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Homework Help: Titration of Sr(OH)2 by HCl. What is the pH?

  1. Jan 30, 2010 #1
    1. COnsider the titration of 80.0 mL of 0.100 M Sr(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added.

    a. 0.0 mL
    b. 20 mL
    c.80 mL

    2. Relevant equations
    Henderson–Hasselbalch equation or direct -log



    3. The attempt at a solution
    a) before I added any HCl, I just did the -log(.1)=1 14-1=13 is that correct?
    B)i know it is a strong acid & strong base. & i cannot use pKa for Henderson–Hasselbalch equation. what else can i do?
    Sr(OH)2 + 2HCl -> 2H2O + Sr
    0.092 ...... 0.0016 ....... 0
    -0.008 ..... -0.0016 ...... +0.008
    0.0912 ....... 0 ....... . 0.008
     
  2. jcsd
  3. Jan 30, 2010 #2

    Borek

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    Staff: Mentor

  4. Feb 1, 2010 #3
    in this do i also have to multiply the HCL molarity by two or only the Sr(OH)2
    for letter b i got a pH of 0 and when i did it with 30 mL i got a higher pH...is that normal?
     
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