You have a solution of 0.15M Ba(OH)2 and a solution of H2SO4 whose concentration

Question

You have a solution of 0.15M Ba(OH)2 and a solution of H2SO4 whose concentration you want to determine. You start with 25 ml H2SO4 in the Erlenmeyer and titrate in the Ba(OH)2. At the end of the titration, you find that you have used 20.4 ml Ba(OH)2 and an additional 2.2 ml H2SO4 because you hadto back-titrate.

a) How many moles of OH- are in 20.4 ml of a 0.15 Ba(OH)2 solution?
b) What's [H2SO4]?

I don't understand titration but I do know that H2SO4 is sulfuric acid which I guess is start. Can someone explain how find the amount of moles of OH-?

Explanation / Answer

I have uploaded a picture of the solution here http://i.imgur.com/yOfzSFp.jpg

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