Question

The concentration of a solution of sodium hydroxide, NaOH, was determined by using it to titrate a known volume of a 0.250 M sulfuric acid (H₂SO₄) in accordance with the following equation:

  H₂SO₄(aq) + 2 NaOH(aq) --> Na₂SO₄(aq) + 2 H₂O(l)

If it required 46.57 mL of the NaOH solution to neutralize 25.00 mL of a 0.250 M H₂SO₄ solution, complete the following:

The moles of H₂SO₄ consumed were 

The moles of NaOH reacted were 

The molarity of NaOH(aq) is 

Answer 1

Moles of H₂SO₄ =

$$(M×L) = (0.250×0.025)=6.25×10^{-3}Moles$$

Moles of NaOH = $6.25×10^{-3}× 2= 0.0125 Moles$

Molarity of NaOH =$\frac{0.0125}{0.04657}=0.2684 M$