Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA] initial x 100% Percent ionization For strong acids, ionization is nearly complete (100%) at most concentrations. However, for weak acids, the percent ionization changes significantly with concentration. The more diluted the acid is, the greater percent ionization. A certain weak acid, HA, has a K₂ value of 2.1x10-7. Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures. ▸ View Available Hint(s) VO Submit ΑΣΦ Part B Previous Answers * Incorrect; Try Again; 5 attempts remaining ? Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures. ▸ View Available Hint(s) ΠΑΣΦ ?
Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA] initial x 100% Percent ionization For strong acids, ionization is nearly complete (100%) at most concentrations. However, for weak acids, the percent ionization changes significantly with concentration. The more diluted the acid is, the greater percent ionization. A certain weak acid, HA, has a K₂ value of 2.1x10-7. Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures. ▸ View Available Hint(s) VO Submit ΑΣΦ Part B Previous Answers * Incorrect; Try Again; 5 attempts remaining ? Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures. ▸ View Available Hint(s) ΠΑΣΦ ?
Introduction to General, Organic and Biochemistry
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Chapter8: Acids And Bases
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Question
![Percent lonization
Percent ionization for a weak acid (HA) is determined by the following
formula:
Percent ionization =
HA ionized
x 100%
[HA] initial
For strong acids, ionization is nearly complete
(100%) at most concentrations. However, for weak acids, the percent
ionization changes significantly with concentration. The more diluted the
acid is, the greater percent ionization.
A certain weak acid, HA, has a K₂ value of 2.1x10-7.
Part A
Calculate the percent ionization of HA in a 0.10 M solution.
Express your answer as a percent using two significant figures.
▸ View Available Hint(s)
V | ΑΣΦ 3
Submit
▾ Part B
Previous Answers
* Incorrect; Try Again; 5 attempts remaining
P
IV ΑΣΦ 1
Submit
?
Calculate the percent ionization of HA in a 0.010 M solution.
Express your answer as a percent using two significant figures.
▸ View Available Hint(s)
?
%
Review | Con](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7ba769ef-ff41-4f27-8bf9-2761389b1d49%2F7fec2d4f-3d03-4eb0-afe1-9ed7e00832e0%2F7vfn545_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Percent lonization
Percent ionization for a weak acid (HA) is determined by the following
formula:
Percent ionization =
HA ionized
x 100%
[HA] initial
For strong acids, ionization is nearly complete
(100%) at most concentrations. However, for weak acids, the percent
ionization changes significantly with concentration. The more diluted the
acid is, the greater percent ionization.
A certain weak acid, HA, has a K₂ value of 2.1x10-7.
Part A
Calculate the percent ionization of HA in a 0.10 M solution.
Express your answer as a percent using two significant figures.
▸ View Available Hint(s)
V | ΑΣΦ 3
Submit
▾ Part B
Previous Answers
* Incorrect; Try Again; 5 attempts remaining
P
IV ΑΣΦ 1
Submit
?
Calculate the percent ionization of HA in a 0.010 M solution.
Express your answer as a percent using two significant figures.
▸ View Available Hint(s)
?
%
Review | Con
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