5. Answer the following questions a-d: Type all questions and answers. a. i) Look at your results for Table II. Which one of the three buffers was the best buffer overall? ii) Look at the number of drops. Which solution preparation was the best buffer against HCI? iii) Which was the best buffer against NaOH? b. Looking at the method of preparation and molarities in the prepared solutions; Explain why you think the particular preparation chosen in answer (a) above buffered better against HCl or NaOH. c. Using your text book or internet sources, summarize the use of another chemical buffer in our body, environment, or industrial usage THAT WAS NOT MENTIONED IN THIS EXPERIMENT. Include your reference. Just saying "so and so is a buffer" does not answer this question. Your answer should include appropriate reactions as well. d. Was water a good buffer? Explain your answer. Be careful to not just restate the facts.

5. Answer the following questions a-d: Type all questions and answers. a. i) Look at your results for Table II. Which one of the three buffers was the best buffer overall? ii) Look at the number of drops. Which solution preparation was the best buffer against HCI? iii) Which was the best buffer against NaOH? b. Looking at the method of preparation and molarities in the prepared solutions; Explain why you think the particular preparation chosen in answer (a) above buffered better against HCl or NaOH. c. Using your text book or internet sources, summarize the use of another chemical buffer in our body, environment, or industrial usage THAT WAS NOT MENTIONED IN THIS EXPERIMENT. Include your reference. Just saying "so and so is a buffer" does not answer this question. Your answer should include appropriate reactions as well. d. Was water a good buffer? Explain your answer. Be careful to not just restate the facts.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.7QE

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Similar questions

Did either buffer F or G reach buffer capacity? How do you know? Explain your reasoning.
a). What are acids, bases and buffers?b) What are the different types of buffers? Describe the mechanism howbuffers resist pH change in a system.c) Elaborate all chemical reactions in the standardization of NaOH withKHP?d) Why do you need to use KHP in the standardization of NaOH?e) Why is phenolphthalein used as an indicator in this experiment?f) Compare and contrast: endpoint vs equivalence point.g) Discuss the role of acids, bases, buffers and pH in water qualitymonitoring and post-harvest fisheries.
I need help calculating the concentration of acid in each buffer solution show in the second picture!!!! ALSO - make sure for the unrounded values there is 6 sig figs!! EXPERIMENTAL DATA Sample HIn (mL) 1.10 M Acetic Acid (mL) 0.90 M Sodium Acetate (mL) 1 10.00 8.00 2.00 2 10.00 7.00 3.00 3 10.00 6.00 4.00 4 10.00 5.00 5.00 5 10.00 4.00 6.00 6 10.00 3.00 7.00 7 10.00 2.00 8.00 8 10.00 1.00 9.00 9 10.00 10.00 mL NaOH (0.10 M) 10 10.00 10.00 mL HCl (0.10 M)
How would the results of an experiment change if a basic buffer was utilized instead of an acidic one? in this experiment a strong base and strong acid are titrated agaisnt water and an acidic buffer. however, how were the reuslts differ with a basic buffer? please explain
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I need answer for question 1 2 3 and 4 based on the finished titration data sheet
To prepare the buffer, a total volume of 600 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 1.5 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (round off final answer to 2 decimal places)
Compute for the titratable acidity of vinegar sample if 6 ml of 1.0 N NaOH was used to titrate 25 ml of sample. Can this sample be used commercially if the standard is 4% titratable acidity?
ou let your partner do a trial since you're nice. He/she adds a few mL of NaOH, but you realize that nobody recorded the initial buret level! RATS! What do you do? a) Just get light pink since that's the point of titrations anyways. b) Finish the titration and record the final buret reading. Ask your instructor what the initial buret reading was since he knows all of them by heart...right? c) Just record the current level as the "initial" reading. Precision isn't THAT important. d) Restart the trial since you have no idea how much NaOH was added so far.
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To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is available at 1 gallon with a concentration of 0.45 M. (Remember the lesson on dilution: C1V1=C2V2) 4. How many mL should be taken from the stock solution to prepare the desired buffer solution? (Supply answer up to the 2nd decimal point)