pH at the equivalence point?

Question

Need to show all appropriate calculations to estimate the pH at the equivalemce point for the titration of:
a) 0.1 M hydrocloric acid with 0.1 M sodium hydroxide
b) 0.1 M acetic acid with 0.1 M sodium hydroxide (hint: what is the concentration of the salt formed after mixing equal amount of these two reagents? you then need to determine the pH of the salt.)
c) 0.1 M ammonia with 0.1 M hydrochloric acid (hint: consider same hint as in b.)

You may need to look up pKa values.

THANK YOU!!!!!!

Answer 1

a) 7

b) pKa of CH3COOH ???????

c) pKb of NH3 ?????????????

Answer 2

NaOH and HBr are strong base and strong acid, the resulting salt is NaBr which would be completely soluble. The pH at the equivalence point should be 7. Generally you should do some work in such type of questions if the resulted salt has a low dissociation constant like CH3COONa or NH4Cl .. in such cases the dissociation constant will play the vital role in determining the pH.