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

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

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itemderby itemderby · Answer 2 · 2019-02-09T16:06:45+01:00

Explanation:

The given data is as follows.

[tex]M_{1}[/tex] = 0.6 M, [tex]V_{1}[/tex] = ?

[tex]M_{2}[/tex] = 0.5 M, [tex]V_{2}[/tex] = 100.0 ml

Therefore, we calculate the volume of NaOH as follows.

[tex](Molarity \times Volume)_{HCl}[/tex] = [tex](Molarity \times Volume)_{NaOH}[/tex]

[tex]M_{1} \times V_{1} = M_{2} \times V_{2}[/tex]

[tex]V_{1} = \frac{M_{2} \times V_{2}}{M_{1}}[/tex]

= [tex]\frac{0.5 M \times 100.0 ml}{0.6 M}[/tex]

= 83.33 ml

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