Acetic acid ionizes in water according to the following equation: CH3COOH = H^+ +CH4COO-
If the solution is .906 M acetic acid, what is the concentration of H+?
CH3COOH --> H^+ + CH3COO^-
Ka = (H^+)(CH3COO^-)/(CH3COOH)
Set up x = H^+, x = CH3COO^-, and CH3COOH = 0.906-x. Solve for x.
To calculate the concentration of H+ ions in the given acetic acid solution, we need to consider the ionization equation provided:
CH3COOH --> H+ + CH3COO-
The stoichiometric ratio for H+ ions to acetic acid is 1:1. This means that for every molecule of acetic acid that ionizes, one H+ ion is produced. Therefore, the concentration of H+ ions will be equal to the concentration of acetic acid.
Given that the concentration of acetic acid (CH3COOH) is 0.906 M, the concentration of H+ ions will also be 0.906 M.
So, the concentration of H+ ions in the solution is 0.906 M.