What would the concentration of CH3C00 be at pH 5.3 if 0.1M CH3CO0H was adjusted to that pH. 1) pH = pK + Log [A ] %3D [HA] 2) CH3C00H CH3C00 + H 3) Find equilibrium value of [A ]i.e [CH3C00 ] 4) pH = 5.3; pK = 4.76 5) Let X = amount of CH3C00H dissociated at equilibrium (A ] = [X] [HA] = [0.1 - X] 6) 5.3 = 4.76 + Log IXI [0.1- X]
What would the concentration of CH3C00 be at pH 5.3 if 0.1M CH3CO0H was adjusted to that pH. 1) pH = pK + Log [A ] %3D [HA] 2) CH3C00H CH3C00 + H 3) Find equilibrium value of [A ]i.e [CH3C00 ] 4) pH = 5.3; pK = 4.76 5) Let X = amount of CH3C00H dissociated at equilibrium (A ] = [X] [HA] = [0.1 - X] 6) 5.3 = 4.76 + Log IXI [0.1- X]
Chapter31: Introduction To Analytical Separations
Section: Chapter Questions
Problem 31.17QAP
Related questions
Question
What would the concentration of CH3COO be at pH 5.3 if 0.1M CH3COOH was adjusted to that pH.
![Quiz No. 3
What would the concentration of CH3C00 be at pH 5.3 if 0.1M
CH3C00H was adjusted to that pH
1) pH = pK + Log [A ]
%3D
[HA]
2) CH3C00H CH3C00 +H
3) Find equilibrium value of [A ]i.e [CH3C00 ]
4) pH = 5.3; pK = 4.76
5) Let X = amount of CH3COOH dissociated at equilibrium
[A ] = [X]
[HA] = [0.1 - X]
6) 5.3 = 4.76 + Log [XI
[0.1- X]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F951d688d-c98d-4052-aeaa-7ebbd1a43088%2Fedfea1b3-c3ed-4c5d-a6af-bfc3910f51fc%2Fjp6cod5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Quiz No. 3
What would the concentration of CH3C00 be at pH 5.3 if 0.1M
CH3C00H was adjusted to that pH
1) pH = pK + Log [A ]
%3D
[HA]
2) CH3C00H CH3C00 +H
3) Find equilibrium value of [A ]i.e [CH3C00 ]
4) pH = 5.3; pK = 4.76
5) Let X = amount of CH3COOH dissociated at equilibrium
[A ] = [X]
[HA] = [0.1 - X]
6) 5.3 = 4.76 + Log [XI
[0.1- X]
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