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B. Molar Concentration of an Acid Solution Acid type, HA or H₂A: Unknown No. Balanced equation for neutralization of acid with NaOH. Bum Sampte 1 Trail Sample 2 Trail 2 Sample 3

B. Molar Concentration of an Acid Solution Acid type, HA or H₂A: Unknown No. Balanced equation for neutralization of acid with NaOH. Bum Sampte 1 Trail Sample 2 Trail 2 Sample 3

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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Help with the CHEM Lab report please! It is about Volumetric Analysis 

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B. Molar Concentration of an Acid Solution Acid type, HA or H₂A: Unknown No. Balanced equation for neutralization of acid with NaOH. 1. Volume of acid solution (mL) Bum Sampte 1 25.0 Buret reading of NaOH, initial (mL) 3 Buret reading of NaOH, final (mL) 4 Volume of NaOH dispensed (mL) 5 Molar concentration of NaOH (mol/L), Part A 6. Moles of NaOH dispensed (mol) 7. Molar concentration of acid solution (mol/L) 8. Average molar concentration of acid solution (mol/L) 9. Standard deviation of molar concentration 10. Relative standard deviation of molar concentration (%RSD) SO.O 30.0 Traill 142 A Volumetric Analysis Sample 2 25.0 49.5 29.8 Trail 2 Sample 3 25.0 49.7 29.2 Data Analysis, B Data Analysis, C Data Analysis, D Laboratory Questions Circle the questions that have been assigned. 1. Part A.1. Pure potassium hydrogen phthalate is used for the standardization of the sodium hydroxide solution. Suppose that the potassium hydrogen phthalate is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be too high, too low, or unaffected because of the moistness of the potassium hydrogen phthalate? Explain. 2. Part A.2. The student forgot to prepare any boiled, deionized water for the preparation of the NaOH solution and then forgot to cap the bottle. Will the concentration of the NaOH solution be greater than, less than, or unaffected by this carelessness? Explain. 3. Part A.6. A drop of the NaOH titrant adheres to the side of the buret (because of a dirty buret) between the initial and final readings for the titration. As a result of the "clean glass" error, will the molar concentration of the NaOH solution be reported as too high or too low? Explain. 4. Part A. The mass of KHC,H4O4 is measured to the nearest milligram; however, the volume of water in which it is dis- solved is never of concern-water is even added to the wall of the Erlenmeyer flask during the titration. Explain why water added to the KHC,H4O4 has no effect on the data, whereas water added to the NaOH solution may drastically affect the data. 5. Part B.2. The wall of the Erlenmeyer flask is occasionally rinsed with water from the wash bottle (see Part A.6) during the analysis of the acid solution. Will this technique result in the molar concentration of the acid solution being reported as too high, too low, or unaffected? Explain. 6. Parts A.6 and B.2. For the standardization of the NaOH solution in Part A.6, the endpoint was consistently reproduced to a faint pink color. However, the endpoint for the titration of the acid solution in Part B.2 was consistently repro- duced to a dark pink color. Will the reported molar concentration of the acid solution be too high, too low, or unaf- fected by the differences in the colors of the endpoints. Explain.
Transcribed Image Text:B. Molar Concentration of an Acid Solution Acid type, HA or H₂A: Unknown No. Balanced equation for neutralization of acid with NaOH. 1. Volume of acid solution (mL) Bum Sampte 1 25.0 Buret reading of NaOH, initial (mL) 3 Buret reading of NaOH, final (mL) 4 Volume of NaOH dispensed (mL) 5 Molar concentration of NaOH (mol/L), Part A 6. Moles of NaOH dispensed (mol) 7. Molar concentration of acid solution (mol/L) 8. Average molar concentration of acid solution (mol/L) 9. Standard deviation of molar concentration 10. Relative standard deviation of molar concentration (%RSD) SO.O 30.0 Traill 142 A Volumetric Analysis Sample 2 25.0 49.5 29.8 Trail 2 Sample 3 25.0 49.7 29.2 Data Analysis, B Data Analysis, C Data Analysis, D Laboratory Questions Circle the questions that have been assigned. 1. Part A.1. Pure potassium hydrogen phthalate is used for the standardization of the sodium hydroxide solution. Suppose that the potassium hydrogen phthalate is not completely dry. Will the reported molar concentration of the sodium hydroxide solution be too high, too low, or unaffected because of the moistness of the potassium hydrogen phthalate? Explain. 2. Part A.2. The student forgot to prepare any boiled, deionized water for the preparation of the NaOH solution and then forgot to cap the bottle. Will the concentration of the NaOH solution be greater than, less than, or unaffected by this carelessness? Explain. 3. Part A.6. A drop of the NaOH titrant adheres to the side of the buret (because of a dirty buret) between the initial and final readings for the titration. As a result of the "clean glass" error, will the molar concentration of the NaOH solution be reported as too high or too low? Explain. 4. Part A. The mass of KHC,H4O4 is measured to the nearest milligram; however, the volume of water in which it is dis- solved is never of concern-water is even added to the wall of the Erlenmeyer flask during the titration. Explain why water added to the KHC,H4O4 has no effect on the data, whereas water added to the NaOH solution may drastically affect the data. 5. Part B.2. The wall of the Erlenmeyer flask is occasionally rinsed with water from the wash bottle (see Part A.6) during the analysis of the acid solution. Will this technique result in the molar concentration of the acid solution being reported as too high, too low, or unaffected? Explain. 6. Parts A.6 and B.2. For the standardization of the NaOH solution in Part A.6, the endpoint was consistently reproduced to a faint pink color. However, the endpoint for the titration of the acid solution in Part B.2 was consistently repro- duced to a dark pink color. Will the reported molar concentration of the acid solution be too high, too low, or unaf- fected by the differences in the colors of the endpoints. Explain.
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