Calculate the pH of 2.0 ×10^-4 M H3X solution assuming the first dissociation to be 100% second to be 50% and third to be negligible

Calculate the pH of 2.0 ×10^-4 M H3X solution assuming the first diss

1.	Calculate the pH of 2.0 ×10^-4 M H3X solution assuming the first dissociation to be 100% second to be 50% and third to be negligible
Answer» EXPLANATION:[OH-] = 8 x 10^-3In equilibrium concentration is C∝ where ∝ is the DEGREE of dissociationOH-] = (8x 10^-3) x 0.5 = 4 x 10^-3 MOLES pOH = -LOG 4 x 10^-3 = 2.4 pH = 14 - 2.4 pH= 11.6