Equilibrium Calculation for Chlorous Acid
What are the equilibrium concentrations for H3O+ and ClO2- in the dissociation of chlorous acid?
(a) Calculate the concentration of H3O+ at equilibrium if the initial concentration of HClO2 is 1.81×10^2 MM.
(b) Calculate the concentration of ClO2- at equilibrium if the initial concentration of HClO2 is 1.81×10^2 MM.
(c) Calculate the concentration of HClO2 at equilibrium if the initial concentration of HClO2 is 1.81×10^2 MM.
Equilibrium Concentrations of H3O+, ClO2-, and HClO2
(a) The concentration of H3O+ at equilibrium is 1.33×10^-3 M.
(b) The concentration of ClO2- at equilibrium is 0.149 M.
(c) The concentration of HClO2 at equilibrium is 0.018 M.
When calculating the equilibrium concentrations for the dissociation of chlorous acid (HClO2), we can use the acid dissociation constant, Ka. Given that the acid-dissociation constant for chlorous acid is 1.1×10^-2, we can determine the concentrations of H3O+, ClO2-, and HClO2 at equilibrium.
(a) To calculate the concentration of H3O+ at equilibrium, we use the equation Ka = [H3O+][ClO2-]/[HClO2]. By rearranging the equation, we find that the concentration of H3O+ at equilibrium is 1.33×10^-3 M.
(b) Next, to find the concentration of ClO2- at equilibrium, we again use the equation Ka = [H3O+][ClO2-]/[HClO2] and determine that the concentration of ClO2- at equilibrium is 0.149 M.
(c) Lastly, by utilizing the same equation with known concentrations of H3O+ and ClO2-, we calculate the concentration of HClO2 at equilibrium to be 0.018 M.
Understanding equilibrium concentrations in acid dissociation reactions is essential for chemical equilibrium calculations. By applying the principles of equilibrium, we can determine the concentrations of reactants and products at equilibrium, offering insights into the behavior of acids and their dissociation processes.