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Acetic acid dissociated to $1.20 \%$ in its $0.01 \mathrm{M}$ solution. What is the value of its dissociation constant?
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$1.44 \times 10^{-6}$
Percent dissociation $=1.20 \%$
Degree of dissociation $(\alpha)=0.012$
For a weak monobasic acid, $\mathrm{K}_{\mathrm{a}}=\alpha^2 \mathrm{c}=(0.012)^2 \times 0.01=1.44 \times 10^{-6}$
Degree of dissociation $(\alpha)=0.012$
For a weak monobasic acid, $\mathrm{K}_{\mathrm{a}}=\alpha^2 \mathrm{c}=(0.012)^2 \times 0.01=1.44 \times 10^{-6}$
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