“Calculate the H3O+ concentration and pH of the solution that results when 22.0mL of 0.15M acetic acid is mixed with 22.0 mL of 0.15 M NaOH”.
First thing - volumes ond concentration are identical. That means you get just solution of sodium acetate and you must concentrate on hydrolysis (as already pointed out by AWK).
Ok…. I think that this will eventually be an I.C.E. problem but first I need to get to a net equation? The book talks about adding the acid to water, then the base to water and going from there. First of all, where do they get the water and second of all, is it alright to just add NaOH + CH3CO2H --> H2O + CH3CO2- or is that ignoring steps and going to cause problems later on?
All is solved in water, there is plenty of water around
You have lost Na+ on the right side of the equation. Besides, you should either write everything in ionic form, or not. So it is either
NaOH + CH3CO2H --> H2O + CH3CO2Na
or
Na+ + OH- + CH3CO2H --> H2O + CH3CO2- + Na+
Why CH3CO2H? Because it is a weak acid and it is dissociated only partially. NOw, look at both sides - there is Na+ floating here and there. Cancel it out and you will get net ionic reaction for the problem.
Another question, do I use the reciprocal of Kb for CH3CO2 since it is the resulting conjugate base of acetic acid?
Be more specific, I have no idea what you are writing about.
Am I properly ignoring Na, since it doesn’t affect the pH, or do I need to have it in the equation?
You may safely ignore it. See above.