Question

An aqueous solution of barium hydroxide is standardized by titration with a 0.102 M solution of perchloric acid. If 10.3 mL of base are required to neutralize 24.0 mL of the acid, what is the molarity of the barium hydroxide solution?

Answer 1

Answer: The molarity of barium hydroxide solution is 0.118 M.

Step-by-step explanation:

To calculate the concentration of acid, we use the equation given by neutralization reaction:

`n_1M_1V_1=n_2M_2V_2`

where,

`n_1,M_1\text{ and }V_1` are the n-factor, molarity and volume of acid which is
`HClO_4`

`n_2,M_2\text{ and }V_2` are the n-factor, molarity and volume of base which is
`Ba(OH)_2`

We are given:

`n_1=1\\M_1=0.102M\\V_1=24.0mL\\n_2=2\\M_2=?M\\V_2=10.3mL`

Putting values in above equation, we get:

`1* 0.102* 24.0=2* M_2* 10.3\\\\M_2=0.118M`

Hence, the molarity of
`Ba(OH)_2` solution will be 0.118 M.