Calculating the pH of a Buffer Solution
My Question is from the F325 June 2012 A2 Exam, Found here http://ocr.org.uk/Images/131289-question-paper-unit-f325-equilibria-energetics-and-elements.pdf.
My issue is with Question 3 c ii)
I cant calculate the pH correctly, the answer is 4.22 but for the life of me even looking at the mark scheme I dont see where the numbers come from. Can anyone give me a proper explanation?
-Ere
My issue is with Question 3 c ii)
I cant calculate the pH correctly, the answer is 4.22 but for the life of me even looking at the mark scheme I dont see where the numbers come from. Can anyone give me a proper explanation?
-Ere
Whoops. Sorry. I only read part ii and didn't bother reading part i. Oh the shame.
Work out the amount of acid (n=c.v=0.250x50.0/1000)
The amount of NaOH (=0.050x50.0/1000)
Then subtract the second from the first, which will give you the number of moles of acid left after partial neutralisation
The number of moles of butanoate is equal to the number of moles of hydroxide
The rest, you should be able to do (now [H+] =/= [A-])
Work out the amount of acid (n=c.v=0.250x50.0/1000)
The amount of NaOH (=0.050x50.0/1000)
Then subtract the second from the first, which will give you the number of moles of acid left after partial neutralisation
The number of moles of butanoate is equal to the number of moles of hydroxide
The rest, you should be able to do (now [H+] =/= [A-])
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