To standardize EDTA solution, three independent titrations were conducted,cach with 20 mL of 0.01 (N) hard water. The average volumes of EDTAconsumed at the end point of the titrations was 23.3 mL respectively.The same EDTA solution was used to determine the hardness of your hostelwater. In each of the three independent experiments, 60 mL of your hostelwater was used. The average volume of EDTA solution consumed in thethree titrations is 24.9 mL. The hardness of your hotel water in terms ofCACO3 is: Anhydrous CuO4S is white in color, but a solution of coper (II) sulphateturns blue. Which of the following statements is/are true for thisobservation?(i) It forms a hydrated compound, thus regaining its color(ii) The color is due to metal-to-ligand charge transfer transition(iii) The octahedral aquo-complex gives rise to Laporte relaxed d-dtransition(iv)The octahedral aquo-complex gives rise to spin- allowed & Laporte-allowed LMCT transition(v) The tetrahedral aquo-complex gives rise to Laporte allowed d-dtransition.Options:(a) (i) & (iii)(b) (ii) & (iv)(c) (ii)(d) (v)(e) (iv)

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To standardize EDTA solution, three independent titrations were conducted, each with 20 mL of 0.01 (N) hard water. The average volumes of EDTA consumed at the end point of the titrations was 23.3 mL respectively. The same EDTA solution was used to determine the hardness of your hostel water. In each of the three independent experiments, 60 mL of your hostel water was used. The average volume of EDTA solution consumed in the three titrations is 24.9 mL. The hardness of your hotel water in terms of CACO3 is:

To standardize EDTA solution, three independent titrations were conducted, each with 20 mL of 0.01 (N) hard water. The average volumes of EDTA consumed at the end point of the titrations was 23.3 mL respectively. The same EDTA solution was used to determine the hardness of your hostel water. In each of the three independent experiments, 60 mL of your hostel water was used. The average volume of EDTA solution consumed in the three titrations is 24.9 mL. The hardness of your hotel water in terms of CACO3 is:

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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A 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? The Fe concentration of the water sample is higher than 100 ppm. It is impossible to estimate the Fe content of the water sample from information presented. The Fe concentration of the water sample is lower than 100 ppm. The Fe concentration of the water sample is equal to 100 ppm.
A 1.000 mL aliquot of a solution containing Cu²+ and Ni²+ is treated with 25.00 mL of a 0.03703 M EDTA solution. The solution is then back titrated with 0.02138 M Zn²+ solution at a pH of 5. A volume of 22.13 mL of the Zn²+ solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu²+ and Ni²+ solution is fed through an ion-exchange column that retains Ni²+. The Cu²+ that passed through the column is treated with 25.00 mL of 0.03703 M EDTA. This solution required 18.53 mL of 0.02138 M Zn²+ for back titration. The Ni²+ extracted from the column was treated witn 25.00 mL of 0.03703 M EDTA. How many milliliters of 0.02138 M Zn²+ is required for the back titration of the Ni²+ solution? volume: mL
What is the mass of pure dry CaCO3 (MW: 100.0869 g/mol) standard used in the standardization of EDTA solution? Assume that 1.758 M EDTA solution was computed based on the titration of CaCO3 standard. The volume of titrant needed to reach the endpoint was 35.00 mL. Ca2+ + Y4- → CaY2- 0.1500 g 5.630 g 6.158 g 0.6158 g
The calcium content of a milk sample was to be determined by EDTA titration. A sample weighing 0.206 g was mixed with an aqueous buffer at pH 11.5. A few drops of EBT indicator were added and the solution required 24.25 mL of 1.538 x 10-2 M EDTA to reach the endpoint. Calculate the weight percent of calcium (FW =40) in the milk.
A solution containing 60 mL of a 0.025 mol / L metal ion (Mn +) buffer buffered to pH 7.0 was titrated with a 0.05 mol / L EDTA solution. Data: Conditional formation constant (Kf)=10^15. Determine: i) The concentration of the free metal when ½ of the equivalence volume is added. ii) the concentration of free metal in the equivalence volume. iii) the concentration of free metal with an excess of 2 mL of EDTA? (Data - EDTA constants: K1=0.01; K2=2.19.10^-3; K3=6.92.10^-7; K4=5.75.10^-11)