[" When "Cbar(O)_(2)" dissolves in water,the following equi- "],[" librium is established,"],[CO_(2)+2H_(2)O rightleftharpoons H_(3)O^(*)+HCO_(3)-" for which the "],[" equilibrium constant is "3.8times10^(-7)" and "pH=6.0" ."],[" The ratio of "[HCO_(3)^(-)]/[CO_(2)]" is : "]

When CO_2 dissolves in water the following equilibrium is established, CO_2 + 2H_2O hArr H_3O^+ HCO_3^- for which the equilibrium constant is 3.8 xx 10^(-7) and PH =6.0 The ratio of [HCO_3]/[CO_2^-] IS :

When CO_(2) dissolves in water, the following equilibrium is established. CO_(2)+2H_(2)O hArr H_(3)O^(+) +HCO_(3)^(-) for which the equilibrium constant is 3.8 xx 10^(-6) and pH 6.0. What would be the ratio of concentration of bicarbonate ion to carbon dioxide i.e.[HCO_(3)^(-)]//[CO_(2)]

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)] ?

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)]

BaCO_(3)darr+CO_(2)+H_(2)O to Ba(HCO_(3))_(2)

BaCO_(3)darr+CO_(2)+H_(2)O to Ba(HCO_(3))_(2)

BaCO_(3)darr+CO_(2)+H_(2)O to Ba(HCO_(3))_(2)