What `%` of the carbon in the `H_(2)CO_(3)-HCO_(3)^(-)` buffer should be in the form of `HCO_(3)^(-)` so as to have a neutral solution? `(K_(a)=4xx10^(-7))`

CO_(3)^(2-) and HCO_(3)^(-) can be distingusihed by:

Find the concentration of H^(o+), HCO_(3)^(Θ) , and CO_(3)^(-2) in a 0.01M solution of carbonic acid if the pH of solution is 4.18 . K_(1) = 4.45 xx 10^(-7),K_(2) = 4.69 xx 10^(-11)

Find the concentration of H^(o+), HCO_(3)^(Θ) , and CO_(3)^(-2) in a 0.01M solution of carbonic acid if the pH of solution is 4.18 . K_(1) = 4.45 xx 10^(-7),K_(2) = 4.69 xx 10^(-11)

Find the concentration of H^(o+), HCO_(3)^(Θ) , and CO_(3)^(-2) in a 0.01M solution of carbonic acid if the pH of solution is 4.18 . K_(1) = 4.45 xx 10^(-7),K_(2) = 4.69 xx 10^(-11)

What percentage of Co_(2) is transported as bicarbonate HCO_(3)^(-) ?

HCO_(3)^(-) is conjugate base of H_(2)CO_(3) .

When the carbon-oxygen bonds in H_(3)COH,H_(2)CO, and HCO_(2)^(-) are arranged in order of increasing length, what is the correct order?