Question

An aqueous solution of perchloric acid is standardized by titration with a 0.191 M solution of barium hydroxide. If 13.8 mL of base are required to neutralize 17.0 mL of the acid, what is the molarity of the perchloric acid solution?

Answer 1

Molarity of
`HClO_(4)` solution is 0.311 M

Step-by-step explanation:

Neutralization reaction:
`2HClO_(4)+Ba(OH)_(2)\rightarrow Ba(ClO_(4))_(2)+2H_(2)O`

According to balanced reaction, 1 mol of
`Ba(OH)_(2)` neutralizes 2 moles of
`HClO_(4)`

Number of moles of
`Ba(OH)_(2)` in 13.8 mL of 0.191 M
`Ba(OH)_(2)` solution =
`(0.191)/(1000)* 13.8moles` =
`0.00264moles`

Let's assume molarity of
`HClO_(4)` solution is C (M) then-

Number of moles of
`HClO_(4)` in 17.0 mL of C (M)
`HClO_(4)` solution =
`(C)/(1000)* 17.0moles` =
`0.017Cmoles`

Hence,
`0.017C=(2* 0.00264)`

or,
`C=0.311`

So, molarity of
`HClO_(4)` solution is 0.311 M