DOC PREVIEW
UT CH 302 - Lecture Slides
Type Miscellaneous
Pages 16

This preview shows page 1-2-3-4-5 out of 16 pages.

Save
View full document
View full document
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience
View full document
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience
Premium Document
Do you want full access? Go Premium and unlock all 16 pages.
Access to all documents
Download any document
Ad free experience

Unformatted text preview:

Principles of Chemistry II © Vanden BoutExam Wednesday NightPlaceUTC 2.102A Last name A-KUTC 2.112A Last name L-ZTime7:30-9:00We will start right at 7:30We will end right at 9:00get there earlyPrinciples of Chemistry II © Vanden BoutMakeup Exam Sunday nightPlaceTBDTime6:30-8:00Anyone who would like to can take the makeup examYou cannot take bothPrinciples of Chemistry II © Vanden BoutWhen are you planning to take the examA. Wednesday nightB. Sunday nightPrinciples of Chemistry II © Vanden BoutConverting pH and pOHKw = [H+][OH-]log(Kw) = log([H+][OH-])log(Kw) = log[H+]+ log[OH-]log(10-14) = log[H+]+ log[OH-]-14 = -pH - pOH14 = pH + pOHPrinciples of Chemistry II © Vanden BoutFor the next exam Which of the following would be more helpfulA. More worksheetsB. Suggested back of the book problemsC. Suggested problems on eduspaceD. otherPrinciples of Chemistry II © Vanden BoutBuffer Both HA and A-HA(aq) H+(aq) + A-(aq)HA H+ A-ICE[HA]0-x[HA]0 -xO+x+xKa =[H+][A-][HA][A-]0+x[A-]0 + x(x)([A-]0+x)[HA]0 -x=really 10-7assuming x << C=(x)([A-]0)[HA]0Principles of Chemistry II © Vanden BoutpH in a buffer solution[H+][A-]0[HA]0Ka ≈we have approximated a small change[H+][A-]0[HA]0log(Ka) ≈log = log[H+] +log[A-]0[HA]0pKa = pH - log[A-]0[HA]0Principles of Chemistry II © Vanden BoutpKa = pH - log[A-]0[HA]0initial weak acidinitial conjugate base[A-]0=[HA]0equal acid/basepH = pKa-log[A-]0[HA]0=0[A-]0 < [HA]0more acidpH < pKa-log[A-]0[HA]0> 0[A-]0 > [HA]0more basepH > pKa-log[A-]0[HA]0< 0Principles of Chemistry II © Vanden BoutWhat is the pOH of a 0.01M solution of HClO4?" A." " 1 " B." " 2" C." " 7"" D." " 10" E." " 12[H+] = 10-2 pH = 2 pOH =12Principles of Chemistry II © Vanden BoutStrong Acids and Bases"Strong" means one thingThe substance dissociates 100% in waterStrong AcidHCl(aq) H+(aq) + Cl-(aq)Ka =[H+][Cl-][HCl]≈∞Strong ElectrolyteNaCl(s) Na+(aq) + Cl-(aq)Ksp = [Na+][Cl-] ≈∞Principles of Chemistry II © Vanden BoutWhat is the pH of a 10-10M solution of HCl?" A." " 2 " B." " 4" C." " 7"" D." " 10" E." " very slightly less than 7Principles of Chemistry II © Vanden BoutWhen do we get into problems with approximationsWhat approximations are we makingTypically that [H+]0 = 0 no H+ at the startnot a problem along as the concentration of acid or base is large enoughwhat is large enough big compared to 10-7Principles of Chemistry II © Vanden BoutWhen do we get into problems with approximationsWhat approximations are we makingThat the change is smallwhat is required for thisK should be small (weak acid, weak base)The initial concentration should be largeC-x is approximately Cthis is a comparison between C and xPrinciples of Chemistry II © Vanden BoutFor which of this will our approximations fail?" A." " 0.1 M solution of sodium acetate " B." " 1 M solution of HF " C." " 10-6 M solution of benzoic acid"" D." " 0.5 M solution of HCl" E." " 0.2 M solution of NaOHPrinciples of Chemistry II © Vanden BoutThe pKa of HF is 3.18. What is the pH of solution of100 mL of 0.1 M HF and 100 mL of a 0.2 M NaF?" A."" slightly less than 3.18 " B."" 3.18 " C."" slightly more than 3.18"Principles of Chemistry II © Vanden BoutpKa = pH - log[A-]0[HA]0initial weak acidinitial conjugate baseif the initial acid and base are similar in concentration than the pH is close to the pKaFor the pH to be 1 unit different than the pKa the difference in concentrations must be at least 10


View Full Document

UT CH 302 - Lecture Slides

Type: Miscellaneous
Pages: 16
Documents in this Course
Exam 2

Exam 2

6 pages

Exam 3

Exam 3

8 pages

Acids

Acids

21 pages

Exam 3

Exam 3

7 pages

SYLLABUS

SYLLABUS

15 pages

ex1s08

ex1s08

11 pages

Load more
Download Lecture Slides
Our administrator received your request to download this document. We will send you the file to your email shortly.
Loading Unlocking...
Login

Join to view Lecture Slides and access 3M+ class-specific study document.

or
We will never post anything without your permission.
Don't have an account?
Sign Up

Join to view Lecture Slides 2 2 and access 3M+ class-specific study document.

or

By creating an account you agree to our Privacy Policy and Terms Of Use

Already a member?