yeh, but if you mean the cabage question whats the diff on the level of ionisation of the second proton in the H2SO4. is it assumed to be complete and therefore pH 2 or incomplete and then ph higher.champo14 said:Haha, nice one. Did you mean the Haber process one?
I thought the exam was pretty good, and I got most of the calculations.
Did everyone multiply by 2 in the Sulfuric acid one? (Because it's diprotic)
ah~hahahaForbidden. said:I agree with the first part.
I kept asking people at school and MSN, "Who didn't select Ethanol as their renewable resource ?"
Also, when they handed the exam papers to us before reading time, I could see through the first page and saw the first question, from then on I knew it was an easy exam.
Thanks BOS for thin and almost transparent papers, they look like someone's white T-shirt after they've been drenched, saturated, soaked and bombarded by water bombs .
Yeah, you're right. I wrote it small so hopefully they won't notice it.k4t5UM0t0 said:NaHCO3 is definitely not a buffer
buffer is a solution containing equimolar amounts of a weak acid and its conjugate base, that is able to maintain a constant pH when large amounts of acid or base are added.
Amphiprotic: a substance that can act as a bronsted lowry acid (i.e proton donor) and bronsted lowry base (i.e. proton acceptor)
NaHCO3 is cheap, easy to store, weak base, stops bubbling when neutralisation complete with an acid and easy to clean up after neutralisation. Preferable over dilution and neutralisation with strong acid or base.
However large amounts required for large spills
I wish now that I had BSd more on that answer. I wrote that it was amphiprotic but honestly had no idea whether it was or not. I probably could have come up with something about why it's useful. Ah well.Originality said:NaHCO3 is amphiprotic.
I didnt like that exam.