Mixing Strong Acids with Strong Bases What is the pH of the solution that results from mixing 8.00 mL of 0.030 M perchloric acid with 28.00 mL of 0.050 M barium hydroxide? Check all of the following species that would be present in solution as a result of these two solutions being mixed. Ignore the traces of hydronium and hydroxide ions that would naturally be present from the autoionization of water. Ba2 + (aq) H2O (l) ClO3 - (aq) OH - (aq) ClO4 - (aq) H3O + (aq)

Answer: PH = 1.4

Explanation:

n (mole) = concentration (c) * volume (v)

n (HClO4) = 0.08 * 0.03

n (HClO4) = 0.0024 mole

n (Ba (OH) 2) = 0.28 * 0.05

n (Ba (OH) 2) = 0.014

2HClO4 + Ba (OH) 2 ... >Ba (ClO4) 2 + 2H2O.

Hence, the limiting reagent is perchloric acid. According to the reaction:

0.0024 HClO4 req 1/2 * 0.0024 of Ba (OH) 2.

n (Ba (OH) reacted = 0.0012

Excess n (Ba (OH) 2) = 0.014-0.0012

Excess n (Ba (OH) 2) = 0.0128

Conc (Ba (OH) 2) unreacted = 0.0128/.32 (vol. of mix is 32ml)

= 0.04M = [H+]

PH = - log[0.04] = 1.397

PH = 1.4