Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter17: Equilibrium
Section: Chapter Questions
Problem 1ALQ: Consider an equilibrium mixture of four chemicals (A. B. C. and D. all gases) reacting in a closed...
Related questions
Question
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff7e0b628-1887-4036-8cfa-486903c53c1e%2F6dac2021-b276-4ab9-b65c-167f55dad436%2Fp0co35q_processed.jpeg&w=3840&q=75)
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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