Below is the question that I am working on. Will someone check my work for part (a) and (b). I am also in need of some help on parts (c) and (d). The questions I Have are below.
The question is: A person mixes 50.0ml of 0.115 M HAc with 25.0 ml of 0.182 M NaOH and then dilutes the resulting mixture to 100.0ml.
a. Write the net ionic equation-----HC2H3O2(aq) + NaOH
NaC2H3O2(aq) + H20[/b]
b. Determine which reagent is in excess. I determined that it is the HC2H3O2 that is in excess and the NaOH that is the limiting reagent.
c. Calculate the concentration of HC2H3O2, C2H3O2 and Na in the final solution. [NaAc] [H2o]
[HAc] [NaOH] = [ 0.0455-x] [0.0455-x] =
I know that the Ka for HC2H3O2 is 1.8x10^-5
I am not sure how to figure out the number that I should make the above equation that I figutred out equal to. If someone could explain this to me that would be great.
d. Calculate the concentration H+ (aq) in this solution.
I know that in this problem I am dealing with:
H+ C2H3O2 Na OH and H2O.
The H+ from the C2H3O2 would be the only major contributor of H+ ions to the initial solution because the H2O acts either as a weak acid or weak base. These are my thoughts on this problem so far. I am not exactly sure of where to go from here.
I am thinking that maybe I should set up the problem where
[H+] [C2H3O2] = Ka for HC2H3O2 Ka =1.8*10^-5
Does this make sense to you? Then I would calculate it out for x where H+ equals x.
Thank you for your time and *delete me*!!
It is very much appreciated!