Lecture 12--Intro to Buffers

Lecture 12--Intro to Buffers - cH 302 53210 Introduction to...

Info iconThis preview shows pages 1–3. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: cH 302 53210 Introduction to Buffers October 30" 2009 Dilute Strong Acids When the concentration of an acid is below l0-6 M, the autoprotolysis of water will make a significant contribution to the [H3O*1 concentration (and hence the pH). Using our traditional formula in these situations will lead to false answers. Example: Compute the pH F[tl+ fxl0qA of a I F\* + lxtD h \{=-\ of HCl. l/l ^,^l; ,1\f lY %Y;^"t4* The solution: Take the autoprotolysis of water into account. #r-ur. u a/)')u method called the systematic treatment of equilibriumto do this. Steps: 1. 2. Identifo all the major species. write charge balance equation [positively charges] : [Negative Charges]. Write the Water Equilibrium. write the mass balance equations (not necessary here). Solve for [H*]. 3. 4. 5. Derivation: @ l-\rO --+ H* oq u- Hd+ H++ C'o'- guulo <--+ ;-911o C"u lou.-J= L flttl t H-f 'z = C.sts-f r+11:" C.o /o 'l c6 $*c ,i*y@ tN&' Final Equation' [". f' --o 0uf,+i1'' Using the quadratic formula: Example: Compute the pH...
View Full Document

This note was uploaded on 01/30/2010 for the course GOV 312L taught by Professor Madrid during the Fall '07 term at University of Texas.

Page1 / 6

Lecture 12--Intro to Buffers - cH 302 53210 Introduction to...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online