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IV. Laboratory Report: (Parts 1,4,5 are typed.) 1. Title page including the average calculated value of molarity of NaOH and the precision of the titrations, as well as your section number and date. 2. Signed prelab assignment torn from manual. 3. Photocopies of laboratory notebook pages containing data. 4. Prepare a table summarizing each titration, including average molarity and relative standard deviation. If you do more than three titrations, show all the data and include your relative standard deviation for all titrations. Title: Give table a descriptive title Titration MNaOH (mol/L) Maverage NaOH 1 3 Precision: If you do more than three titrations, show all the data and indicate which ones were used to calculate your average molarity. Show all calculations for this table (neatly) on additional paper and attach. 5. Error Analysis Questions: A detailed discussion on how to approach error analysis questions was covered in the introduction to this lab manual. Please go back and read that section again. On the following pages are questions that ask "Will the calculated Molarity of NaOH be too HIGH or too LOW or UNAFFECTED if the following errors happen?". An example of how to approach error analysis of this type is shown below: The weight of KHP written in the data book is higher than was actually used. Since moles of NaOH is calculated from the recorded weight of KHP, this gives a high value of moles of NaOH. Also since we actually titrate less KHP we use less volume of NaOH than what you expect. Our calculation becomes: high moles Molarity of NaOH Molarity will be too HIGH low volume

IV. Laboratory Report: (Parts 1,4,5 are typed.) 1. Title page including the average calculated value of molarity of NaOH and the precision of the titrations, as well as your section number and date. 2. Signed prelab assignment torn from manual. 3. Photocopies of laboratory notebook pages containing data. 4. Prepare a table summarizing each titration, including average molarity and relative standard deviation. If you do more than three titrations, show all the data and include your relative standard deviation for all titrations. Title: Give table a descriptive title Titration MNaOH (mol/L) Maverage NaOH 1 3 Precision: If you do more than three titrations, show all the data and indicate which ones were used to calculate your average molarity. Show all calculations for this table (neatly) on additional paper and attach. 5. Error Analysis Questions: A detailed discussion on how to approach error analysis questions was covered in the introduction to this lab manual. Please go back and read that section again. On the following pages are questions that ask "Will the calculated Molarity of NaOH be too HIGH or too LOW or UNAFFECTED if the following errors happen?". An example of how to approach error analysis of this type is shown below: The weight of KHP written in the data book is higher than was actually used. Since moles of NaOH is calculated from the recorded weight of KHP, this gives a high value of moles of NaOH. Also since we actually titrate less KHP we use less volume of NaOH than what you expect. Our calculation becomes: high moles Molarity of NaOH Molarity will be too HIGH low volume

Chemistry
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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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IV. Laboratory Report: (Parts 1,4,5 are typed.) 1. Title page including the average calculated value of molarity of NaOH and the precision of the titrations, as well as your section number and date. 2. Signed prelab assignment torn from manual. 3. Photocopies of laboratory notebook pages containing data. 4. Prepare a table summarizing each titration, including average molarity and relative standard deviation. If you do more than three titrations, show all the data and include your relative standard deviation for all titrations. Title: Give table a descriptive title Titration MNaOH (mol/L) Maverage NaOH 1 3 Precision: If you do more than three titrations, show all the data and indicate which ones were used to calculate your average molarity. Show all calculations for this table (neatly) on additional paper and attach. 5. Error Analysis Questions: A detailed discussion on how to approach error analysis questions was covered in the introduction to this lab manual. Please go back and read that section again. On the following pages are questions that ask "Will the calculated Molarity of NaOH be too HIGH or too LOW or UNAFFECTED if the following errors happen?". An example of how to approach error analysis of this type is shown below: The weight of KHP written in the data book is higher than was actually used. Since moles of NaOH calculated from the recorded weight of KHP, this gives a high value of moles of NaOH. Also since we actually titrate less KHP we use less volume of NaOH than what you expect. Our calculation becomes: high moles Molarity of NaOH Molarity will be too HIGH low volume 42
