Calcium in powdered milk is determined by ashing a 1.50 g sample and then titrating the calcium with EDTA solution, 12.10 mL being required. The EDTA was standardized by titrating 10.00 mL of a zinc solution prepared by dissolving 0.632 g zinc metal in acid and diluting to 1.00 liter (10.80 mL EDTA required for titration). What is the ppm concentration of Ca in the powdered milk?

Calcium in powdered milk is determined by ashing a 1.50 g sample and then titrating the calcium with EDTA solution, 12.10 mL being required. The EDTA was standardized by titrating 10.00 mL of a zinc solution prepared by dissolving 0.632 g zinc metal in acid and diluting to 1.00 liter (10.80 mL EDTA required for titration). What is the ppm concentration of Ca in the powdered milk?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions

Section4.9: Spectrophotometry

Problem 2.1ACP: Excess KI is added to a 100.0-mL sample of a soft drink that had been contaminated with bleach,...

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Calcium in powdered milk is determined by dry ashing a 1.50-g sample and then titrating the calcium with EDTA solution; 12.1 mL is required. The EDTA was standardized by titrating 10.0 mL of a zinc solution prepared by dissolving 0.632 g zinc metal in acid and diluting it to 1 L (10.8 mL EDTA required for titration). What is the concentration of calcium in the powdered milk in parts per million? is the correct answer 2.89 ppm?
Calcium in powdered milk is determined by dry ashing a 1.50-g sample and then titrating the calcium with EDTA solution; 12.1 mL is required. The EDTA was standardized by titrating 10.0 mL of a zinc solution prepared by dissolving 0.632 g zinc metal in acid and diluting it to 1 L (10.8 mL EDTA required for titration). What is the concentration of calcium in the powdered milk in parts per million?
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.
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. 251
A sample of pure CaCO3 weighing 0.2428g is dissolved in HCl and the solution diluted to 250ml in a volumetric flask. A 50.00ml aliquot requires 42.74ml of an EDTA solution for titration. A 200ml sample of water containing Ca+2 is titrated with 16.38ml of the EDTA solution. Calculate the degree of hardness of water in ppm CaCO3.
To determine the concentration of an EDTA solution, the following magnesium(II) solution is prepared: metallic magnesium (m(Mg) = 0.5915 g) is dissolved in dilute sulfuric acid, the resulting solution is poured into a volumetric flask with a volume of 0.250 L and is filled to the graduation mark with water. The titration of an aliquot of magnesium(II) solution with a volume of 25.00 ml consumes (11.11 ml; 11.32 ml; 11.24 ml; 11.29 ml) of EDTA. Calculate the concentration of EDTA solution with accuracy corresponding to the starting data, give confidence interval.
1) 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 CaC2O4 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 Mg2+ (24.305 g/mol) ions in the water? 2) 10 g of a solution, containing one or more of NaOH, Na3PO4, Na2HPO4, NaH2PO4, H3PO4 and HCl substances, is titrated with 1.0 M NaOH using the phenolphthalein indicator and 34.5 mL NaOH is used. Another 10 g mixture was titrated to reach the bromocresol green end point and 20.50 mL NaOH is used. What is the composition of the solution? What are the percentages of the species(H:1.0078, O:15.99, Na: 22.98, P:30.974, Cl:35.453)?
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 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, what is the amount of magnesium in the sample in ppm?
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 0.00376 M EDTA, requiring 0.135 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).
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