How many milliliters of 0.100 m naoh are required to neutralize the following solutions?

a.) 10.0 ml of 0.0500 m hcl
b.) 25.0 ml of 0.126 m hno3
c.) 50.0 ml of 0.215 m h2so4

Answers:

Explanation:

All the reactions are the neutralization of strong acids with the same strong base.

At the neutralization point you have:

And the number of equivalents (#EQ) may be calculated using the normality (N) concentration and the volume (V)

Then, at the neutralization point:

Also, you can use the formula that relates normality with molarity

a.) 10.0 mL of 0.0500 M HCl

         ⇒ V base = 10.0 ml ×0.0500 M / 0.100 M = 5.00 ml

b.) 25.0 mL of 0.126 M HNO₃

         ⇒ V base = 25.0 ml ×0.126 M / 0.100 M = 31.5 ml

c.) 50.0 mL of 0.215 M H₂SO4

         ⇒ V base = 50.0 ml ×0.215 M × 2 / 0.100 M = 215. ml

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since electrons are negative the answer is neagtaive