Question

Find the volume of 0.130M sulfuric acid necessary to react completely with 65.9g sodium hydroxide

Answer 1

The volume of the 0.130 M sulfuric acid, H₂SO₄ required to react completely with 65.9 g sodium hydroxide, NaOH is 6.34 L

• We'll begin by calculating the number of mole of in 65.9 g sodium hydroxide, NaOH. This can be obtained as follow:

Mass of NaOH = 65.9 g

Molar mass of NaOH = 23 + 16 + 1 = 40 g/mol

Mole of NaOH =?

Mole = mass / molar mass

Mole of NaOH = 65.9 / 40

Mole of NaOH = 1.6475 mole

• Next, we shall determine the number of mole of H₂SO₄ needed to react with 1.6475 mole of NaOH. This can be obtained as follow:

2NaOH + H₂SO₄ —> Na₂SO₄ + 2H₂O

From the balanced equation above,

2 moles of NaOH reacted with 1 mole of H₂SO₄.

Therefore,

1.6475 mole of NaOH will react with = $\frac{1.6475}{2}$ = 0.82375 mole of H₂SO₄.

• Finally, we shall determine the volume of 0.130 M sulfuric acid, H₂SO₄ required for the reaction.

Molarity of H₂SO₄ = 0.130 M

Mole of H₂SO₄ = 0.82375 mole

Volume of H₂SO₄ =?

Volume = mole / Molarity

Volume of H₂SO₄ = 0.82375 / 0.130

Volume of H₂SO₄ = 6.34 L

Therefore, the volume of the 0.130 M sulfuric acid, H₂SO₄ required for the reaction is 6.34 L

Learn more: https://brainly.com/question/7882345