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Topic: What is the pH of a solution...?  (Read 2979 times)

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Offline flaren5

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What is the pH of a solution...?
« on: July 10, 2012, 01:17:19 PM »
Good day all,

I have a question regarding pH, if anyone has any insight for the following question it would be greatly appreciated.

Question:

What is the pH of a solution prepared by mixing 25.0 ml of 0.180 M CH3COOH with 40.0 ml 0.250 M NaOH?

I'm just not sure what formula to use...
Thank you.
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Offline Borek

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Re: What is the pH of a solution...?
« Reply #1 on: July 10, 2012, 01:31:34 PM »
What reaction takes place? What are the products?
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Offline flaren5

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Re: What is the pH of a solution...?
« Reply #2 on: July 10, 2012, 01:39:11 PM »
Unfortunately I'm not too sure...
I think the reaction that takes place is a base reaction..
And the product I'm not sure... :-[
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Offline Borek

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Re: What is the pH of a solution...?
« Reply #3 on: July 10, 2012, 02:57:29 PM »
That means your problem is not "just what formula to use". It is hardly possible to answer questions about pH if you don't know anything about simple neutralization reactions.

You have an acid and a base. What are products of reactions between acids and bases?
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Offline wheresthebic

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Re: What is the pH of a solution...?
« Reply #4 on: July 10, 2012, 08:20:49 PM »
CH3COOH+NaOH ---->CH3COO- + H20(l)


-Convert to moles
-Do an ICE Chart
-Convert back to Molarity with new volume
-Then pH can be found using -log.....side note, this will give you your pOH-14.

I got 12.93. I could be wrong, I'm just learning this as well as I am in Chem2 at my university.
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Offline AWK

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Re: What is the pH of a solution...?
« Reply #5 on: July 11, 2012, 03:16:54 AM »
Result is correct.
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Offline Borek

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Re: What is the pH of a solution...?
« Reply #6 on: July 11, 2012, 03:59:57 AM »
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