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)

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

i would say b

explanation:

but i think i would need more information than that