How many milliliters of 0.755 M H₂SO₄ solution is needed to react with 55.0 mL of 2.50 M KOH solution?
Given: 2 KOH (aq) + H₂SO₄ (aq) → 2 H₂O (l) + K₂SO₄ (aq)

Question

Quizplus · Accepted Answer

To solve this problem, we need to use stoichiometry and the equation given to us. First, let's balance the equation: 2 KOH (aq) + H₂SO₄ (aq) → 2 H₂O (l) + K₂SO₄ (aq) We can see that the ratio of KOH and H₂SO₄ is 2:1, which means that for every 2 moles of KOH, we need 1 mole of H₂SO₄ to react. We can use the equation: moles = concentration (M) x volume (L) to find the number of moles of KOH we have: moles of KOH = concentration (2.50 M) x volume (55.0 mL / 1000 mL/L) = 0.1375 mol Since the ratio of KOH to H₂SO₄ is 2:1, we need half the number of moles of H₂SO₄: moles of H₂SO₄ = 0.1375 mol / 2 = 0.06875 mol Finally, we can use the equation: volume (L) = moles / concentration (M) to find the volume of 0.755 M H₂SO₄ we need: volume of H₂SO₄ = 0.06875 mol / 0.755 M = 0.0911 L = 91.1 mL Therefore, the best choice is C.

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