Please type it Volume of the original unknown AGNO3 solution =mLMass of AgCl (s) =,Mole of AgCl =(mole = mass /molar mass)Calculate mole of AgNO3 in the 10 mL unknown solution based on the following reactionequation:NaCl(aq)+ AGNO3(aq) → NaNO(aq) + AgCls)Mole of AGNO3 in the 10 mL unknown solution =use the coefficient ratio)_(hint,Mass of AGNO, in the 10 mL unknown solution =(mass = mole x molar mass)Calculate mass of AGNO, in the original unknown solution as follows:Mass of AGNO, in the original unknown solution= Mass of AGNO3 in the 10 mL unknown solution xvolume of the unknown AGNO3 solution in mL10 ml i.Watch the Introductory Video and Support Information on the upper left to learn how touse this virtual lab.Place a bottle of 0.1 M NaCl solution, the unknown AGNO, solution, a 250 mL Erlenmeyerflask, a 10 mL pipette, and a burette (in Glassware→Other) on the workbench. If thebench is said to be too full, set the items along the right side the bench to save space.Record the volume of the original unknown AGNO3 solution in the Data sheet.ii.Workbench 1Unknown AgNO,52.500 ml. @ 25.0°C0.1M NaCI100.00 ml. 25.0C250 ml Flask0.0000 ml @25.0°C10 mL Pipette0.0000 ml@ 25.0°C50 mL Burette0.0000 ml 25.0°Cii.Transfer 50 mL of 0.1 M NaCl solution into the burette.iv.Withdraw 10 mL of the unknown AgNO, solution into the pipette and transfer the solutioninto the empty Erlenmeyer flask.v.Deliver 1 mL of the 0.1 M NaCI solution from the burette into the 10 mL unknown AGNO,solution. Pay attention to mass of AgCl displayed in the information windowInformationName: 250 mL. FlaskVolume: 11.007 mlSpecies (s)ABCIgrams0.01433210 ml PipetteTemperature: 25.00°C0.0000 mle 25.ordnknown AgNO,500 ml@ 25.0°C250PrediseSig FigRealisticpHt: 7.00Pour 0From 50 ml. Burette to 250 ml. Flask1.00 mL transferred.250 ml. Flask0.1M NaCI11.007 ml@25.0'C50.000 mle 25.0cvi.Repeat addition of 1 mL of the 0.1 M NaCl solution from the burette into the unknownsolution until the mass of AgCl doesn't change any more. Record the mass of theprecipitate AgCI on the Data Sheet.

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Volume of the original unknown AGNO3 solution = mL Mass of AgCI (s) = . Mole of AgCI = . (mole = mass /molar mass) Calculate mole of AGNO, in the 10 mL unknown solution based on the following reaction equation: NaClag) + AGNO3(aq) → NaNO3(aq) + AgCle) Mole of AGNO3 in the 10 mL unknown solution = use the coefficient ratio) _(hint, Mass of AGNO, in the 10 mL unknown solution = (mass = mole x molar mass) Calculate mass of AGNO, in the original unknown solution as follows: Mass of AGNO, in the original unknown solution = Mass of AGNO3 in the 10 mL unknown solution x volume of the unknown AGNO3 solution in ml 10 ml

Volume of the original unknown AGNO3 solution = mL Mass of AgCI (s) = . Mole of AgCI = . (mole = mass /molar mass) Calculate mole of AGNO, in the 10 mL unknown solution based on the following reaction equation: NaClag) + AGNO3(aq) → NaNO3(aq) + AgCle) Mole of AGNO3 in the 10 mL unknown solution = use the coefficient ratio) _(hint, Mass of AGNO, in the 10 mL unknown solution = (mass = mole x molar mass) Calculate mass of AGNO, in the original unknown solution as follows: Mass of AGNO, in the original unknown solution = Mass of AGNO3 in the 10 mL unknown solution x volume of the unknown AGNO3 solution in ml 10 ml

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 38CR

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On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado. The spill was neutralized with sodium carbonate: 2HNO3(aq)+Na2CO3(aq)2NaNO3(aq)+H2O(l)+CO2(g) a. Calculate H for this reaction. Approximately 2.0 104 gal nitric acid was spilled. Assume that the acid was an aqueous solution containing 70.0% HNO3 by mass with a density of 1.42 glcm3. What mass of sodium carbonate was required for complete neutralization of the spill, and what quantity of heat was evolved? (Hf for NaNO3(aq) = 467 kJ/mol) b. According to The Denver Post for April 4, 1983, authorities feared that dangerous air pollution might occur during the neutralization. Considering the magnitude of H, what was their major concern?
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ou have two solutions containing solute A. To determine which solution has the highest concentration of A in molarity, which of the following must you know? (There may be more than one answer.) the mass in grams of A in each solution the molar mass of A the volume of’ water added to each solution the total volume of the solution plain your answer.
Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.
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A chemist performs a gravimetric analysis. The chemist combines 1.00L of 2.00MAgNO3(aq) with 1.00L of 4.00MNaCl(aq) in an Erlenmeyer flask. Both the AgNO3(aq) solution and the NaCl(aq) solution are colorless. After the mixture has been stirred, a cloudy white substance is observed at the bottom of the flask. What is the expected mass of AgCl(s)AgCl(s), in grams, assuming that the yield is 100%100%? In the box, enter the mass to the nearest gram. g