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3. Write a balanced net 1onic equation for all 3 rcactions in this experiment.

3. Write a balanced net 1onic equation for all 3 rcactions in this experiment.

Introduction to Chemical Engineering Thermodynamics
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
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For the series of reactions in picture one, what is the answer to the attached question?

Procedure Part I: Standardization of the Hydrochloric Acid 1. Obtain about 100 mL of hydrochloric acid. Prepare a butet for titration with the HCl by rinsing first with distilled water and then again with the acid. Be sure to fill the buret tip. Record the initial volume. 2. Place a about 0.3 grams of sodium carbonate into a weighing boat and record the mass. Transfer about balf into an Erlenmeyer flask and re-record the mass. Add about 20 mL of water to the flask along with a few drops of methyl orange. 3. Titrate the sodium carbonate to the end point, carefully recording the final volume. 4. Repeat steps 2&3 for a 2nd trial. Part II: Standardization of the Calcium Hydroxide 1. Obtain about 60 mL of the calcium hydroxide solution. Pour the mixture through filter paper to remove any undissolved solids. Record the temperature of the solution. 2. Wearing a rubber glove, discard the filter paper into the dry waste container and repeat the filtration with a new piece of filter paper. 3. Measure exactly 20.00 mL of the filtrate and pour into a 125 mL Erlenmeyer and add about 5 drops of indicator. Use distilled water to rinse residual liquid from the cylinder into the flask. 4. Prepare the buret for titration with the hydrochloric acid. Fill the buret with the standardized acid solution and record the initial volume. 5. Titrate the calcium hydroxide to the end point, carefully recording the final volumc. 6. Repeat the titration for a 2nd trial. 7. Dispose of any extra base solution in the liquid waste coutainer. 8. Thoroughly rinse all glassware.
Transcribed Image Text:Procedure Part I: Standardization of the Hydrochloric Acid 1. Obtain about 100 mL of hydrochloric acid. Prepare a butet for titration with the HCl by rinsing first with distilled water and then again with the acid. Be sure to fill the buret tip. Record the initial volume. 2. Place a about 0.3 grams of sodium carbonate into a weighing boat and record the mass. Transfer about balf into an Erlenmeyer flask and re-record the mass. Add about 20 mL of water to the flask along with a few drops of methyl orange. 3. Titrate the sodium carbonate to the end point, carefully recording the final volume. 4. Repeat steps 2&3 for a 2nd trial. Part II: Standardization of the Calcium Hydroxide 1. Obtain about 60 mL of the calcium hydroxide solution. Pour the mixture through filter paper to remove any undissolved solids. Record the temperature of the solution. 2. Wearing a rubber glove, discard the filter paper into the dry waste container and repeat the filtration with a new piece of filter paper. 3. Measure exactly 20.00 mL of the filtrate and pour into a 125 mL Erlenmeyer and add about 5 drops of indicator. Use distilled water to rinse residual liquid from the cylinder into the flask. 4. Prepare the buret for titration with the hydrochloric acid. Fill the buret with the standardized acid solution and record the initial volume. 5. Titrate the calcium hydroxide to the end point, carefully recording the final volumc. 6. Repeat the titration for a 2nd trial. 7. Dispose of any extra base solution in the liquid waste coutainer. 8. Thoroughly rinse all glassware.
3. Write a balanced net ionic equation for all 3 reactions in this experiment.
Transcribed Image Text:3. Write a balanced net ionic equation for all 3 reactions in this experiment.
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