Chemistry, 24.01.2020 08:31 lw057080

How many ml of 0.100 m naoh is needed to titrate 20.0 ml of 0.100 m h2so4

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So the first thing we must do is write a balanced equation for the reaction and we know the equation is balnced when all the species on the RHS is equal to the species on the LHS
2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

So now it's time to identify what you know from the question (volume & conc. of H₂SO₄) and use that info to find the unknown (volume of NaOH)

If 1000 ml of H₂SO₄ contain 0.100 mol [0.100 M is the amount of moles in
1 L (1000 ml)]
then let 20 ml of H₂SO₄ contain x mol [20 ml is the amount of the acid that    took place in the reaction]

⇒ x = $\frac{20 ml * 0.1 mol}{1000 mol}$

= 0.002 mol

Mole ratio of NaOH to H₂SO₄ can be obtained from the balanced equation
2NaOH + 1H₂SO₄ → Na₂SO₄ + 2H₂O

thus mole ratio of   NaOH to H₂SO₄ is 2 : 1

∴ if mole of of H₂SO₄  = 0.002 mol
then moles of NaOH = (0.002 mol) × 2
= 0.004 mol

Now molarity = $\frac{MOLES}{MOLARITY}$
  ∴ by transposition

Volume = $\frac{moles}{molarity}$
= $\frac{0.004 mol}{0.1 mol/L}$
= 0.04 L
= 40 mL

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