(g) (2 pts.) How does the hydrogen ion (H+) [or the hydronium ion (H3O+)] and the hydroxide ion (OH-) fit into all of this? What is their role in this reaction? In the case of this particular example that you watched, where would each of these ions have come from?
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(h) (2 pts.) Suppose I wanted to calculate the pH of the acid used in this titration. How (explain) can I use the results from this experiment to do this? What would the pH be in this case? Show all work.
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(i) (2 pts.) Throughout the video there were various suggestions that came up that were useful tips for you to remember that would help make sure your titration was a successful one. Dr. Yee mentions a few, but there were also some that came up within the images on the screen. What were at least 2 tips for carrying out a successful titration?
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(j) (1 pts.) In the second video listed above, red cabbage was demonstrated as a natural indicator, and the hydrangea flower was also mentioned. Do some research (include references) and find and discuss another natural acid/base indicator that was not mentioned in the video.
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(k) Suppose your instructor handed you a bottle of sulfuric acid of unknown concentration. The chemistry department was considering using it for a summer program for elementary students to test rock samples to see if they contain limestone. However, they don’t want to give it to the kids if it is too strong, and noone in the department was willing to drop some on their skin, and all the graduate students and TA’s were already guinea pigs in other experiments, and the department did not want to compromise the data from that research in any way. So, the task falls to you, the eager undergraduate student.
(2 pts.) First, explain, using a chemical equation, and then describing it, how sulfuric acid could test for the presence of limestone. What specific reaction would be taking place, and what easily noticeable phenomenon would you be looking for when doing this test? Why?
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[ii] (3 pts.) Suppose you take a 25.00 mL sample of this sulfuric acid solution. You then titrate it with a 0.1322 M potassium hydroxide solution. A volume of 41.22 mL of potassium hydroxide was required to complete the titration. What is the concentration of this unknown sulfuric acid solution?
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