Turn on thread page Beta
 You are Here: Home

# i need help in solving this please help watch

1. 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

### Related university courses

TSR Support Team

We have a brilliant team of more than 60 Support Team members looking after discussions on The Student Room, helping to make it a fun, safe and useful place to hang out.

This forum is supported by:
Updated: May 16, 2015
Today on TSR

### Edexcel C3 Maths Unofficial Markscheme

Find out how you've done here

### 1,521

students online now

Exam discussions

Poll
Useful resources

## Make your revision easier

Can you help? Study Help unanswered threadsStudy help rules and posting guidelines

## Groups associated with this forum:

View associated groups

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.