A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4 (233.39). How many grams of barium ion (137.33) are in a 458-mg sample of the barium compound if a solution of the sample gave 513 mg BaSO4 precipitate? What is the mass percentage of barium in the compound?

A chemist added an excess of sodium sulfate to a solution of a soluble barium compound to precipitate all of the barium ion as barium sulfate, BaSO4 (233.39). How many grams of barium ion (137.33) are in a 458-mg sample of the barium compound if a solution of the sample gave 513 mg BaSO4 precipitate? What is the mass percentage of barium in the compound?

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...

See similar textbooks

Similar questions

If 25.2 mL of AgNO3 is needed to precipitate all the Cl ions in a 0.775-mg sample of KCI (forming AgCl), what is the molarity of the AgNO3 solution?
In an experiment, a student combines 75.0 mL of a 0.190 M iron (III) chloride solution with 125.0 mL of a 0.240 M sodium carbonate solution. What is the theoretical yield of sodium chloride (in grams)?
The active ingredient in Antabuse, a drug used in the treatment of chronic alcoholism, is tetraethylthiuram disulfide, shown below. All the sulfur in a 0.8329 g sample of an Antabuse preparation is converted to sulfuric acid (by digestive oxidation) which is then titrated with 29.13 mL of 0.04336 M sodium hydroxide. Determine the % Antabuse in the preparation.
If you have 155 mL solution of a 0.762 M FeCl3 solution, how many moles of are FeCl3 are contained in this sample.
A student pipets 18 mL of a 0.0459 M solution of CaCl2 into a 100.00 mL volumetric flask and dilutes to the mark. What is the concentration of the resulting solution?
A 2.85 g sample of NaCl and CaCl2 was dissolved in water, and an excess of AgNO3 was added to precipitate all of the chloride ions.The AgCl was collected and dried, and weighed to give 7.20 g of AgCl. How much NaCl and CaCl2 was in the sample? i g NaCl g CaCl2
What mass of iron(III) hydroxide precipitate can be produced by reacting 76.0 mL of 0.290 M iron(III) nitrate with 194 mL of 0.130 M sodium hydroxide
Barium can be analyzed by precipitating it as BaS04 and determining the mass of the precipitate. When a 0.269 g sample of a barium compound was treated with excess H2S04, 0.0891 g of BaS04 formed. What percentage of barium is in the compound?
0.8888 g a mixture contains calcium chloride and potassium nitrate. To determine the % of each compound, silver nitrate was added to these solutions to precipitate all the chlorine in a form of silver chloride. 1.885 grams of silver chloride was precipitated, washed and dried. Calculate the % of calcium chloride in the sample.
20.0 mL of a 0.617 M lithium phosphide and 25.0 mL of a 0.592 M molybdenum (IV) chloride. What mass of solid, in grams, is formed?
If a solution containing 54.2154.21 g of lead(II) chlorate is allowed to react completely with a solution containing 8.5648.564 g of sodium sulfide, how many grams of solid precipitate will be formed? mass of solid precipitate: gg How many grams of the reactant in excess will remain after the reaction? mass of excess reactant: gg Assuming complete precipitation, how many moles of each ion remain in solution? If an ion is no longer in solution, enter a zero (0) for the number of moles. Pb2+=Pb2+= molmol ClO–3=ClO3–= molmol Na+=Na+= molmol S2−S2− mol
A student determines the calcium content of a solution by first precipitating it as calcium hydroxide, and then decomposing the hydroxide to calcium oxide by heating. How many grams of calcium oxide should the student obtain if his solution contains 48.0 mL of 0.479 M calcium nitrate? g