25. A 2L sample of mineral water was titrated with EDTA to determine its hardness in terms of ppm CaCO3. The EDTA solution was titratedusing 255 mg of primary standard CaCO3 requiring 31.85 mL for titration to the Calmagite endpoint. A 50 mL aliquot was titrated with 34.34mL EDTA. Determine the hardness of the sample.a. - COOHb. - SO3Hc. - NO2d. - NHCO26. A 6.881 g sample containing magnesium chloride (95.21) and sodium chloride (58.45) was dissolved in sufficient water to give 500 mL ofsolution. Analysis for the chloride content of a 50.0 mL aliquot resulted in the formation of 1.2501 gram AgCl (143.32). The magnesium in asecond 25 mL aliquot was precipitated as MgNH PO; on ignition, 0.1269 gram of Mg2P2O7 (222.57) was found. Calculate the percentage ofnon-chloride component in the sample.a. 33.1%b. 33.3%c. 33.5%d. 33.7%

Answered: 25. A 2L sample of mineral water was…

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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7. Sodium nitrite was assayed by residual titration with 0.1N potassium permanganate and 0.1 N oxalic acid. What is the gram-equivalent weight (gew) of sodium nitrite? (NaNO2=68.99g/mol) NaNO2+ KMnO4 +H2SO4 ® HNO3 + MnSO4 + Na2SO4 + K2SO4 + H2O KMnO4 + H2C2O4 + H2SO4 ® MnSO4 + K2SO4 + CO2 + H2O ㅋ
A 1.000 mL aliquot of a solution containing Cu²+ and Ni²+ is treated with 25.00 mL of a 0.04333 M EDTA solution. The solution is then back titrated with 0.02071 M Zn²+ solution at a pH of 5. A volume of 20.01 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 0.04333 M EDTA. This solution required 18.20 mL of 0.02071 M Zn²+ for back titration. The Ni²+ extracted from the column was treated witn 25.00 mL of 0.04333 M EDTA. How many milliliters of 0.02071 M Zn²+ is required for the back titration of the Ni²+ solution? volume: mL
2. Consider the titration of 25.00 mL of 0.08230 M KI with 0.05110 M AgNO3. Calculate pAg at the following volumes of added AgNO3. A) 39.00 mL; B) equivalence point and C) 44.30 mL. Ksp of Agl = 8.3 x 10-17 M.
A 1.000 ml. aliquot of a solution containing Cu?* and Ni* is treated with 25.00 ml, of a 0.03468 M EDTA solution. The solution is then back titrated with 0.02308 M Znt solution at a pH of 5. A volume of 20.28 ml. of the Zn+ solution was needed to reach the xylenol orange end point. A 2.000 ml. aliquot of the Cu* and Ni* solution is fed through an ion- exchange column that retains Ni*. The Cu+ that passed through the column is treated with 25.00 ml. of 0.03468 M EDTA. This solution required 23.18 ml. of 0.02308 M Zn* for back titration. The Ni" extracted from the column was treated witn 25.00 mL of 0.03468 M EDTA. How many milliliters of 0.02308 M Zn?* is required for the back titration of the NP solution? volume: ml.
COMPLEXOMETRIC TITRATION A deep well sample of 100 mL was titrated with 0.010 M EDTA at pH=10 (with Mg-EDTA-PH10 reagent) and consumed 31.95 mL using EBT indicator. Titration of another 100 mL of the same deep well sample with the same titrant but the pH was adjusted to 12.10 and murrexide as indicator consumed 24.25 ml to reach end point. Calculate: А. Total Hardness of water as CaCO3 В. ppm of Ca and Mg 76
The titration of an unknown weak acid with 0.10M NaOH is carried out and the pH at the equivalence point was found to be 8.50. Which indicator is best suited for the analyte? pKa=4.2 a. phenolphthalein pKa=9.7 b. methyl red pKa=5.0 c. methyl orange pKa=4.2 d. cresol purple pKa=8.3
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
Standard oxylate solution used to standardize KMnO4 was prepared by dissolving 3.299g of Na2C2O4 in 1.000L of water containing H2SO4. add 25mL aliquot of the Na2C2O4 solution required 28.39 mL of KMnO4 for titration. A blank titration of 25mL of water containing H2SO4 required 0.03 mL of KMnO4. what is the molarity of the KMnO4 solution? 5C2O42-+2MnO4-+16H+ → 10CO2+2Mn2++8H2O
11
Concerning EDTA titrations, which of the following is incorrect? 1. OEDTA forms 1:1 complexes with metal ions. 2. OThe most widely used indicators are murexide and Eriochrome Black T. 3. Oln presence of NaOH, EDTA reacts only with Mg2 ions, using murexide indicator. 4. OThe water hardness is usually expressed as CACO3 mg /L water. 5. OEDTA solution was standardized using Zinc Sulfate.
A 1.00 mL aliquot of a solution containing Cu and Ni is treated with 25.00 ml. of a 0.03468 M EDTA solution. The solution is then back titrated with 0.02308 M Zn+ solution at a pH of 5. A volume of 20.28 ml. of the Zn solution was needed to reach the xylenol orange end point. A 2.000 mL aliquot of the Cu* and Ni* solution is fed through an ion- exchange column that retains Ni?*. The Cu?+ that passed through the column is treated with 25.00 mL of 0.03468 M EDTA. This solution required 23.18 mL of 0.02308 M Zn* for back titration. The Ni extracted from the column was treated witn 25.00 mL of 0.03468 M EDTA. How many milliliters of 0.02308 M Zn+ is required for the back titration of the Ni solution? volume: ml.
Answer all of the f

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