Buffer solution

  • Thread starter lha08
  • Start date
  • #1
164
0

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?

Homework Equations





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
 

Answers and Replies

  • #2
Borek
Mentor
28,631
3,105

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:
 
  • #3
symbolipoint
Homework Helper
Education Advisor
Gold Member
6,112
1,159
Problem description is incomplete. Are you trying to solve a general problem?
 

Related Threads on Buffer solution

  • Last Post
Replies
1
Views
3K
  • Last Post
Replies
9
Views
3K
  • Last Post
Replies
1
Views
10K
  • Last Post
Replies
1
Views
1K
  • Last Post
Replies
12
Views
9K
  • Last Post
Replies
2
Views
2K
  • Last Post
Replies
2
Views
11K
  • Last Post
Replies
5
Views
26K
  • Last Post
Replies
2
Views
868
  • Last Post
Replies
2
Views
3K
Top