What mass of NaOH is required to react exactly with 25.0 mL of 2.7 M H₂SO₄? A)2.7 g B)0.7 g C)5.4 g D)135 g E)none of these

Question

Quizplus · Accepted Answer

First, we need to write out the balanced equation between NaOH and H₂SO₄: NaOH + H₂SO₄ -> Na₂SO₄ + H2O Based on this equation, we can see that 1 mole of NaOH will react with 1 mole of H₂SO₄. To find the number of moles of H₂SO₄ that we have in 25.0 mL of 2.7 M solution, we can use the equation: moles H₂SO₄ = Molarity x Volume (in liters) moles H₂SO₄ = 2.7 mol/L x 0.0250 L = 0.0675 mol Therefore, we need an equal number of moles of NaOH to react with all of the H₂SO₄. That means we need: moles NaOH = 0.0675 mol To find the mass of NaOH needed, we can use its molar mass: mass NaOH = moles NaOH x molar mass NaOH mass NaOH = 0.0675 mol x 40.00 g/mol = 2.70 g Therefore, the answer is choice C, 5.4 g.

What Mass of NaOH Is Required to React Exactly with 25.0