Question

. a 25.00 ml sample of a sulfuric acid solution (h2so4) is titrated with sodium hydroxide (naoh). if it requires 35.88 ml of 0.1127 m naoh to reach the endpoint, what is the molarity of the sulfuric acid solution? (all of the hydrogens of the sulfuric acid react with the sodium hydroxide.) hint: write a balanced chemical equation of this reaction first

Answer 1

To calculate the molarity of the sulfuric acid solution, use the balanced chemical equation for the reaction between sulfuric acid and sodium hydroxide.

Calculate the number of moles of sodium hydroxide used and then calculate the number of moles of sulfuric acid used. Finally, use the volume of sulfuric acid used to calculate the molarity.

Step-by-step explanation:

To calculate the molarity of the sulfuric acid solution, we need to use the balanced chemical equation for the reaction between sulfuric acid (H₂SO₄) and sodium hydroxide (NaOH):

H₂SO₄ (aq) + 2NaOH(aq) → Na₂SO₄ (aq) + 2H₂O (l)

From the equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydroxide. We can use this information to calculate the number of moles of sulfuric acid:

1. Calculate the number of moles of sodium hydroxide used: Moles of NaOH = Molarity of NaOH × Volume of NaOH used (in liters)
2. Since the reaction is 1:2, the moles of sulfuric acid used will be half of the moles of sodium hydroxide used.
3. Finally, calculate the molarity of the sulfuric acid solution by dividing the moles of sulfuric acid by the volume of sulfuric acid used (in liters).

Using the given data:

1. Moles of NaOH = (0.1127 M) × (0.03588 L) = 0.004044 mol NaOH
2. Moles of H₂SO₄ = 0.004044 mol NaOH ÷ 2 = 0.002022 mol H₂SO₄
3. Molarity of H₂SO₄ = 0.002022 mol H₂SO₄ ÷ (0.02500 L/1000) = 0.08088 M