pH=7.40,K_(1)" of "H_(2)CO_(3)=4.5times10^(-7)." What will be the ratio of "[HCO_(3)]" to "[H_(2)CO_(3)]?

pH = 7.4 , K_1 of H_2CO_3 = 4.5 X 10^(-7) . What will be the ratio of [HCO_3^-] to [H_2CO_3]

When CO_(2) dissolves in water, the following equilibrium is established : for which K_(c )=3.95xx10^(-7) and pH = 6.0. What would be the ratio of [HCO_(3)^(-)]//[CO_(2)] ?

When CO_(2) is bubbled in excess of water , the following equilibrium is established . CO_(2) + 2 H_(2)O hArr H_(3) O^(+) + HCO_(3)^(-) K_(c) = 3.8 xx 10^(-7) , pH = 6 What would be the [HCO_(3)^(-)] //[CO_(2)] ?

(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))

When CO_(2) is bubbled in excess of water, the following equilibrium is establisheed. CO_(2) + 2H_(2)O hArr H_(3)O^(+) + HCO_(3)^(-) K_(c) = 3.8 xx 10^(-7), p^(H) = 6 What would be the [HCO_(3)^(-)]//[CO_(2)]

Acid rain takes place dur to combination of acidic oxides with water and it is an environmental concern all over the world. Assuming rain water is uncontaminated with HNO_(3) or H_(2)SO_(4) and is in equilibrium with 1.25 xx 10^(-4) atm CO_(2) . The Henry's law constant (K_(H)) is 1.25 xx 10^(6) "torr". K_(a_(1)) of H_(2)CO_(3) = 4.3 xx 10^(-7) What is the pH of neutral rain water ?

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