A weak acid HA has a Kₐ of 1.00 × 10^{-5} . If 0.100,mol of this acid is dissolved in one litre o

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6-2.Equilibrium-II (Ionic Equilibrium)

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A weak acid $HA$ has a $K_a$ of $1.00 \times 10^{-5} $. If $0.100\,mol$ of this acid is dissolved in one litre of water the percentage of acid dissociated at equilibrium is closest to.....$\%$

A

$0.100$

B

$99$

C

$1$

D

$99.9$

Solution

$\mathrm{K}_{\mathrm{a}}=\mathrm{C} \alpha^{2}$

$\Rightarrow 10^{-5}=0.1 \times \alpha^{2}$

$\Rightarrow 10^{-2}=\alpha$

$\Rightarrow 1 \%=\alpha$

Standard 11

Chemistry

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