The degree of dissociation of acetic acid in a 0 .1 M solution is 1.0 × 1 0 – 2 . The p K a of acetic acid value.

K a = C α 2 1 - α = 0.1 × 1 0 - 2 2 1 - 0.01 = 1.01 × 1 0 - 5 p K a = - log ⁡ 1 × 1 0 - 5 = 5

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ChemistryIonic EquilibriumMiscellaneous/MixedEasy2 minPYQ_2020

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The degree of dissociation of acetic acid in a $0 .1 M$ solution is $1.0 \times 1 0^{- 2}$ . The $p K_{a}$ of acetic acid value.

Answer:

Solution:

$K_{a} = \frac{C α^{2}}{1 - α} = \frac{0.1 \times {(1 0^{- 2})}^{2}}{(1 - 0.01)} = 1.01 \times 1 0^{- 5}$
$p K_{a} = - \log (1 \times 1 0^{- 5}) = 5$

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

⏱ 2mℹ️ Source: PYQ_2020

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