AP Chemistry
posted by KorieBird
DrBob222 thank you for your previous response. I am reposting the entire question.
Two different 1.2 L buffered solutions were prepared using HOBr and LiOBr. Both buffered solutions had a pH of 5.2 at 25C. After 0.17 mols of HI were added to each of the solutions, it was found that the pH of one solution had dropped to 4.9 and the pH of the other had dropped to 3.1.
a. What is the balanced net ionic equation for the reaction that occurred when HI was added to these buffered solutions?
b. What trend must be true when comparing the concentrations of HOBr and OBr in the two solutions is they shared the same pH before the HI was added?
Thank you!
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I'm having trouble getting the net ionic equation when HI is added to a buffered solution of HOBr. And the net ionic when HI is added to LiOBr. From those results I'm supposed to compare why one pH drops more than the other.