The dissociation constant of acetic acid is 1.6 × 1 0 - 5 . The degree of dissociation of 0.01 M acetic acid in the presence of 0.1 M HCl is equal to

For weak acid: α = Ka C α = 1 .6 × 10 − 5 10 − 2 α = 4 × 10 − 2

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ChemistryIonic EquilibriumMiscellaneous/MixedEasy2 minPYQ_2020

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The dissociation constant of acetic acid is 1.6 $\times 1 0^{- 5}$ . The degree of dissociation of 0.01 M acetic acid in the presence of 0.1 M HCl is equal to

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Answer:

Solution:

For weak acid:
$α = \sqrt{\frac{Ka}{C}}$
$α = \sqrt{\frac{1 .6 × 10^{- 5}}{10^{- 2}}}$
$α = 4 \times 10^{- 2}$

Stream:NTA_ABHYASSubject:ChemistryTopic:Ionic EquilibriumSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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