Question

Write the balanced NET IONIC equation for the reaction that occurs when perchloric acid and barium hypochlorite are combined. It is not necessary to include states such as (aq) or (s). + This reaction is classified as: The extent of this reaction is: When 35.0 mL of 0.300 M perchloric acid and 35.0 mL of 0.150 M barium hypochlorite are combined, the pH of the resulting solution will be seven

This reaction is classified as: Strong Acid + Strong Base, Weak Acid + Strong Base, Strong Acid + Weak Base, Weak Acid + Weak Base.

The extent of this reaction is: Below 50%, 50%, Above 50%, 100%

When 35.0 mL of 0.300 M perchloric acid and 35.0 mL of 0.150 M barium hypochlorite are combined, the pH of the resulting solution will be greater than, equal to, less than seven.

Answer 1

HClO_​​​4 + Ba(OCl)₂ ----------> Ba(ClO_{​​​​4} )₂ + 2 HOCl

This reaction occurs in 2 steps

Ba(OCl)₂ + H₂O -----------> Ba(OH)₂ + 2HOCl

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

Perchloric acid is a strong and HOCl is weak acid.

In the presence of strong acid, the dissociation of weak acid suppresses due to common ion effect.

Number of moles of HClO4 in 35 mL of 0.3M acid is 35*0.3/1000 = 0.105

Number of moles of Ba(OH)2 in 35 mL of 0.15 M is 0.105 moles

But barium Hydroxide is a weak base. Hence resultant solution is Acidic &has pH of <7

Extent of the reaction is 100%