Question:
The degree of dissociation of weak acid is 7.2 x 10-4 . What is the value of it’s percent dissociation in 0.025 M solution?
The degree of dissociation of weak acid is 7.2 x 10-4 . What is the value of it’s percent dissociation in 0.025 M solution?
Updated On: May 4, 2025
- 0.80%
- 0.062%
- 8.2%
- 0.072%
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The Correct Option is D
Approach Solution - 1
Given:
α = 7.2 × 10-4
and the initial concentration of the weak acid is 0.025 M.
The percent dissociation can be calculated using the formula:
Percent dissociation = α × 100
Substituting the given value of α:
Percent dissociation = 7.2 × 10-4 × 100 = 0.072%
Therefore, the correct option is (D) 0.07%.
α = 7.2 × 10-4
and the initial concentration of the weak acid is 0.025 M.
The percent dissociation can be calculated using the formula:
Percent dissociation = α × 100
Substituting the given value of α:
Percent dissociation = 7.2 × 10-4 × 100 = 0.072%
Therefore, the correct option is (D) 0.07%.
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Approach Solution -2
Given:
α = 7.2 × 10⁻⁴
Initial concentration of weak acid = 0.025 M
Percent dissociation is calculated as: Percent dissociation =α×100
Substituting the value of α: Percent dissociation =\(7.2\times 10^{-4}\times 100 = 0.072%\) %
Thus, the correct option is (D) 0.07%.
α = 7.2 × 10⁻⁴
Initial concentration of weak acid = 0.025 M
Percent dissociation is calculated as: Percent dissociation =α×100
Substituting the value of α: Percent dissociation =\(7.2\times 10^{-4}\times 100 = 0.072%\) %
Thus, the correct option is (D) 0.07%.
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