[lpf1991]

Here is the actual problem:

A solution with pH of about 9.7 is prepared by mixing 0.5 L of 1M (HO)₂SO₄ with about _____ mols of H₃N

Answers are: 4.8 , 2.8 , 3.8 , 1.8 , 0.9

Now I'm not sure if the problem is supposed to be (HO)₂SO₂, because last test he put (HO)₂SO₄ and the class was told he meant (HO)₂SO₂ instead.  If both make sense, I would like to know how to do both.

Now I assume that H₂SO₄ dissociates completely in water correct?  So you would have HSO₄^- if that is true.  What then happens?

Thanks

0.5L of 1M H2SO4

[AWK]

Ammonia is a base and react with sulphuric acid to form buffer solution

[magician4]

in addition:

Now I'm not sure if the problem is supposed to be (HO)2SO2, because last test he put (HO)2SO4 and the class was told he meant (HO)2SO2 instead. 

to the best of my knowledge, there is no such acid that has the formula H₂SO₆  (i.e. (HO)₂SO₄ )

furthermore:
as long as there's no water involved, you won't result in whatsoever "solution" with a meaningfull pH
however, if there was water involved, that guy at least should have told you the concentration of sulphuric acid therein, else you can't definitively calculate nothin'

IMHO, this (esp. in combination with this repeatedly nonsensical H₂SO₆) is not a case of bad wording or something like that: this is a case of a completely incompetent "teacher" , who should immediately be removed from class, and be sent back to serious studies himself


regards

Ingo