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 tin(II) chloride, which would react with silver nitrate solution like this: SnCl (aq) + 2 AGNO3(aq) → 2 AgCl(s) + Sn(NO3),(aq) The chemist adds 48.0 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 2.7 mg of silver chloride. Calculate the concentration of tin(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg

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 tin(II) chloride, which would react with silver nitrate solution like this: SnCl (aq) + 2 AGNO3(aq) → 2 AgCl(s) + Sn(NO3),(aq) The chemist adds 48.0 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 2.7 mg of silver chloride. Calculate the concentration of tin(II) chloride contaminant in the original groundwater sample. Round your answer to 2 significant digits. mg

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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Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO;(aq) → NaCl(aq) + H,O(1) + CO,(g) The CO, gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 100. mL of a 0.048 M HCI solution. What mass of NaHCO, would he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. x10
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One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe (s) + CuSO4 (aq) → Cu (s) + FeSO4 (aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 73.mg . Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits.
1.58g of magnesium hydrogencarbonate was added to a 1.68 mol/L solution of acetic acid, CH3COOH in water (50.0 mL), producing carbon dioxide gas, water and magnesium acetate, Mg(CH3COO)2. a) Write a balanced chemical equation for the reaction. b) What mass of acetic acid is in the aqueous solution? | c) Which of the reactants is the limiting reagent? Justify your answer. d) If 1.23 g of magnesium acetate was produced, what is the percentage yield of the reaction? e) What is the theoretical yield (in grams) of carbon dioxide from this reaction? f) The above reaction is performed in a closed 25 L container at 10 °C. Upon completion of the reaction, what will the final pressure of CO2 be inside the container?
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The discharge of chromate ions (CrO42) to sewers or natural waters is of concern because of both its ecological impacts and effects on human health if the receiving water is used as a drinking water source. One way in which chromate can be removed from solution is by its reaction with ferrous iron (Fe²+) to form a mixture of chromic hydroxide and ferric hydroxide solids [Cr(OH)3(s) and Fe(OH)3(s), respectively], which can then be filtered out of the water. The overall reaction can be represented as CrO4 + 3Fe²+ + 8H₂O → Cr(OH)3(s) + Fe(OH)3(s) + 4H+ How much particulate matter would be generated daily by this process at a facility that treats 60 m³/h of a waste stream containing 40 µg/L CrO4²- if the treatment reduced the Cr concentration enough to meet a discharge limit of 10 µg/L (MCL proposed in 2013, voted into law in 2015 and ruled invalid in 2017 for California) or 50 µg/L (current MCL) CrO4²-?
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: FeCl,(aq) + 3 AgNO,(aq) 3 AgCl(s) + Fe(NO₂),(ag) The chemist adds 21.0 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 3.3 mg 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. e -12 D.P C P
Classify the reactions represented by these equations as either single or double placement.
Sodium hydrogen carbonate (NaHCO,), also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid (HCI) , which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO, neutralizes excess HCl through this reaction: HCl(aq) + NaHCO,(aq) → NaCl(aq) + H,O(1) + CO,(g) The CO, gas produced is what makes you burp after drinking the solution. olo Suppose the fluid in the stomach of a man suffering from indigestion can be considered to be 150. mL of a 0.086 M HCl solution. What mass of NaHCO, would Ar he need to ingest to neutralize this much HCl ? Be sure your answer has the correct number of significant digits. Ox10
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Mercury as an amalgam with copper, silver, and tin is used fro fillings in teeth and in the production of chlorine. Soluble mercury compounds can be toxic and must be removed from wastewater. Aqueous mercury (II) nitrate is a toxic compound formed in wastewater and must be removed. To remove this compound, an aqueous sodium sulfide (Na2S) solution is added to wastewater to form a solid mercury (II) sulfide (HgS) precipitate and aqueous sodium nitrate in solution. From the analysis, 0.051 L of 0.010 M mercury (II) nitrate was reacted with 0.020 L of 0.10 M sodium sulfide. Write a balance equation for this chemical reaction. Determine the limiting reactant. How many grams of mercury (II) sulfide form? How many grams of excess reactant remain after the reaction is finished?
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