In a 0.3000M solution of a monoprotic weak acid (HA), [H

Last updated: 7/30/2022

In a 0.3000M solution of a monoprotic weak acid (HA), [H] = 2.35 X 10-4 M. What is the dissociation constant (K₂) of this acid? The equilibrium constant of [H*] and of the corresponding anion are both equal to 2.35 X 10-4 M What is the equilibrium concentration of the acid [HA] to four significant figures? ___M (The equilibrium value of [HA] is the initial value minus the equilibrium value of [H*].) The formula for the dissociation constant is K₂=([H]X [A]) + [HA] Substitute the known values and calculate. Give your answer in scientific notation and to three significant digits. K₂= Type your answer here. X 10-7