Turn on thread page Beta
    • Thread Starter
    Offline

    0
    ReputationRep:
    Calculate the pH in titration of 25mL of 0.1M CH3COOH by NaOH after the addition to the acid solution of :
    a) 10mL of 0.1M NaOH
    b) 25mL of 0.1M NaOH
    c) 35mL of 0.1M NaOH

    so far i only got (a) by using Henderson-Hasselbalch equation. For (b) i don't know how to solve since the number of moles of CH3COOH and NAOH are the exact same, wouldn't they just cancel out? Doesn't that mean the pH of the solution would just be -log(Ka) + log(1mol/1mol) = pKa = 4.74 ??

    Meanwhile for (c) i just lost it. i don't know how to do it.

    I would really appreciate some help solving these question.
 
 
 
Reply
Submit reply
Turn on thread page Beta
Updated: May 16, 2015

1,521

students online now

800,000+

Exam discussions

Find your exam discussion here

Poll
Should predicted grades be removed from the uni application process

The Student Room, Get Revising and Marked by Teachers are trading names of The Student Room Group Ltd.

Register Number: 04666380 (England and Wales), VAT No. 806 8067 22 Registered Office: International House, Queens Road, Brighton, BN1 3XE

Write a reply...
Reply
Hide
Reputation gems: You get these gems as you gain rep from other members for making good contributions and giving helpful advice.