The first and second ionization constants of H_2 X are 2.5 x 10^-8 and 1.0 x 10^-13 respectively. The concentration of X^2- in 0.1 M H_2 X solution is \_\_\_\_ x 10^-15 M. (Nearest Integer)

H_2 X H^++ HX^- 0.1-x x+y x-y 2.5 x 10^-8=frac( x+ y)( x- y)0.1- x HX^- H^++ X^2-, x-y x+y y 1 x 10^-13=frac( x+ y)( y) x- y Approximate : K_ a_1 gg K_ a_2 => So x gg y. x+ y = x, x- y = x 10^-13=(x * y / x) y=10^-13\ [ X^2-]=10^-13 [ X^2-]=100 x 10^-15

The first and second ionization constants of H 2 X are ... | null (Chemistry)

\mathrm{H}_{2} \mathrm{X} \rightleftharpoons \mathrm{H}^{+}+\mathrm{HX}^{-}

\\0.1-x \quad x+y \quad x-y\\

2.5 \times 10^{-8}=\frac{(\mathrm{x}+\mathrm{y})(\mathrm{x}-\mathrm{y})}{0.1-\mathrm{x}}\\

\mathrm{HX}^{-} \rightleftharpoons \mathrm{H}^{+}+\mathrm{X}^{2-}

\\x-y \quad x+y \quad y\\

1 \times 10^{-13}=\frac{(\mathrm{x}+\mathrm{y})(\mathrm{y})}{\mathrm{x}-\mathrm{y}}\\

Approximate :

\mathrm{K}_{\mathrm{a}_{1}} \gg \mathrm{~K}_{\mathrm{a}_{2}} \Rightarrow

\mathrm{x} \gg \mathrm{y}.\\

\mathrm{x}+\mathrm{y} \approx \mathrm{x}, \mathrm{x}-\mathrm{y} \approx \mathrm{x}\\

10^{-13}=\frac{x \cdot y}{x}\\

\mathrm{y}=10^{-13}

\left[\mathrm{X}^{2-}\right]=10^{-13}\\

\left[\mathrm{X}^{2-}\right]=100 \times 10^{-15}

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