Question

An aqueous solution of hydrochloric acid is standardized by titration with a 0.143 M solution of potassium hydroxide. If 20.5 mL of base are required to neutralize 27.6 mL of the acid, what is the molarity of the hydrochloric acid solution?

Answer 1

Answer: Molarity of the given hydrochloric acid solution is 0.106 M.

Step-by-step explanation:

Given:
`M_(1)` = 0.143 M,
`V_(1) = 20.5 mL`

`M_(2)` = ? ,
`V_(2) = 27.6mL`

Hence, molarity of the given hydrochloric acid solution is as follows.

`M_(1)V_(1) = M_(2)V_(2)`

`0.143 M * 20.5 mL = M_(2) * 27.6 mL`

`M_(2) = (0.143M * 20.5 mL)/(27.6 mL)`

= 0.106 M

Therefore, molarity of the given hydrochloric acid solution is 0.106 M.