Transcribed Image Text:IV. Laboratory Report: (Parts 1,4,5 are typed.) 1. Title page including the average calculated value of molarity of NaOH and the precision of the titrations, as well as your section number and date. 2. Signed prelab assignment torn from manual. 3. Photocopies of laboratory notebook pages containing data. 4. Prepare a table summarizing each titration, including average molarity and relative standard deviation. If you do more than three titrations, show all the data and include your relative standard deviation for all titrations. Title: Give table a descriptive title Titration MNaOH (mol/L) Maverage NaOH 1 3 Precision: If you do more than three titrations, show all the data and indicate which ones were used to calculate your average molarity. Show all calculations for this table (neatly) on additional paper and attach. 5. Error Analysis Questions: A detailed discussion on how to approach error analysis questions was covered in the introduction to this lab manual. Please go back and read that section again. On the following pages are questions that ask "Will the calculated Molarity of NaOH be too HIGH or too LOW or UNAFFECTED if the following errors happen?". An example of how to approach error analysis of this type is shown below: The weight of KHP written in the data book is higher than was actually used. Since moles of NaOH calculated from the recorded weight of KHP, this gives a high value of moles of NaOH. Also since we actually titrate less KHP we use less volume of NaOH than what you expect. Our calculation becomes: high moles Molarity of NaOH Molarity will be too HIGH low volume 42
using it. Fill the buret to about the 0 mL mark. Release some of the solution into an empty beaker. There should be no air bubbles in the tip of the buret. When this is completed, be sure to record the starting volume of the solution in the buret. The initial reading will not be 0.0. When you record volume of a liquid in a 50 mL buret, be sure to record two digits to the right of the decimal point. The last digit is estimated. 7. In your data book prepare the following table (Give a title to the table). With any measured value you must show its units with the column heading. Use a ruler to prepare the lines for the table. Title Titration # KHP (g) Vfinal (mL) | Vinitial (mL) | Vtotal NaOH (mL) 33 36 3. D-7430 1 22.05 14.00 2 1.05 |0.7805 37 3 Proper reading of your buret: 3.0 3.0 - Meniscus (3.30 ml) Meniscus (3.90 ml) 4.0 4.0 Assume that the buret is filled to the point indicated in the figure at the left. You would record the initial point as 3.30 ml; the ending point would be 3.90 ml. Therefore, the titration would have required 0.60 ml. Remember that you should read the number that is at the bottom of the meniscus. 3.90 – 3.30 = 0.60 mL Your buret volume readings for this example would be entered on your table as follows: Titration # KHP (g) Vfinal (mL) Vinitial (mL) Vtotal NAOH (mL) 1 3.90 3.30 0.60 2 3 8. Add 3 drops of phenolphthalein indicator and a clean magnetic stirring bar to the first flask and titrate using the standard NaOH to the first faint pink end point that persists 40
Transcribed Image Text:using it. Fill the buret to about the 0 mL mark. Release some of the solution into an empty beaker. There should be no air bubbles in the tip of the buret. When this is completed, be sure to record the starting volume of the solution in the buret. The initial reading will not be 0.0. When you record volume of a liquid in a 50 mL buret, be sure to record two digits to the right of the decimal point. The last digit is estimated. 7. In your data book prepare the following table (Give a title to the table). With any measured value you must show its units with the column heading. Use a ruler to prepare the lines for the table. Title Titration # KHP (g) Vfinal (mL) | Vinitial (mL) | Vtotal NaOH (mL) 33 36 3. D-7430 1 22.05 14.00 2 1.05 |0.7805 37 3 Proper reading of your buret: 3.0 3.0 - Meniscus (3.30 ml) Meniscus (3.90 ml) 4.0 4.0 Assume that the buret is filled to the point indicated in the figure at the left. You would record the initial point as 3.30 ml; the ending point would be 3.90 ml. Therefore, the titration would have required 0.60 ml. Remember that you should read the number that is at the bottom of the meniscus. 3.90 – 3.30 = 0.60 mL Your buret volume readings for this example would be entered on your table as follows: Titration # KHP (g) Vfinal (mL) Vinitial (mL) Vtotal NAOH (mL) 1 3.90 3.30 0.60 2 3 8. Add 3 drops of phenolphthalein indicator and a clean magnetic stirring bar to the first flask and titrate using the standard NaOH to the first faint pink end point that persists 40
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