a. The balanced net ionic equation for the reaction that occurred when HI was added to these buffered solutions is: HOBr + HI → H2O + I- + Br-.
b. The trend that must be true when comparing the concentrations of HOBr and OBr- in the two solutions is that the solution with the lower pH (3.1) must have had a higher concentration of OBr- than the solution with the higher pH (4.9).
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!
1 answer
1 answer