An organic monobasic acid has dissociation constant 2.25 × 1 0 − 6 . What is percent dissociation in its 0.01 M solution?

K a = 2.25 × 1 0 − 6 For a weak monobasic acid, α = c K a = 0.01 2.25 × 1 0 − 6 = 2.25 × 1 0 − 4 = 0.015 ∴ Percent dissociation = α × 100 = 0.015 × 100 = 1.5%

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ChemistryElectrochemistryConductance/conductivity/^mMedium2 minPYQ_2023

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An organic monobasic acid has dissociation constant $2.25 \times 1 0^{- 6}$ . What is percent dissociation in its $0.01 M$ solution?

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Solution:

$K_{a} = 2.25 \times 1 0^{- 6}$ For a weak monobasic acid, $α = \frac{K _{a}}{c} = \frac{2.25 \times 1 0 ^{- 6}}{0.01} = 2.25 \times 1 0^{- 4} = 0.015 ∴ Percent dissociation = α \times 100 = 0.015 \times 100 = 1.5%$

Stream:MHT_CETSubject:ChemistryTopic:ElectrochemistrySubtopic:Conductance/conductivity/^m

⏱ 2mℹ️ Source: PYQ_2023

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