B. Determining the Composition of a Mixture of Sodium Chloride and Sodium Nitrate Partner I Prepare a solution of sodium chloride + sodium nitrate and indicator. Obtain a dropper bottle of potassium chromate (indicator) solution. To a clean and dry 125 mL Erlenmeyer flask, add about 40 mL of water and 8 drops of indicator solution. Weigh out approximately 0.05 grams of sodium chloride + sodium nitrate solid and record its exact mass. Dissolve the solid in the solution from step 1, stirring with a stirring rod to ensure complete dissolution. Determine and record the total mass of the Erlenmeyer flask and solution, noting the balance that you use to weigh. Rather than measuring the volume of silver nitrate solution added as in Part A, we will measure the mass of titrant added and make use of the weight-percentage concentration of silver nitrate in calculations. Prepare the silver nitrate solution. Obtain about 15 mL of 1.70% w/w silver nitrate solution in a 50 mL beaker. Designate a Pasteur pipet and Pasteur pipet bulb to use for the addition of silver nitrate solution to the Erlenmeyer flask. Titrate the chloride solution with silver nitrate to a persistent orange endpoint. Add about one pipet's worth of silver nitrate solution to the Erlenmeyer flask and gently swirl. You should observe a chemical change; record your observations. Continue to add silver nitrate solution dropwise via Pasteur pipet to the Erlenmeyer flask. Every few drops, swirl the flask until its color stabilizes. Stop adding silver nitrate solution immediately when you observe a persistent orange color in the flask. Measure the mass of silver nitrate solution added. Reweigh the flask and solution using the same balance you used in step 3. Record the final mass and determine the mass of silver nitrate solution delivered into the flask. Partner II Once the titration is complete, ensure that you have recorded the exact mass of solid mixture used and the mass of silver nitrate solution delivered. Discard any excess silver nitrate solution and the contents of the Erlenmeyer flask in the waste bottle in the hood. Use your wash bottle and some water to rinse the precipitate out of the flask and into the waste bottle. In Part B of the experiment 0.103 g of a solid mixture of NaCl and NaNO3 was dissolved in 100 mL of water with K2CrO4 indicator. A mass of 4.18 g of 1.70% AgNO3 solution was required to fully consume all of the chloride in the mixture. What was the mass percentage of NaCl in the original solid mixture? Enter your answer to the nearest tenth of a percent; do not include the percent symbol.

B. Determining the Composition of a Mixture of Sodium Chloride and Sodium Nitrate Partner I Prepare a solution of sodium chloride + sodium nitrate and indicator. Obtain a dropper bottle of potassium chromate (indicator) solution. To a clean and dry 125 mL Erlenmeyer flask, add about 40 mL of water and 8 drops of indicator solution. Weigh out approximately 0.05 grams of sodium chloride + sodium nitrate solid and record its exact mass. Dissolve the solid in the solution from step 1, stirring with a stirring rod to ensure complete dissolution. Determine and record the total mass of the Erlenmeyer flask and solution, noting the balance that you use to weigh. Rather than measuring the volume of silver nitrate solution added as in Part A, we will measure the mass of titrant added and make use of the weight-percentage concentration of silver nitrate in calculations. Prepare the silver nitrate solution. Obtain about 15 mL of 1.70% w/w silver nitrate solution in a 50 mL beaker. Designate a Pasteur pipet and Pasteur pipet bulb to use for the addition of silver nitrate solution to the Erlenmeyer flask. Titrate the chloride solution with silver nitrate to a persistent orange endpoint. Add about one pipet's worth of silver nitrate solution to the Erlenmeyer flask and gently swirl. You should observe a chemical change; record your observations. Continue to add silver nitrate solution dropwise via Pasteur pipet to the Erlenmeyer flask. Every few drops, swirl the flask until its color stabilizes. Stop adding silver nitrate solution immediately when you observe a persistent orange color in the flask. Measure the mass of silver nitrate solution added. Reweigh the flask and solution using the same balance you used in step 3. Record the final mass and determine the mass of silver nitrate solution delivered into the flask. Partner II Once the titration is complete, ensure that you have recorded the exact mass of solid mixture used and the mass of silver nitrate solution delivered. Discard any excess silver nitrate solution and the contents of the Erlenmeyer flask in the waste bottle in the hood. Use your wash bottle and some water to rinse the precipitate out of the flask and into the waste bottle. In Part B of the experiment 0.103 g of a solid mixture of NaCl and NaNO3 was dissolved in 100 mL of water with K2CrO4 indicator. A mass of 4.18 g of 1.70% AgNO3 solution was required to fully consume all of the chloride in the mixture. What was the mass percentage of NaCl in the original solid mixture? Enter your answer to the nearest tenth of a percent; do not include the percent symbol.

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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B. Determining the Composition of a Mixture of Sodium Chloride and Sodium Nitrate

Partner I

Prepare a solution of sodium chloride + sodium nitrate and indicator. Obtain a dropper bottle of potassium chromate (indicator) solution. To a clean and dry 125 mL Erlenmeyer flask, add about 40 mL of water and 8 drops of indicator solution.
Weigh out approximately 0.05 grams of sodium chloride + sodium nitrate solid and record its exact mass. Dissolve the solid in the solution from step 1, stirring with a stirring rod to ensure complete dissolution.
Determine and record the total mass of the Erlenmeyer flask and solution, noting the balance that you use to weigh. Rather than measuring the volume of silver nitrate solution added as in Part A, we will measure the mass of titrant added and make use of the weight-percentage concentration of silver nitrate in calculations.
Prepare the silver nitrate solution. Obtain about 15 mL of 1.70% w/w silver nitrate solution in a 50 mL beaker. Designate a Pasteur pipet and Pasteur pipet bulb to use for the addition of silver nitrate solution to the Erlenmeyer flask.
Titrate the chloride solution with silver nitrate to a persistent orange endpoint. Add about one pipet's worth of silver nitrate solution to the Erlenmeyer flask and gently swirl. You should observe a chemical change; record your observations.
Continue to add silver nitrate solution dropwise via Pasteur pipet to the Erlenmeyer flask. Every few drops, swirl the flask until its color stabilizes.
Stop adding silver nitrate solution immediately when you observe a persistent orange color in the flask.
Measure the mass of silver nitrate solution added. Reweigh the flask and solution using the same balance you used in step 3. Record the final mass and determine the mass of silver nitrate solution delivered into the flask.

Partner II

Once the titration is complete, ensure that you have recorded the exact mass of solid mixture used and the mass of silver nitrate solution delivered.
Discard any excess silver nitrate solution and the contents of the Erlenmeyer flask in the waste bottle in the hood. Use your wash bottle and some water to rinse the precipitate out of the flask and into the waste bottle.

In Part B of the experiment 0.103 g of a solid mixture of NaCl and NaNO₃was dissolved in 100 mL of water with K₂CrO₄ indicator. A mass of 4.18 g of 1.70% AgNO₃ solution was required to fully consume all of the chloride in the mixture. What was the mass percentage of NaCl in the original solid mixture? Enter your answer to the nearest tenth of a percent; do not include the percent symbol.

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