Answer:
1.332 L
Explanation:
The reaction that takes place is:
- H₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O
First we calculate the number of NaOH moles, using the given volume and concentration:
- 350 mL * 3.33 M = 1165.5 mmol NaOH
Then we convert NaOH moles into H₂SO₄ moles, using the stoichiometric coefficients:
- 1165.5 mmol NaOH * [tex]\frac{2mmolH_2SO_4}{1mmolNaOH}[/tex] = 2331 mmol H₂SO₄
Finally we calculate the required volume of a 1.75 M solution of H₂SO₄, using the concentration and number of moles:
- 2331 mmol / 1.75 M = 1332 mL
We can convert mL into L:
