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

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.

To determine the final concentrations in the given reaction and set up the problem, we can use the concept of stoichiometry and the stoichiometric ratio between the reactants and products.

In the balanced chemical equation:

HF(aq) + KOH(aq) <-> KF(aq) + H2O(l)

we can see that 1 mole of HF reacts with 1 mole of KOH to produce 1 mole of KF and 1 mole of H2O.

To set up the problem, we need to consider two scenarios:

1. If the reaction goes to completion: In this case, all the reactants will react entirely, and none of them will be left over. So, we can start by subtracting the initial concentrations of HF and KOH from each other to find the limiting reactant. The limiting reactant is the reactant that will be entirely consumed in the reaction. The other reactant will be in excess.

In this case, since both HF and KOH have initial concentrations, we need to compare their concentrations to identify the limiting reactant.

HF (initial concentration) - KOH (initial concentration) = 2.0 M - 1.0 M = 1.0 M

Since the difference is positive, HF is the limiting reactant.

So, we can write down the change in concentrations as follows:

HF: -2.0 M (since it is entirely consumed)
KOH: -1.0 M (since its concentration is assumed to be entirely consumed)
KF: +2.0 M (since 1 mole of HF produces 1 mole of KF)
H2O: +1.0 M (since 1 mole of HF produces 1 mole of H2O)

2. If the reaction does not go to completion: In this case, there would be an excess of either HF or KOH, meaning some of it would be left over after the reaction reaches equilibrium. To determine the final concentrations, we need additional information, such as the equilibrium constant (Kc) for the reaction or the degree of completion of the reaction.

Once you have determined the final concentrations for each species, you can compare them to decide which option best describes the final solution.