What is the molarity of a NaOH solution, if 25.0 mL of this NaOH solution is required to neutralize 20.0 mL of 0.300 M H₂SO₄?
(Write a balanced reaction to ascertain the stoichiometry of this reaction.)

Question

Quizplus · Accepted Answer

The balanced reaction between NaOH and H₂SO₄ is: NaOH + HH₂SO₄ → NaH₂SO₄ + H2O From this reaction, we can see that 1 mole of NaOH reacts with 1 mole of H₂SO₄. To find the molarity of the NaOH solution, we need to use the formula: Molarity (M) = moles of solute / volume of solution (in liters) First, we need to calculate the number of moles of H₂SO₄: moles of H₂SO₄ = Molarity x volume (in liters) moles of H₂SO₄ = 0.300 M x 0.0200 L moles of H₂SO₄ = 0.0060 moles Since the reaction is 1:1, the number of moles of NaOH required to neutralize the H₂SO₄ is also 0.0060 moles. Now, we can use the formula to find the molarity of the NaOH solution: Molarity (M) = moles of NaOH / volume of NaOH solution (in liters) We know that 25.0 mL of the NaOH solution was required to neutralize the H₂SO₄. We need to convert this to liters: volume of NaOH solution = 25.0 mL = 0.0250 L Now we can plug in the values: Molarity (M) = 0.0060 moles / 0.0250 L Molarity (M) = 0.240 M Therefore, the molarity of the NaOH solution is 0.240 M, and the best choice is answer choice C.

What Is the Molarity of a NaOH Solution, If 25