Complete this table of initial and final concentrations
HF(aq) + KOH(aq) <-> KF(aq) + H20(l)
Initial concentrations: HF-2.0M KOH-1.0M KF-0M Final Concentrations? how do I set this up to figure out the final concentrations?
How can I tell which of the following best describes the final solution?
a) a neutral salt solution
b) a buffer
c) none of the above
3 answers
I'm a little confused by the problem. HOW MUCH 2.0M HF and HOW MUCH 1.0M KOH? For example I could take 1L of 2.0 M HF and mix with 2L of 1.0M KOH and I would have only KF at the equivalence point.l But if I take a larger amount of KOH the solution will have an excess of KOH and be basic. If I take less than that HF will be in excess and the solution will be a buffered solution. Does the problem say you take equal volume of each What about posting the complete question.
The hint says the acid and base will react completely until one or both is completely used up.
HF and KOH react in a 1:1 ratio. So if all of the KOH reacts (1.0 M) then the amount of HF that reacts must also be 1.0 M. The amount of KF formed is also equal to the amounts of HF and KOH that react because of the reaction stoichiometry.