When \[C{{O}_{2}}\] dissolves in water, the following equilibrium is established \[C{{O}_{2}}+2{{H}_{2}}O\rightleftharpoons {{H}_{3}}{{O}^{+}}+HC{{O}_{3}}^{-}\] for which the equilibrium constant is \[3.8\times {{10}^{-7}}\] and pH = 6.0. The ratio of \[\left[ HC{{O}_{3}}^{-} \right]\] to \[[C{{O}_{2}}]\] would be

• A. \[3.8\times {{10}^{-13}}\]       
• B. \[3.8\times {{10}^{-1}}\]
• C.  6.0                              
• D. 13.4