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^+, HCO_3^- , and CO_3^(2-) in a 0.01 M solution of carbonic acid if the pH of the solution is 4.18. k_1 = 4.45 xx 10^(-7), k_2 = 4.69 xx 10^(-11)

Calculate the pH of 0.010M NaHCO_(3) solution. K_(1)=4.5xx10^(-7) , K_(2)= 4.7xx10^(-11) for carbonic acid.

Calculate pH solution: 0.1 M CH_(3)COOH (K_a=1.8 xx 10^(-5))

(a) Prove that in the aqueous solution of NH_(4)CI concentration of H_(3)O^(+) ions is sqrt(K_(h) xx c) . (b) Find out the ration of [[HCO_(3)^(-)]]/[[H_(2)CO_(3)]] in the aqueous solution of carbonic acid whose pH is 7.4. (K_(a) = 4.5 xx 10^(-7))