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The concentration of an aqueous solution of the weak acid, HA is 0.1(M). Calculate the pH and concentrations of `A^-` ion and HA at equilibrium in the solution. Given: `K_b(HA)=1.35xx10^(-3)`

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`[H_3O+]=0.02xx0.2=4xx10^(-3)(M)`
`:.pH=-log_(10)[H_3O^+]=-log(4xx10^(-3))=2.4`
`pH=1/2pK_a-1/2logc` or `2.4=1/2pK_a-1/2log0.2`
or `pK_a=4.1:.K_a=7.94xx10^(-5)`
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