Question

Calculate the volume, in milliliters, of a 0.211 M solution of NaOH that will completely neutralize each of the following. 2.30 mL of a 0.820 M solution of H2SO4. Express the volume in milliliters to three significant figures.

Answer 1

`V_(base)=17.9mL`

Step-by-step explanation:

Hello,

In this case, as the reaction between sodium hydroxide and sulfuric is:

`2NaOH+H_2SO_4\rightarrow Na_2SO_4+2H_2O`

We can notice a 2:1 molar ratio between the base and the acid, for that reason for the titration at the equivalence point we find:

`n_(base)=2*n_(acid)`

Which in terms of concentrations and volumes is:

`M_(base)V_(base)=2*M_(acid)V_(acid)`

In such a way, solving for the required volume of base we find:

`V_(base)=(2*M_(acid)V_(acid))/(M_(base)) \\\\V_(base)=(2*0.820M*2.30mL)/(0.211M)\\ \\V_(base)=17.9mL`

Best regards.