The following data were obtained from the spectrophotometric titration of Cu(II) and Ca(II) in an unknown solution. A 25.00 mL aliquot of the unknown was taken to which 50.0 mL of ethanolamine buffer and 25.0 mL of distilled water were added. The solution was then titrated with standard 0.2508 M EDTA solution. Plot the recorded data, absorbance against volume of EDTA in mL. Correct the absorbance for volume changes. Calculate the number of moles of Ca(II) and Cu(II) in the unknown sample. Vol of Titrant, mL Vol of Titrant, mL Abs Abs
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- 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)Complexometric titrations are generally conducted to determine divalent cations. The most important applications are the titration of calcium and magnesium with EDTA. (a) A supplement tablet containing about 300.00 mg of calcium ion was dissolved, filtered, and diluted to 100.00 ml volume. Several 2.00 ml samples of the total solution were titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 13.65 mL. Calculate the calcium content of the supplement tablet in mg units. (b) A sample of Epsom Salt of mass 0.7567 g was dissolved uniformly in distilled water in a 250.00 mL volumetric flask. Portions of the magnesium ion solution of volume 10.00 mL were titrated using a 0.01000 M solution of EDTA. The mean corrected titration volume was 12.25 ml. Calculate the percentage by mass (% w / w) of the magnesium in the Epsom Salt sample. (c) A 100.00 mL sample of tap water was titrated with 0.0100 M EDTA solution. The mean corrected titration volume was 14.80 mL. Determine…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
- 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)Standard CaCO, is used to standardize the EDTA solution prior to titration. Suppose 0.385 g of CaCO, was dissolved and diluted to 250.0 ml. A 25.0 mL aliquot of this standard CaCO3 solution was then titrated to endpoint using 29.50 mL of the EDTA solution. Afterwards, the standardized EDTA solution was used to analyze the hardness of a 1000-ml water sample buffered at pH 10. The sample required 44.35 ml. of the EDTA solution to reach the endpoint. Determine the hardness of the sample in ppm CaCO3.Solutions of cobalt (II) ions have a magenta color with a molar absorptivity constant (e) value at 511 nm of 5.87 M-1cm-1. A 0.500 mL sample is transferred from a 50.0 mL stock solution of Co(NO3)2 and diluted with water to a final volume of 7.50 mL. The dilution had an absorbance value at 511 nm in a standard cuvette (1.00 cm light path) of 0.382. Calculate the mass of Co(NO3)2 contained in the original 50.0 mL stock solution.
- The standard curve was made by spectrophotographic analysis of equilibrated iron(III) thiocyanate solutions of known concentration. You are asked to analyze a Fe(SCN)2+Fe(SCN)2+ solution with an unknown concentration and an absorbance value of 0.4150.415 . The slope-intercept form of the equation of the line is ?=4558.4?+0.0147y=4558.4x+0.0147 . The unknown was analyzed on the same instrument as the standard curve solutions at the same temperature. What is the Fe3+Fe3+ concentration of the unknown solution?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. 7.42A standard solution contains 100 ppm of Fe, which was found to have an absorbance of 0.151 au at 508 nm after the addition of 1,10-phenanthroline, pH 4 buffer, and hydroxylamine. Then, a water sample treated similarly exhibited an absorbance of 0.109 au. Which of the following statements is true? (A) The Fe concentration of the water sample is higher than 100 ppm. B) The Fe concentration of the water sample is equal to 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. D) The Fe concentration of the water sample is lower than 100 ppm.
- 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 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)A 20.0 mL portion of a deep well water sample was diluted to 250.00 mL solution. A 50.0 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 100.0 mL containing 0.8622 mg primary standard calcium carbonate, CaCO₃ (FW=100.09 g/mol) 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.