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Topic: Titration 2  (Read 2696 times)

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Offline Sayanthan

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Titration 2
« on: May 19, 2010, 10:56:38 AM »
When 20 mL of 0.300 mol/L HC2H3O2(aq) is titrated with 20 mL of 0.300 mol/L NaOH(aq), what is the pH of the solution at equivalence point?
Please include steps to completing this problem and thanks in advance. :)
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Offline Schrödinger

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Re: Titration 2
« Reply #1 on: May 19, 2010, 01:40:38 PM »
You need to show us your attempt. Please read forum rules
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Offline Sayanthan

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Re: Titration 2
« Reply #2 on: May 19, 2010, 10:17:32 PM »
Because the two solutions have equal molarity, and HCl and NaOH react 1:1

Total volume of solution = 20+20 = 40 ml.
What is the molarity of 0.3 mol HCl dissolved in 40ml solution:
1000/40*0.3 = 7.5M

Because [HCl] = 7.5M, [H+] = 7.5M

pH = -log [H+]
pH = -log 7.5
pH = -0.88
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Offline Borek

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Re: Titration 2
« Reply #3 on: May 20, 2010, 03:14:52 AM »
There is no HCl in this solution.

You are at the equivalence point.

http://www.titrations.info/acid-base-titration-equivalence-point-calculation
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