Ethanoic acic has a dissociation constant of 1.85 x 10^-5 at 25C.

If 25 cm^3 of 0.1M ethanoic acid solution is mixed with 12.5cm^3 sodium hydroxide solutionm, what is the pH of the resulting solution?

Limxy, since this is obviously a homework question, I've moved the thread to the appropriate forum.

 

Now, since we don't give answers here, can you share with us what you've done? Are you familiar with what pH is and have you been taught about ICE tables at all?

hypervalent_iodine, I hope you won't mind if I give my input here and there as well. I love helping people with problems. (:

 

If you are familiar too with what the properties of acids and bases are according to the Bronsted-Lowry theory, it will be a huge help in getting started on the problem.

Of course you can; the more the merrier.

 

Also, you'll find that teaching to others is an excellent way to learn a subject. I would absolutely encourage you to help out in the homework questions, etc., since I know it would help you with your own studies.

Ethanoic acic has a dissociation constant of 1.85 x 10^-5 at 25C.

If 25 cm^3 of 0.1M ethanoic acid solution is mixed with 12.5cm^3 sodium hydroxide solutionm, what is the pH of the resulting solution?

 

Alright so what's the definition of pH? I'm sure you know that there is a [H⁺] term in there somewhere. If [H⁺] equals some value for the ethanoic acid solution, what will adding sodium hydroxide (remember it's a strong base) do to that value?

 

Now tie that in to the definition of dissociation constant.