Question

How many milliliters of 1.0M NaOH solution are needed to neutralize 10.0mL of 2.5M CH3COOH solution?

Answer 1

To neutralize 10 mL of 2.5 M acetic acid, we first need to analyze the neutralization reaction:

CH₃COOH + NaOH -> H₂O + CH₃COONa

We then, turn the 10 mL of acetic acid to moles with the definition of molarity:

Molarity = Moles of Solute / Liters of Solution

2.5 M = Moles of Acetic Acid / 0.01 L

Moles of Acetic Acid = 0.025

Now, we need the equal amount of moles of sodium hydroxide to neutralize the acid, so we use again the definition of molarity to get our desired volume:

Molarity = moles of hydroxide / liters of solution

1 = 0.025 / L

Liters of Hydroxide solution = 0.025 L or 25 mL