A certain weak acid, HA, has a K, value of 3.6x10-7. Y Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B 4 → Units ? Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures, and include the appropriate units.
A certain weak acid, HA, has a K, value of 3.6x10-7. Y Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B 4 → Units ? Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures, and include the appropriate units.
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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![Percent lonization
Percent ionization can be used to quantify the extent of ionization
of an acid in solution and is defined by the following formula for
the acid HA:
Percent ionization
HA) lonized
HA initial
x 100%
Percent ionization increases with increasing K₁. Strong acids,
for which K, is very large, lonize completely (100%). For weak
acids, the percent ionization changes with concentration. The
more diluted the acid is, the greater percent ionization.
A convenient way to keep track of changing concentrations is
through what is often called an I.C.E table, where I stands for
"Initial Concentration," C stands for "Change," and E stands for
"Equilibrium Concentration." To create such a table, write the
concentrations of reactant(s) and product(s) across the top,
creating the columns, and write the rows I.C.E on the left-hand
side. Such a table is shown below for the reaction:
A+B= AB
[A] [B] [AB]
Initial (M)
Change (M)
Equilibrium (M)
A certain weak acid, HA, has a K, value of 3.6x10-7.
Part A
Calculate the percent ionization of HA in a 0.10 M solution.
Express your answer to two significant figures and include the appropriate units.
▸ View Available Hint(s)
Value
Submit
μA
Part B
HA
4 →
Value
Calculate the percent ionization of HA in a 0.010 M solution.
Express your answer to two significant figures, and include the appropriate units.
View Available Hint(s)
Units
4
?
Units
?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9213f74a-8300-4e96-b6c1-e531928eb87c%2Fa4fc73c1-1d65-42f4-bc4d-546501f02f36%2F9lvhl1s_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Percent lonization
Percent ionization can be used to quantify the extent of ionization
of an acid in solution and is defined by the following formula for
the acid HA:
Percent ionization
HA) lonized
HA initial
x 100%
Percent ionization increases with increasing K₁. Strong acids,
for which K, is very large, lonize completely (100%). For weak
acids, the percent ionization changes with concentration. The
more diluted the acid is, the greater percent ionization.
A convenient way to keep track of changing concentrations is
through what is often called an I.C.E table, where I stands for
"Initial Concentration," C stands for "Change," and E stands for
"Equilibrium Concentration." To create such a table, write the
concentrations of reactant(s) and product(s) across the top,
creating the columns, and write the rows I.C.E on the left-hand
side. Such a table is shown below for the reaction:
A+B= AB
[A] [B] [AB]
Initial (M)
Change (M)
Equilibrium (M)
A certain weak acid, HA, has a K, value of 3.6x10-7.
Part A
Calculate the percent ionization of HA in a 0.10 M solution.
Express your answer to two significant figures and include the appropriate units.
▸ View Available Hint(s)
Value
Submit
μA
Part B
HA
4 →
Value
Calculate the percent ionization of HA in a 0.010 M solution.
Express your answer to two significant figures, and include the appropriate units.
View Available Hint(s)
Units
4
?
Units
?
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