in terms of hardness