Find the correct equilibrium constant that shows the ionization constant of a weak acid HA. A)K_a = $\frac{[\mathrm{HA}]}{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{A}^{-}\right]}$ B)K_a = $\frac { \left[ \mathrm { H } _ { 3 } \mathrm { O } ^ { + } \right] \left[ \mathrm { A } ^ { - } \right] } { [ \mathrm { HA } ] \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] }$ C)K_a = $\frac { \left[ \mathrm { H } _ { 3 } \mathrm { O } ^ { + } \right] \left[ \mathrm { A } ^ { - } \right] } { [ \mathrm { HA } ] }$ D)K_a = $\frac { [ \mathrm { HA } ] \left[ \mathrm { H } _ { 2 } \mathrm { O } \right] } { \left[ \mathrm { H } _ { 3 } \mathrm { O } ^ { + } \right] \left[ \mathrm { A } ^ { - } \right] }$ E)K_a = $\frac{\left[\mathrm{A}^{-}\right]}{[\mathrm{HA}]}$

Question

Quizplus · Accepted Answer

The ionization constant of a weak acid is defined as the ratio of the concentration of products to reactants when the acid dissociates in water. In this case, the weak acid HA dissociates into its conjugate base A- and a hydronium ion H3O+. The correct equilibrium constant should have the products (H3O+ and A-) in the numerator and the reactant (HA) in the denominator. Choice C is the only option that follows this format, making it the correct answer.

Find the Correct Equilibrium Constant That Shows the Ionization Constant [HA][H3O+][A−]\frac{[\mathrm{HA}]}{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{A}^{-}\right]}[H3​O+][A−][HA]​

Find the Correct Equilibrium Constant That Shows the Ionization Constant $\frac{[\mathrm{HA}]}{\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\left[\mathrm{A}^{-}\right]}$