A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: H2SO, (aq) + BaCI, (aq) → BaSO, (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 35.4 grams of barium sulfate are produced, what mass of H2SO, dissolved in the initial aqueous solution? g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol • sulfuric acid = 98.0 g/mol

A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: H2SO, (aq) + BaCI, (aq) → BaSO, (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 35.4 grams of barium sulfate are produced, what mass of H2SO, dissolved in the initial aqueous solution? g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol • sulfuric acid = 98.0 g/mol

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...

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One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl₂(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cd(NO3)₂(aq) The chemist adds 75.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 7.0 mg of silver chloride. Calculate the concentration of cadmium chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits. mg L
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A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: H,SO, (aq) + BaCl, (aq) → Baso4 (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 39.5 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? g [Number in standard notation; round your answer to one decimal place] The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol • sulfuric acid = 98.0 g/mol
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A mixture of barium chloride and sulfuric acid yield the precipitate barium sulfate and hydrochloric acid according to the double replacement reaction: 1H2SO4 (aq) +1 BaCl2 (aq) --> 1 BaSO4 (s) + 2 HCI (aq) A large quantity of barium chloride is used to ensure that the sulfuric acid is the limiting reactant. If 37.2 grams of barium sulfate are produced, what mass of H2SO4 must be dissolved in the initial aqueous solution? -g round your answer to appropriate significant digits. The following molar masses may or may not be needed, but are provided to save you time: • barium sulfate = 233 g/mol sulfuric acid = 98.0 g/mol
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One way the U.S. Environmental Protection Agency (EPA) tests for chloride contaminants in water is by titrating a sample of silver nitrate solution. Any chloride anions in solution will combine with the silver cations to produce bright white silver chloride precipitate. Suppose an EPA chemist tests a 200. mL sample of groundwater known to be contaminated with copper(II) chloride, which would react with silver nitrate solution like this: CuCl2(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Cu(NO3)2(aq) The chemist adds 75.0 mM silver nitrate solution to the sample until silver chloride stops forming. He then washes, dries, and weighs the precipitate. He finds he has collected 6.3 mg of silver chloride. Calculate the concentration of copper(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg L