Final answer:
The molarity of the sulfuric acid solution is calculated by using the molarity and volume of the KOH solution to find the moles of the base, determining the moles of the acid from the balanced equation, and then dividing these moles by the volume of the acid solution. The molarity of the H₂SO₄ solution is found to be 0.2422 M.
Step-by-step explanation:
To determine the molarity of the sulfuric acid (H₂SO₄) solution, the concept of acid-base titration is used. Titrating a 25.0-mL sample of H₂SO₄ with 0.350 M KOH means we need to calculate how many moles of KOH reacts with the H₂SO₄ and then use this information to find the molarity of the acid.
The balanced chemical equation for the reaction between H₂SO₄ and KOH is:
H₂SO₄ (aq) + 2KOH(aq) → K₂SO₄ (aq) + 2H₂O (l)
Using the volumes and molarity of KOH, we can calculate the moles of KOH which have reacted:
Moles of KOH = Molarity of KOH × Volume of KOH in liters
Moles of KOH = 0.350 mol/L × 0.0346 L = 0.01211 mol
From the equation, we see that each mole of H₂SO₄ reacts with two moles of KOH. Therefore, the moles of H₂SO₄ will be half of the moles of KOH:
Moles of H₂SO₄ = Moles of KOH / 2
Moles of H₂SO₄ = 0.01211 mol / 2 = 0.006055 mol
We can calculate the molarity of the H₂SO₄ solution by dividing the moles of H₂SO₄ by the volume of the acid in liters:
Molarity of H₂SO₄ = Moles of H₂SO₄ / Volume of H₂SO₄ in liters
Molarity of H₂SO₄ = 0.006055 mol / 0.0250 L = 0.2422 M
Therefore, the molarity of the acid is 0.2422 M.