posted by HELP Plz .
What is the pH of the solution created by combining 2.00 mL of the 0.10 M base[ammonia] with 8.00 mL of the 0.10 M acid[acid acid]?
I tried this problem so many times, but always got it wrong. It's a weak base and acid titration. but i don't know the method of do this type of proble
It's done with moles.
You have acid acid for the acid so I don't know which acid you are using.
mols base = M x L = 0.1 x 0.002 L = xx
mols acid = M x L = 0.1 x 0.008 L = yy
There will be xx mols salt formd.
There will be xx mols acid - yy mols base = excess acid unreacted. All of the base will be gone.
The pH will be that of the acid/salt system but we need to know the acid to proceed.
I believe he was referring to hydrochloric acid