A 49.10 mL aliquot from a 0.500 L solution that contains 0.530 g of MnSO4 (MW=151.00 g/mol) required 41.6 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 ( MW=100.09 g/mol) will react with 1.53 mL of the EDTA solution?
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A 49.10 mL aliquot from a 0.500 L solution that contains 0.530 g of MnSO4 (MW=151.00 g/mol) required 41.6 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 ( MW=100.09 g/mol) will react with 1.53 mL of the EDTA solution?
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- A sample of pure CaCO3 weighing 0.3677g is dissolved in hydrochloric acid and the solution diluted to 250.0ml in a volumetric flask. A 25.00ml aliquot requires 30.26ml of an EDTA solution for titration. Calculate a) the molarity of the EDTA solution; b) the number of grams Na2H2Y•2H2O (FW = 372.2) required to prepare 500.0ml of the solution.To adjust the EDTA solution, a 0.01 M 10 mL Ca+2 sample was taken and 10 mL of pH 10 buffer was added to it, and the volume was completed to 100 mL. Then, two drops of EBT indicators were added and titrated with EDTA. Since the consumption is 10.4 mL, which of the following is the concentration of the EDTA solution in terms of molarity? A. 0.0076B.0.0101C. 0.0096D.0.006750 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, what is the amount of magnesium in the sample in ppm?
- Given that the titration of Ca2+ and Mg2+ in a 50.00-mL sample of hard water required 22.35 mL of 0.01115 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate the Mg2+ as Mg(OH)2(s) . The supernatant liquid was titrated with 15.19 mL of the EDTA solution. Calculate the concentration in ppm of CaCO3 in the sample.A 0.4071-g sample of pure CaCO3 was transferred to a 500-mL volumetric flask, dissolved using a minimum of 6 M HCl, and diluted to volume. After transferring a 50.00-mL portion of this solution to a 250-mL Erlenmeyer flask, the pH was adjusted by adding 5 mL of a pH 10 buffer. After adding an indicator, the solution was titrated with the EDTA, requiring 42.63 mL to reach the end point. What is the concentration of EDTA? Choices: 0.0191 M, 0.0955 M, 0.00955 M, 0.477 MCalamine, which is used for relief of skin irritations, is a mixture of zinc and iron oxides. A 1.022-g sample of dried calamine was dissolved in acid and diluted to 250.0 mL. A 50.00 mL aliquot was suitably buffered and titrated with 2.40 mL of 0.002727 M ZnY-2 (Zn-EDTA) solution to allow the following reaction: Fe+3 + ZnY-2 → FeY- + Zn+2. Molecular mass: Fe2O3 = 165.74 a. The weight of sample in the aliquot portion is _________g ? b. the percentage composition of Fe2O3 in the sample is ______ % ?
- Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn at the equivalence point of the titration?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?The amount of calcium in physiologic fluids can be determined by a complexometric titration with EDTA. In one such analysis, a 0.100-mL sample of blood serum was made basic by adding 2 drops of NaOH and titrated with 0.00528 M EDTA, requiring 0.233 mL to reach the end point. Report the concentration of calcium in the sample as miligrams of Ca per 100 mL. (Ca = 40.078 amu).
- 50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, what is the value of magnesium in ppm in the sample?(Mg:24 g/mol)50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 g/mol) A. 378 B. 302 C. 214 D. 251Titration of 25.0 mL of a 0.0500 M Zn2+ solution with 0.0550 M EDTA in a solution buffered at pH 8. Assume that the temperature is 25 oC and that the formation constant for Zn2+ is 3.13 x 1016 at this temperature. What is the pZn of the solution after 30 mL of titrant have been added?
