Calculate the volume of 0.0500 M H2SO4 solution required to completely react with 20.0 mL of 1.00 x 10-3 M NaOH.

0.2 mL

Explanation:

When an acid and a base react, they converge in a neutralization reaction. So the formed products are water and a salt. The equation is:

H₂SO₄ (aq) + 2 NaOH (aq) → Na₂SO₄ (aq) + 2H₂O (l)

1 mol of sulfuric needs 2 moles of hydroxide to react.

Let's find out the moles of base:

Molarity = mol / volume (L) → molarity. volume (L) = moles

We make the conversion → 20 mL. 1L / 1000mL = 0.020L

0.001 M. 0.020L = 2*10⁻⁵ moles

So the rule of three is: 2 moles of base react with 1 mol of sulfuric

Therefore 2*10⁻⁵ moles of base will react with (2*10⁻⁵. 1) / 2 = 1*10⁻⁵ moles of acid. Let's find out the volume:

Molarity = mol / volume (L) → mol / Molarity = Volume (L)

1*10⁻⁵ mol / 0.05 M = 2*10⁻⁴ L.

If we want the value in mL, we make the conversion:

2*10⁻⁴ L. 1000 mL / 1L = 0.2 mL