Which statement explains why 10.0 mL of a 0.50 M H2SO4(aq) solution exactly neutralizes 5.0 mL of a 2.0 M NaOH(aq) solution?

(1) The moles of H+(aq) equal the moles of OH-(aq).

Explanation:

Statements are:

(1) The moles of H+(aq) equal the moles of OH-(aq).

(2) The moles of H2SO4(aq) equal the moles of NaOH(aq).

(3) The moles of H2SO(aq) are greater than the moles of NaOH(aq).

(4) The moles of H+(aq) are greater than the moles of OH-(aq).

Neutralization reaction of H₂SO₄ with NaOH is:

H₂SO₄ + 2 NaOH → 2H₂O + Na₂SO₄

Where 1 mole of sulfuric acid (2 moles H⁺), reacts with 2 moles of NaOH (2moles of OH⁻)

As you cans see, the reaction occurs when moles of H⁺ are equal to moles of OH⁻

In the problem, moles of H⁺ are:

0.010L ₓ (0.50moles H₂SO₄ / 1L) ₓ (2moles H⁺ / mole H₂SO₄) =

0.01 moles of H⁺

Moles of OH⁻ are:

0.005L ₓ (2.0moles NaOH / 1L) ₓ (1mole OH⁻ / mole NaOH) =

0.01 moles of OH⁻

Thus, right statement is:

(1) The moles of H⁺(aq) equal the moles of OH⁻(aq).

i just calculated it all out, and not including weekends, and all the different days off. as of this school year (2018-2019) students are spending 2198 hours in school this year