pH
 

A sample of 25.0ml of 0.10 M lactic acid (HC3H5)3 , pKa =3.850 is titrated with 0.10 NaOH aquation solution. What is the volume of the base needed to reach equivalence point?what is the Ph at the equivalance point? help please!!!!!!!!!

Once you will sove the formic acid question this one will be a breeze :)

Besides, these calculations are descibed in the pH cheat sheet, you just have to understand what you have to calculate.

Volume of acid solution => moles of acid => moles of base => volume of base is the process for the first part. The second part requires some equation; can't remember off the top of my head. Henderson-Hasselbach?

Just use some bromthymol blue as a Ph indicator.

Use the indicator to know when you've reached the equivalence point. The use: pH=pKa + log([H+]/[HA](undisociated acid))

I believe that is how you do it.

No, HH can be used before equivalence point. At equivalence you have just a solution of sodium lactate - salt of weak acid and strong base, so you calculate pH from lactate hydrolyzis.

Check titration curve calculation lecture.