A deep well sample of 100 mL was titrated with 0.010M 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: A) Total hardness of water as CaCO3 B) ppm of Ca and Mg

A deep well sample of 100 mL was titrated with 0.010M 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: A) Total hardness of water as CaCO3 B) ppm of Ca and Mg

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter20: Applications Of Oxidation/reduction Titrations

Section: Chapter Questions

Problem 20.29QAP

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10mL of a 10% by weight MgCl2 solution (density = 1.1 g / mL) is precipitated as magnesium ammonium phosphate after necessary processes, filtered and washed. The precipitate is dissolved in 50mL 1M HCl and excess acid is titrated with 2.0M NaOH solution in the presence of methyl orange. Find the NaOH consumption (Mg = 24,3g / mol, Cl = 35,5g / mol)
One of the tests she conducted was EDTA titration to determine the hardness of the water. For this experiment, two 150.0 mL samples were utilized. The first sample required 7.45 mL of 0.02055 M EDTA titrant to reach the endpoint at a pH of 10.00. The second sample was titrated at pH = 13.0 to precipitate Mg(OH)2, and 5.55 mL of the same titrant was used to attain the endpoint. (MW: Ca = 40.08 g/mol, Mg = 24.31 g/mol, CaCO3 = 100.087 g/mol, MgCO3 = 84.314 g/mol) What is the total hardness of the water? What is concentration of Ca & Mg in the water sample? Express the answer in ppm.
Double indicator titration of 1.000g powdered sample containing either alone or any compatible mixture of NaOH/Na2CO3/NaHCO3 and the rest are inert components. The sample was dissolved in 20 ml water then titrated with 0.50 M HCl and reach phenolphthalein endpoint at burette volume of 25.55 ml. Continuing titration, it reached methyl orange endpoint at burette volume of 9.45 ml. Calculate the percentage mass of the possible alkaline component/s.
A deep well sample of 100 mL was titrated with 0.010 M EDTA at pH=10 (with Mg-EDTA-pH 10 reagent) and consumed 30.15 mL using EBT indicator. Titration of another 100 mL of the same deep well sample with same titrant but the pH was adjusted to 12.10 and murrexide as indicator consumed 24.25 to reach end point. Calculate: a. Total hardness of water as CaCO3 b. ppm of Ca and Mg
A sample containing NaOH only was titrated with standard 0.1280 M HCl, requiring 25.45 mL to reach a point beyond the endpoint. To compensate for this, the sample was back titrated with 0.1030 M NaOH solution, requiring 0.35 mL to reach the desired endpoint. If 9.00 mL of the sample was used for titration, calculate % (w/v) NaOH in the sample
The following experimental process steps have been made to determine the hardness of water. Accordingly, 100 mL sample was acidified with a few drops of 6 M HCl and boiled for a while to remove the CO2 in it. Then add a few drops of methyl red (pH: 4.2-6.3) to the cooled sample and neutralize the solution with 0.1M NaOH, then add 2 ml of 0.01M pH10 buffer and 4-5 drops on it. EBT indicator was added and the solution was titrated with 0.0086M EDTA until the color turned blue. Since the consumption of titrant is 11.44mL, calculate the amount of Ca in the water in terms of mg CaCO3. (Ca: 40, C: 12, 0:16)
A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. a) Assume all of the Ca2+ in the water comes from CaCO3. How many moles of CaCO3 are in 1 L of water? How many grams of CaCO3 are in 1 L of water? c) If 1 ppm CaCO3 = 1 mg/liter, what is the water hardness in ppm CaCO3 ?
A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. a) What volume of EDTA is used in titrating the Ca2+ in the hard water? b) How many moles of EDTA are there in that volume? c) How many moles of Ca2+ are in 100 mL of water?
A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. A 100-mL sample of hard water is titrated with 22.4 mL of the EDTA solution created above. The same amount of MgCl2 is added as previously and the total volume of EDTA solution required is 22.44 mL. How many moles of Ca2+ are in 100 mL of water?
A 0.512 g sample of CaCO3 is dissolved in 12 M HCl and the mixture is diluted to 250 mL. A small amount of MgCl2 solution is added to a 25 mL aliquot of the solution., and the mixture is titrated with (ethylenediaminetetraacetic acid) EDTA to the Eriachrome Black T (with MgCl2 is used as indicator) end point. The mixed solution requires 28.55 mL of the EDTA solution to reach the end point. A similar amount of MgCl2 solution requires 2.60 mL to reach the endpoint. How many milliliters of EDTA are needed to titrate the Ca2+ ion in the sample? How many moles of EDTA are there in the volume calculated for the question above? What is the molarity of the EDTA solution?
A Fajans titration of a 0.7908-g sample required 45.32 mL of 0.1046 M AgNO3 . Express the results of this analysis in terms of the percentage of BaCl2 * H2O. (Use a MW value in 4 decimal places)
Solve and write the complete solution: 1. A 100.0 ml sample of drinking water was buffered at pH 10.0 and after addition of calmagite indicator, required 38.41 ml of 4.652 x 10-3 M EDTA for titration. Calculate the total hardness of water as indicated a.) ppm CaCO3 b.) ppm CaO