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First! Make sure you know you strong acids and bases.

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First! Make sure you know you strong acids and bases.

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Remember to not get scared! sometimes short is not better!

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Calculate the Ph in the titration of 40 ml of 0.150M acetic acid  by sodium hydroxide after the addition to the acid solution of:
A) 15 ml of 0.150M NaOH
B) 40 ml of 0.150M NaOH
C) 60 ml of 0.150M NaOH

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Determine with what you are working

CH3COOH <-> H^+  +CH3COO^-  = weak acid
NaOH -> Na^+ + OH^- = second group (Strong Base)
@ 150 M
a) 15ml < 40ml = before (buffer)
b) 40ml = 40ml = at (salt)
c) 60 ml > 40 ml = after (excess)

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Step 1) Find moles for acid and bases
NaOH= 15ml x 0.150M = 2.25 mmol
CH3COOH= 40ml x 0.150m = 6 mmol
* Decide whether it's easier to work with ml and mmol or L and Mol.
Print or have in hand your Ka table

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Remember to choose the correct pH formula.

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Remember to choose the correct pH formula.

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Choosing the wrong pH formula will take you all the way back so be really careful and determine what you have and label it!

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Choosing the wrong pH formula will take you all the way back so be really careful and determine what you have and label it!

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Treat like a buffer.
- Calculate moles of both acid and base.
- Treat problem just like a buffer problem.
- Use Henderson- Hasselbalch to calculate pH.

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Treat like a salt problem.
- Calculate moles of acid/base in the flask.
- Calculate [M] using total volume now in flask.
- Salt with go trough hydrolysis.
- Use ion that controls pH to set up the ice table.
- Calculate [M].
- Calculate the conjugate Ka or Kb.
- Calculate pH.

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Treat like an excess problem.
- Calculate moles of acid/base.
- Subtract moles.
- Calculate [M] of excess moles using total volume in L.
- Calculate pH.

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1- You will always need to determine the moles of acid and base.
From there it will much easier to determine the kind of problem and you will know how to treat it.