Question

What volume of 1.75 h2so4 would be needed to neutralize 350 ml of 3.33 m sodium hydroxide?​

Answer 1

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 * $\frac{2mmolH_2SO_4}{1mmolNaOH}$ = 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:

• 1332 mL / 1000 = 1.332 L