Question

A 25.00-mL sample of H2SO4(aq) requires 22.65 mL of the 0.5510 M NaOH for its titration. Assuming that sulfuric acid behaves as a strong acid with respect to both ionizable hydrogen atoms, what was the concentration of the sulfuric acid (H2SO4)?

Answer 1

A 25.00-mL sample of H2SO4(aq) requires 22.65 mL of the 0.5510 M NaOH for its titration. Assuming that sulfuric acid behaves as a strong acid with respect to both ionizable hydrogen atoms, what was the concentration of the sulfuric acid (H2SO4)?

Solution:

$$H _ {2} S O _ {4} + 2 N a O H = N a _ {2} S O _ {4} + 2 H _ {2} O$$

n (H₂SO₄) = ½n (NaOH)

n (NaOH) = 0.5510*0.02265 = 0,01248015 (mole)

n (H₂SO₄) = 0,01248015/2 = 0,006240075 (mole)

Cₘ (H₂SO₄) = 0,006240075/0.025 = 0,2496 M

Answer: 0.2496 M