A water sample was tested for hardness. To titrate Ca2* and Mg2+, a 25.00-mL sample needed 7.39 ml of 0.00964 M EDTA. Another 25.00-mL aliquot was mixed with sufficient NaOH to precipitate out Mg2* as Mg(OH)216). Titration of the clear supernatant liquid required 4.54 mL of the same standard EDTA solution. FW: CaCO3 = 100.09, Mg = 84.31, Ca = 40.078 %3D (Report answers in 3 SF.) a. Calculate the concentration of CaCO3 (FW=100.09) in the sample in ppm. ppm a. Calculate the concentration of MgCO3 (FW=84.31) in the sample in ppm. ppm

A water sample was tested for hardness. To titrate Ca2* and Mg2+, a 25.00-mL sample needed 7.39 ml of 0.00964 M EDTA. Another 25.00-mL aliquot was mixed with sufficient NaOH to precipitate out Mg2* as Mg(OH)216). Titration of the clear supernatant liquid required 4.54 mL of the same standard EDTA solution. FW: CaCO3 = 100.09, Mg = 84.31, Ca = 40.078 %3D (Report answers in 3 SF.) a. Calculate the concentration of CaCO3 (FW=100.09) in the sample in ppm. ppm a. Calculate the concentration of MgCO3 (FW=84.31) in the sample in ppm. ppm

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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Calcium in powdered milk is determined by dry ashing a 1.46g sample and then titrating the calcium with EDTA solution, 12.1mL being required. The EDTA was standardized by titrating 10.4mL of a Zn solution prepared by dissolving 0.634g Zn metal in acid and diluting to 1L (10.83mL EDTA required for titration). What is the concentration (ppm) of calcium in the powdered milk?
Calculate PCa of the solution that results when 50.0 mL of 0.0050 M Ca2+ is titrated with 25.00 mL of 0.0100 M EDTA in a solution buffered to a conastant pH of 10.00.
A 100.0 mL drinking water containing Ca2+ was treated with ammonia-ammonium chloride buffer solution to give pH about 10.0. Calgamite indicator was added and the solution was titrated with 0.0050 M EDTA. It required 23.50 mL of the titrant to achieve the end point. Calculate the water hardness?
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 B/mol)
An unknown solution containing 25.00 mL of Ni2+ in dilute HCl is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn2+, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2+ in the unknown solution?
Calcium is determined in serum by microtitration with EDTA. A 100-μL sample is treated with two drops of 2 M KOH, Cal-Red indicator is added, and the titration is performed with 0.00122 M EDTA, using a microburet. If 0.203 mL EDTA is required for titration, what is the level of calcium in the serum in mg/dL?
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).
2. 100 mL tap water is titrated with 20 mL of 0.02 M EDTA solution to determine the hardness of the water. The second 100 mL tap water is precipitated as CaC204 and removed by filtration and the filtrate is titrated with 8.0 mL of the same EDTA solution. What are the concentrations (as ppm) of Ca²* (40.078 g/mol) and Mg* (24.305 g/mol) ions in the water?