A 21.524 g paint sample was analyzed for barium (Ba2+, MW = 137.327 g/mole) by an EDTA back titration: Ba2+(aq) + Y4–(aq) à BaY2–(aq). The sample was dissolved in acid and sufficient water was added to produce a volume of 100 mL. 10.00 mL of this concentrated solution was diluted to a volume of 50.00 mL. 25.00 mL of the diluted solution was treated with 33.95 mL of excess 0.09456 M EDTA. The excess EDTA was titrated to the endpoint with 11.04 mL of 0.07238 M Zn2+ by Zn2+(aq) + Y4–(aq) à ZnY2–(aq).
a. Use the results of the back-titration to calculate [Ba2+] in the diluted solution.
b. Calculate [Ba2+] in the concentrated solution.
c. Calculate the total moles of Ba in the sample.
d. Calculate the total mass of Ba in the sample.
e. If the barium in the sample is present as barium oxide (BaO, MW = 153.33 g/mole), calculate the mass of BaO in the sample.
f. Calculate the percentage of BaO in the sample.
A 21.524 g paint sample was analyzed for barium (Ba2+, MW = 137.327 g/mole) by an...
A sample of 0.7360 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2CO3. If the mass of the BaCO3 precipitate formed is 0.7578 g, what is the percent by mass of Ba in the original unknown compound?
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.
4) A sample of 0.870 g of an unknown compound containing barium ions (Ba2+) is dissolved in water and treated with an excess of Na2SO4. If the mass of the BaSO4 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
4) A sample of 0.670 g of an unknown compound containing barium ions (Ba2*) is dissolved in water and treated with an excess of NA2SO4. If the mass of the BaS04 precipitate formed is 0.4105 g, what is the percent by mass of Ba in the original compound?
Calculate the mass of EDTA (C10H12CaNNa2Os: MW=374.20 g/mole) needed to prepare a 100- mL of 0.0100M EDTA solution. (Show your work)
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 15.00 mL sample of nitric acid, HNO3, requires 0.655 g of barium hydroxide, Ba(OH)2 for titration to the equivalence point. What is the concentration of the nitric acid? 2 HNO3(aq) + Ba(OH)2(aq) → Ba(NO3)2(aq) + 2 H2O(l)
Calculate the concentration of a barium hydroxide solution if it takes 35.42 mL of a 0.1042 M solution of phosphoric acid to reach the endpoint of titration for a 25.00 mL sample of the barium hydroxide solution 3 Ba(OH)2 (aq) + 2 H3PO4 (aq) 6H20 (1) + Baz(PO4)2 (aq) Express your answer in molarity. Do not include the units.
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...
A 5.0067 g sample of Na2CrO4 (MW = 161.97 g/mol) is dissolved in 250.0 mL of water. Assume the solution has a density of 1.00 g/mL. A 50.0 mL aliquot of the solution is then diluted to a final volume of 250.0 mL. What is the concentration of Na+ in the diluted solution in units of parts per million (ppm)?