Question

What volume of 0.6 m hcl is required to neutralize 100.0 ml of 0.5 m naoh?

Answer 1

Step-by-step explanation:

The given data is as follows.

`M_(1)` = 0.6 M,
`V_(1)` = ?

`M_(2)` = 0.5 M,
`V_(2)` = 100.0 ml

Therefore, we calculate the volume of NaOH as follows.

`(Molarity * Volume)_(HCl)` =
`(Molarity * Volume)_(NaOH)`

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

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

=
`(0.5 M * 100.0 ml)/(0.6 M)`

= 83.33 ml

Thus, we can conclude that volume of HCl is 83.33 ml.

Answer 2

In order to determine the amount needed, we have to know the chemical reaction that would happen between the substances. In this case the reaction would be:

NaOH + HCl = NaCl + H2O

We calculate as follows:

.1 L (0.5 mol NaOH / L ) ( 1 mol HCl / 1 mol NaOH) ( 1 L / 0.6 mol HCl ) = 0.08 L or 80 mL of 06 M HCl

Hope this answers the question. Have a nice day.