Chemical Forums

Chemistry Forums for Students => High School Chemistry Forum => Chemistry Olympiad and other competitions => Topic started by: CKabes on January 02, 2013, 04:18:25 PM

Title: Titration Math
Post by: CKabes on January 02, 2013, 04:18:25 PM

What Equations do i need to use when my acid is partially ionized?

Determine the Volume of .125 M NaOH required to titrate to the equivalence point 25 ml of a .175 M solution of a monoprotic weak acid that is 20% ionized?

Any help is greatly appreciated!
Thank you in advanced

Title: Re: Titration Math
Post by: Borek on January 02, 2013, 05:12:07 PM

20% ionized, or 20% neutralized?

Title: Re: Titration Math
Post by: CKabes on January 02, 2013, 10:46:05 PM

20% ionized

This is from the 2012 Chemistry Olympiad Regional Exam, number 34.
http://portal.acs.org/portal/PublicWebSite/education/students/highschool/olympiad/pastexams/CNBP_029727

Title: Re: Titration Math
Post by: Borek on January 03, 2013, 03:48:13 AM

What happens when you add base to the solution of the acid?