Response:
702 mL
To elaborate:
Given the following:
Mass of sodium hydroxide = 13.20 g
Molarity of H₂SO₄ = 0.235 M
We're tasked with finding the volume of acid necessary to neutralize the sodium hydroxide solution
Step 1: Write the balanced reaction equation
The reaction between H₂SO₄ and NaOH can be summarized as follows:
2NaOH(aq) + H₂SO₄(aq) → Na₂SO₄(aq) + 2H₂O(l)
Step 2: Calculate the moles of NaOH
Moles are calculated by dividing mass by molar mass
The molar mass of NaOH is 40.0 g/mol
Hence;
Number of moles of NaOH = 13.20 g ÷ 40 g/mol
= 0.33 moles of NaOH
Step 3: Determine moles of H₂SO₄ that react
According to the balanced equation, 2 moles of NaOH react with 1 mole of H₂SO₄
Therefore, the ratio giving moles of H₂SO₄ = Moles of NaOH ÷ 2
= 0.33 moles ÷ 2
= 0.165 moles
Step 4: Find the volume of H₂SO₄
Molarity indicates the concentration of the solution in moles per liter
Molarity = Moles ÷ Volume
By rearranging the formula, we find volume = Moles ÷ Molarity
= 0.165 moles ÷ 0.235 M
= 0.702 L
= 702 mL
Thus, the volume of the 0.235 M H₂SO₄ acid solution required equals
702 mL
