# Buffer solution

## Homework Statement

If the initial buffer pH is 4.45, what is the pH when 1.00 mL NaOH is added to 35 mL of water?
Also, if 0.0 mL NaOH is added, what is the pH then?

## The Attempt at a Solution

I have no idea how to do this...all i can think of is to change the pH to [H+] and add the moles of that with the moles formed by NaOH (i tried using OH and using its pOH and finding the pH and converting back to H+) but when i add them together and divide by the total volume it's wrong...supposedly the measured pH for the addition of 1.00 ml is 11.14 and for the 0.00 added it's 4.73..thanks

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Borek
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## Homework Statement

If the initial buffer pH is 4.45, what is the pH when 1.00 mL NaOH is added to 35 mL of water?
You are not given buffer concentration, nor buffer type? Then there is no answer to this question.

Also, if 0.0 mL NaOH is added, what is the pH then?
This one is easier. Once you add 0.0 mL of a strong base, pH doesn't change. But I suppose that's just a typo :smil:

symbolipoint
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