Calculate [H_3O^{+}] in 0.02 M solution of m | vedclass

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(B) For a weak monobasic acid,the dissociation constant $K_a$ is given by $K_a = c \alpha^2$. Thus,the degree of dissociation $\alpha = \sqrt{\frac{K_

Vedclass · Accepted Answer

$6.0 	imes 10^{-4} \ M$

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(B) For a weak monobasic acid,the dissociation constant $K_a$ is given by $K_a = c \alpha^2$. Thus,the degree of dissociation $\alpha = \sqrt{\frac{K_a}{c}}$. Substituting the given values: $\alpha = \sqrt{\frac{1.8 	imes 10^{-5}}{0.02}} = \sqrt{9 	imes 10^{-4}} = 3 	imes 10^{-2}$. The concentration of hydronium ions is given by $[H_3O^{+}] = c \alpha$. $[H_3O^{+}] = 0.02 	imes 3 	imes 10^{-2} = 6.0 	imes 10^{-4} \ M$.

Calculate $[H_3O^{+}]$ in $0.02 \ M$ solution of monobasic acid if dissociation constant is $1.8 \times 10^{-5}$.

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