(1) Setup an ICE Chart

(2) Calculate for HX^{-} and H_{3}O^{+}

$\overline{){{\mathbf{K}}}_{{\mathbf{a}}}{\mathbf{=}}\frac{\mathbf{products}}{\mathbf{reactants}}{\mathbf{=}}\frac{\mathbf{\left[}{\mathbf{H}}_{\mathbf{3}}{\mathbf{O}}^{\mathbf{+}}\mathbf{\right]}\mathbf{\left[}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{5}}{{\mathbf{CO}}_{\mathbf{2}}}^{\mathbf{-}}\mathbf{\right]}}{\mathbf{\left[}{\mathbf{C}}_{\mathbf{2}}{\mathbf{H}}_{\mathbf{5}}{\mathbf{CO}}_{\mathbf{2}}\mathbf{H}\mathbf{\right]}}}$

What is the concentration of X^{2-} in a 0.150 M solution of the diprotic acid H_{2}X? For H_{2}X, K_{a1 } = 4.5 x 10^{ - 6} and K_{a2 } = 1.2 x 10^{ - 11}.

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