[mirandab17]

Hey there!

Really lost with all this stuff.

Two different 1.2 L buffered solutions are prepared using HOBr and LiOBr. Both
buffered solutions have a pH of 5.2 at 25°C. After 0.17 moles of HI are added to each of
the solutions, it is 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 occurs when HI is
added to these buffered solutions.

Alright, so for this... do I split this up into two equations?
HOBr + HI <> OBr + H2I.
But even here, I get a bit lost... if it is buffered, doesn't that mean its conjugate base has to be on the other side? See, HI, is a strong acid though, so doesn't it have to look like this?

HOBr + HI <> I + H2OBr.

For the LiOBr one...

LiOBr + HI <> I + HOBr.

*delete me*  

b. What trend must be true when comparing the concentrations of HOBr and OBr­ in
the two solution s if they shared the same pH before the HI was added? Justify the
answer. (Hint: The concentration of acid in the solutions is not the same.)

c. Explain why the pH of the two solutions ended up being different after the same
amount of HI was added to each.

[AWK]

You should write and balance correctly these two reaction and all should be clear.

HOBr + HI <> I + H2OBr.

LiOBr + HI <> I + HOBr.