Answer:
[tex]V_{base}=17.9mL[/tex]
Explanation:
Hello,
In this case, as the reaction between sodium hydroxide and sulfuric is:
[tex]2NaOH+H_2SO_4\rightarrow Na_2SO_4+2H_2O[/tex]
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:
[tex]n_{base}=2*n_{acid}[/tex]
Which in terms of concentrations and volumes is:
[tex]M_{base}V_{base}=2*M_{acid}V_{acid}[/tex]
In such a way, solving for the required volume of base we find:
[tex]V_{base}=\frac{2*M_{acid}V_{acid}}{M_{base}} \\\\V_{base}=\frac{2*0.820M*2.30mL}{0.211M}\\ \\V_{base}=17.9mL[/tex]
Best regards.
