Question

(c) Write the balanced neutralization reaction and calculate the volume in mL of a 1.420 M NaOH solution required to titrate 25.00 mL of a 5.400 M H2SO4 solution

Answer 1

Answer:

2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

190.14 mL of the NaOH solution would be required.

Explanation:

The balanced reaction is:

• 2NaOH + H₂SO₄ → Na₂SO₄ + 2H₂O

Now we calculate how many H₂SO₄ moles are there in 25.00 mL of a 5.400 M solution, using the definition of molarity:

• Molarity = moles / liters

• Moles = Molarity * liters

• 25.00 mL * 5.400 M = 135 mmol H₂SO₄

Now we convert H₂SO₄ moles into NaOH moles, using the stoichiometric coefficients of the balanced reaction:

• 135 mmol H₂SO₄ * $\frac{2mmolNaOH}{1mmolH_2SO_4}$ = 270 mmol NaOH

Finally we calculate the volume of a 1.420 M solution that would contain 270 mmoles:

• Molarity = moles / liters

• liters = moles / molarity

• 270 mmol / 1.420 M = 190.14 mL