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 & 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 3.1ACP

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2. Titration of Ca²+ and Mg²+ in a 50mL sample of hard water required 23.65mL of 0.01205M EDTA. A second 50mL aliquot was made strongly basic with NaOH to precipitate Mg2+ as Mg(OH)2. The supernatant liquid was titrated with 14.53mL of the EDTA solution. Calculate a. concentration in ppm of CaCO3 in the sample. b. concentration in ppm of MgCO3 in the sample.
a. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. b. A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 12 and consumed 31 mL. Calculate the Calcium content of the water sample in mg/L.
Titration of Ca2+ and Mg2+ in a 50.00 mL sample of hard water required 23.65 mL of 0.01205 M EDTA. A second 50.00 mL aliquot was made strongly basic with NaOH to precipitate Mg2+ as Mg(OH)2 , filtered, and titrated with 14.53 mL of same EDTA solution. Calculate the ff: a.)The total hardness of water sample. b.)Concentration in ppm CaCO3 in the sample. c.)Concentration in ppm MgCO3 in the sample
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
Volhard titration. A 30.00-mL solution of unknown I2 was treated with 50.00 mL of 0.365 0 M AgNO3. The precipitated AgI was filtered off, and the filtrate (plus Fe31) was titrated with 0.287 0 M KSCN. When 37.60 mL had been added, the solution turned red. How many milligrams of I2 were present in the original solution?
Titration of Ca 2+ and Mg 2+ in a 50.00 ml sample required 25.50 mL Of 0.01115 M EDTA. A second 50 ml aliquot was made strongly basic with NaOH to precipitate the Mg 2+ as Mg(OH) 2(s). The supernatant liquid was titrated with 16.19 mL of the EDTA solution. Calculate the concetration in ppm of CaCO 3 in the sample О а. 100 O b.568.65 О с. 361.04 O d. 207.61
A 25.00 ml of Ni2* solution was diluted in HCI and treated with 25.00 ml of 0.05283 M NazEDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2* at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown. Ans. 0.03664 M
5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
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.
A water was tested for water hardness. A 50.00 mL aliquot was prepared and buffered to pH 10.0, it required 23.55 mL of 0.0250 M EDTA. A second aliquot, prepared with NaOH, was titrated with 14.53 mL of the same EDTA titrant. Calculate the total hardness of the water (expressed in ppm CaCO₃). a. 727.2 ppm b. 1179 ppm c. Insufficient data d. 380.2 ppm Calculate the calcium hardness of the water (expressed in ppm CaCO₃). a. Insufficient data b. 1179 ppm c. 727.2 ppm d. 380.2 ppm Calculate the magnesium hardness of the water (expressed in ppm MgCO₃) a. 727.2 ppm b. Insufficient data c. 380.2 ppm d. 1179 ppm
A deepwell water sample of 100 mL was titrated with 0.010 M EDTA at pH 10 ( with Mg-EDTA pH 10 buffer reagent) and consumed 31 mL. Calculate the Total Hardness of the water sample as mg CaCO3. Ans in 3 sig figures. no need to write the unit.

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