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

Answer:

$V_{base}=17.9mL$

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:

$V_{base}=\frac{2*M_{acid}V_{acid}}{M_{base}} \\\\V_{base}=\frac{2*0.820M*2.30mL}{0.211M}\\ \\V_{base}=17.9mL$

Best regards.