The percent dissociation for a weak acid is given by the following relationship: % Dissociation =...
The percent dissociation for a weak acid is given by the following relationship:
% Dissociation =
![\frac{[A^-]}{[HA]_{0}}\cdot 100](http://img.homeworklib.com/questions/8ed40bc0-57ca-11eb-94b5-61d09f7e12ff.gif?x-oss-process=image/resize,w_560)
for HA + H2O ? H3O+ + A-
Show mathematically that doubling the initial concentration of weak acid lowers the % dissociation. Hint: Start with [HA]o and solve ICE problem for this initial condition, then do the same for [HA]o/2.
*It seems obvious to me that doubling the initial concentration would lower the % dissociation based on the% dissociation equation. I'm having trouble incorporating the ICE tables. Can anyone show me how to do that?
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The percent dissociation for a weak
acid is given by the following relationship:
% Dissociation =...
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is...
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H2O ⇌ H3O+ + A- What is the percent ionization of the acid?
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is...
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H20 = H30* + A What is the percent ionization of the acid? 0.155% 2.34% 0.0993% 0.782% O 0.0118%
1. Consider the following equilibrium for the dissociation of lactic acid, HC3H5O3 (a weak acid): HC3H5O3...
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- Given this concentration n ratio what is the pH (show work), Ka and percent ionization...
- Given this concentration n ratio what is the pH (show work),
Ka and percent ionization of this species
( HA+H2O← → A- + H3O+ , acid. Initial concentration: 0.01
mol/L)
HA: 9.77x10^-3 mol/L
H2O: 55.6 mol/L
A- : 2.34x10^-4 mol/L
H3O+: 2.34x10^-4 mol/L
- Also if we increase the initial concentration how does this
affect the ph n the Ka such as increasing it to .1mol/L
- is you have initial concentration of .001 if u increase
strength what...
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It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
A weak acid has an initial concentration of 0.0415 M. After undergoing dissociation the pH is 5.31. HA + H20 = H30* + A What is the percent ionization of the acid? 0.155% 2.34% 0.0993% 0.782% O 0.0118%
- Given this concentration n ratio what is the pH (show work),
Ka and percent ionization of this species
( HA+H2O← → A- + H3O+ , acid. Initial concentration: 0.01
mol/L)
HA: 9.77x10^-3 mol/L
H2O: 55.6 mol/L
A- : 2.34x10^-4 mol/L
H3O+: 2.34x10^-4 mol/L
- Also if we increase the initial concentration how does this
affect the ph n the Ka such as increasing it to .1mol/L
- is you have initial concentration of .001 if u increase
strength what...
In the rice table for the dissociation of acetic acid, what is the expression for acetic acid taken directly from the equilibrium line of your ICE table? Do not use the x is small assumption. [HAC]; is the initial concentration of acetic acid. Ох O [HAC) O [HAc); -* O not included in the rICE table because it is a (s) or (I) O X - [HAC)
It's a weak acid strong base titration
Experiment 4: Identification of an unknown acid by titration Page 2 of 15 Background In this experiment, you will use both qualitative and quantitative properties to determine an unknown acid's identity and concentration. To do this analysis, you will perform a titration of your unknown acid sample-specifically a potentiometric titration where you use a pH meter and record pH values during the titration, combined with a visual titration using a color indi- cator...
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