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11 August, 09:47

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?

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  1. 11 August, 11:20
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    (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).
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