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

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

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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A sample of brass weighing 1.203 grams was analyzed. Brass is an alloy composed of copper, Cu, and zinc, Zn. The zinc in the alloy was reacted with 35.123 grams of hydrochloric acid, HCl, in excess, according to the following balanced equation: Zn(s) + 2 HCl (aq) → H2 (g) + ZnCl2 (aq) After all of the zinc reacted, the mass of the remaining solution weighed 36.309 grams. What mass of hydrogen gas was produced? What mass of zinc reacted? What was the percentage of zinc (by mass) in the alloy?
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 250.mL sample of groundwater known to be contaminated with cadmium chloride, which would react with silver nitrate solution like this: CdCl2(aq)+2AgNO3(aq)→2AgCl(s)+CdNO32(aq). The chemist adds 51.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 8.9mg 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.
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 3 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
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 iron(III) chloride, which would react with silver nitrate solution like this: FeCl3 (aq) + 3AgNO3 (aq) →3AgCl (s) + (FeNO3)3 (aq) The chemist adds 48.0mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 7.5mg of silver chloride. Calculate the concentration of iron(III) chloride contaminant in the original groundwater sample. Be sure your answer has the correct number of significant digits.
Iron(II) sulfide reacts with hydrochloric acid according to the reaction FeS(s)+2HCl(aq)→FeCl2(aq)+H2S(s) A reaction mixture initially contains 0.218 mol FeS and 0.636 mol HCl. Once the reaction has reached completion, what amount (in moles) of the excess reactant is left?
1)What is the theoretical yield (in grams) of CaCO3 in the precipitation reaction that occurs when when a solution prepared by dissolving 1.004 g of solid CaCl2 in 30 mL of water is mixed with a solution prepared by dissolving 0.997 g of Na2CO3 in 30 mL of water?Include the appropriate number of significant figures in your answer. 2)Suppose that 0.814 g of CaCO3 is actually isolated in the precipitation reaction described in Question 1. What is the percent yield of this reaction?Report your answer to the correct number of significant figures. 3)A solution of Na2CO3 is prepared by dissolving 0.511 g of the solid in approximately 30 mL of water. How many moles of Na2CO3 does this solution contain? Express your answer to the correct number of significant figures. 4)Suppose the Na2CO3 solution described in Question 13 is added to a solution that contains excess CaCl2? What is the maximum number of moles of solid CaCO3 that can form in the resulting precipitation reaction?…
The rocket boosters of the space shuttle Discovery, launched on July 26, 2005, used a fuel mixture containing primarily solid ammonium perchlorate, NH4ClO4, and aluminum metal. The unbalanced chemical equation for the reaction is given below. (Hint: Balance the elements in the order Cl, H, O, Al, N.) Al(s) + NH4CIO4(s) Al₂O3(s) + AlCl3(s) + H₂O(l) + N₂(g) What is the mass (in kilograms) of NH4ClO4 consumed per kilogram of Al, assuming a percent yield of 87.20%? (Answer with two decimal places.)
The useful metal manganese can be extracted from the mineral rhodochrosite by a two-step process. In the first step, manganese(II) carbonate and oxygen react to form manganese(IV) oxide and carbon dioxide: 2MnCO3(s) + O₂(g) → In the second step, manganese (IV) oxide and aluminum react to form manganese and aluminum oxidide: 3 MnO₂ (s) + 4A1(s) 3 Mn (s) + 2 Al₂O3(s) Check 2 MnO₂ (s) + 2 CO₂ (g) Suppose the yield of the first step is 88.% and the yield of the second step is 70.%. Calculate the mass of manganese(II) carbonate required to make 1.0 kg of manganese. Be sure your answer has a unit symbol, if needed, and is rounded to the correct number of significant digits. 0 0 x10 nin 0 0.0 S Save For Later E OL A S C Submit Assignmen
Sulfuric acid dissolves aluminum metal according to the following reaction: 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Suppose you wanted to dissolve an aluminum block with a mass of 15.6 g . a) What minimum mass of H2SO4 would you need? Express your answer in grams. b)What mass of H2 gas would be produced by the complete reaction of the aluminum block?Express your answer in grams.
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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 250. mL sample of groundwater known to be contaminated with iron(II) chloride, which would react with silver nitrate solution like this: FeCl₂(aq) + 2 AgNO3(aq) → 2 AgCl(s) + Fe(NO3)₂(aq) The chemist adds 16.0 mM silver nitrate solution to the sample until silver chloride stops forming. She then washes, dries, and weighs the precipitate. She finds she has collected 2.0 mg of silver chloride. Calculate the concentration of iron(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg 0 L x10 X Ś
In the experiment, a student is given 2.94 g of a mixture containing anhydrous MgCl2 and KNO3. To determine the percentage by mass of MgCl2 in the mixture, the student uses excess AgNO3(aq) to precipitate the chloride ion as AgCl(s). Starting with the 2.94 g sample of the mixture dissolved in water, briefly describe the steps necessary to quantitatively determine the mass of the AgCl precipitate. The student determines the mass of the AgCl precipitate to be 5.48 g. On the basis of this information, calculate each of the following.(i) The number of moles of MgCl2 in the original mixture (ii) The percent by mass of MgCl2 in the original mixture