EBTA TItration Q3. A 1. volumetric flask. A 50.00-ml aliquot of the diluted solution was brought...
a 25.0 ml aliquot of vinegar was diluted to 250 ml in volumetric flask. Titration of 50.0 ml aliquots of diluted solution required an average of 34.88 ml of 0.09600 M NaOH. Express the acidity of the vinegar in terms of percentage (w/v) of acetic acid.
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
A 24-hr urine specimen was diluted to exactly 2.000 L in a volumetric flask. The Ca^2+ and Mg^2+ in a 100.0-mL aliquot of the diluted solution required 20.81 mL of 0.00830 M EDTA, after being buffered to a pH of 10.0. The Ca^2+ second 100.0-mL aliquot was precipitated as CaC_2O_4(s), which was filtered and washed. The filtrate and washings were titrated with 5.98 mL of the EDTA solution. Calculate the milligrams of Ca^2+ and Mg^2+ in the 24-hr sample.
Chromel is an alloy composed of nickel, iron, and chromium. A 0.6445-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.23-mL back-titration with 0.06139 M copper(II) was required. The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 38.95 mL of 0.05173 M EDTA....
A 0.4505 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO2⋅4H2Oand removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 15.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 35.10 mL of 0.001497 M EDTA. Thiosulfate was used to mask the copper in a second 20.00 mL aliquot. Titration of the...
Please help. I will rate! A 0.4721 g sample of pewter, containing tin, lead, copper, and zinc, was dissolved in acid. Tin was precipitated as SnO 4 H,O and removed by filtration. The resulting filtrate and washings were diluted to a total volume of 250.0 mL. A 15.00 mL aliquot of this solution was buffered, and titration of the lead, copper, and zinc in solution required 34.45 mL of 0.001518 M EDTA. Thiosulfate was used to mask the copper in...
A 50.00 mL aliquot from a 0.490 L solution that contains 0.470 g of MnSO4 ( MW=151.00 g/mol) required 38.0 mL of an EDTA solution to reach the end point in a titration. What mass, in milligrams, of CaCO3 ( MW=100.09 g/mol) will react with 1.00 mL of the EDTA solution? mass: mg
A 0.6004 g sample of Ni/Cu condenser tubing was dissolved in acid and diluted to 100.0 mL via a volumetric flask. Titration of both cations in a 25.00 mL aliquot of this solution required 45.81 mL of 0.05285 M EDTA. Mercaptoacetic acid and NH3 were then introduced; production of the Cu complex with the former resulted in the release of an equivalent amount of EDTA, which required a 22.85 mL titration with 0.07238 M Mg2+. Calculate the percentages of Cu...
Mass of antacid in sample: 1.5558 g Antacid tablet: 1.6010 g Composition of antacid: Aluminum hydroxide: 160 mg Magnesium carbonate: 105 mg Protocol A: Pipet a 10.00 mL aliquot of the antacid sample solution into a 125 mL Erlenmeyer flask followed by adding about 10 mL of the bicarbonate-carbonate buffer solution (pH 10.0 ± 0.1). Transfer quantitatively a 34.96 mL aliquot of standard EDTA solutioN, 0.01000 M, to the flask using a buret. Boil gently the mixture for 5 min....
An unknown solution was analyzed for Ni by an EDTA titration. A 50.00 mL sample of the unknown was treated with 25.00 mL of 0.2404 M EDTA. The excess EDTA was then back titrated with 8.52 mL of 0.0694 M Zn2+ to reach the equivalence point. What was the concentration of Ni (in unit of M) in the 50.00 mL sample? Please keep your answer to three decimal places.