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how to find culculated ka and literature Ka for acetic acid

how to find culculated ka and literature Ka for acetic acid

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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how to find culculated ka and literature Ka for acetic acid？
For acetic acid, at equilibrium: loe alee enolnv to llg sdi pnni od I Ka= [H3O*][CH3CO2 /[CH3 CO2 H] -1.8x10 In this case, you know Ka value. This is something you would look up in any chemistry book. Set up your calculations:ollal uen so psd.iblos od liw oiulor a 200ni [H3O'][CH3CO2 V[CH3 CO2 H] =1.8x105, noibulo ne inmusn s mot of pson lliw DRed anona We know that [H3O*]= [CH3CO2¯], because it's a weak acid and the percent of the acetic acid molecules that dissociate is so small, it is usually satisfactory to assume the initial acid concentration equals the equilibrium concentration of the undissociated weak acid. Also, it was given that [CH3CO2H] =1.0x10! M riw toibana ol enoitoson to 20gy Tuoi sri lo zoiamoo Now you can solve for [H3O*]: SCIic OL pazic tups noiteloz iloe zatorioto Hq sli yinimsisCIE slds 1- I CH3COOH]=1.0xW' 1. [H3O*]/(1.0×10' M)=1.8×10-5 2. [H30*]=0.0013 moitensiqx 3. pH=-log[H3O*] w1ad 4. pH=2.9 bosi Holsdaibibs) lag lo sme CH COOH. Table 2. Preparing acetic acid solutions and determining pH OHOs expected. Calculated Ka of acetic acid based on measured pH acetic acid Concentration Measured Theoretical pH Literature Ka of of acetic acid, pH M 0.IM 2.86 0.5/M 8.20 Hg bou nwsd 0.00IM 3.70 0.000IM 4.17 ad pbloow oy tom
Transcribed Image Text:For acetic acid, at equilibrium: loe alee enolnv to llg sdi pnni od I Ka= [H3O*][CH3CO2 /[CH3 CO2 H] -1.8x10 In this case, you know Ka value. This is something you would look up in any chemistry book. Set up your calculations:ollal uen so psd.iblos od liw oiulor a 200ni [H3O'][CH3CO2 V[CH3 CO2 H] =1.8x105, noibulo ne inmusn s mot of pson lliw DRed anona We know that [H3O*]= [CH3CO2¯], because it's a weak acid and the percent of the acetic acid molecules that dissociate is so small, it is usually satisfactory to assume the initial acid concentration equals the equilibrium concentration of the undissociated weak acid. Also, it was given that [CH3CO2H] =1.0x10! M riw toibana ol enoitoson to 20gy Tuoi sri lo zoiamoo Now you can solve for [H3O*]: SCIic OL pazic tups noiteloz iloe zatorioto Hq sli yinimsisCIE slds 1- I CH3COOH]=1.0xW' 1. [H3O*]/(1.0×10' M)=1.8×10-5 2. [H30*]=0.0013 moitensiqx 3. pH=-log[H3O*] w1ad 4. pH=2.9 bosi Holsdaibibs) lag lo sme CH COOH. Table 2. Preparing acetic acid solutions and determining pH OHOs expected. Calculated Ka of acetic acid based on measured pH acetic acid Concentration Measured Theoretical pH Literature Ka of of acetic acid, pH M 0.IM 2.86 0.5/M 8.20 Hg bou nwsd 0.00IM 3.70 0.000IM 4.17 ad pbloow oy tom
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