Question

17.5ml sample of an acetic acid (CH3COOH)solution required 29.6ml of 0.250M NAOH for neutralization.What was the concerntration of acetic acid

Answer 1

To determine the concentration of acetic acid, we calculate the moles of NaOH used in the neutralization, apply the 1:1 stoichiometry of the reaction, and divide the moles of acetic acid by the volume of the acetic acid solution, which results in a concentration of 0.423 M for acetic acid.

Step-by-step explanation:

To calculate the concentration of acetic acid (CH3COOH), we need to use the stoichiometry of the neutralization reaction with sodium hydroxide (NaOH). According to the problem, 17.5 ml of acetic acid solution is neutralized by 29.6 ml of 0.250M NaOH. The reaction between acetic acid and sodium hydroxide is a 1:1 stoichiometry, meaning one mole of acetic acid reacts with one mole of sodium hydroxide.

Steps to Calculate Acetic Acid Concentration:

1. Calculate moles of NaOH used: moles NaOH = volume NaOH (L) × concentration NaOH (mol/L).
2. As the stoichiometry is 1:1, moles of acetic acid = moles of NaOH.
3. Calculate the concentration of acetic acid: concentration acetic acid (mol/L) = moles acetic acid/volume acetic acid solution (L).

Applying these steps:

• Moles NaOH = 0.0296 L × 0.250 mol/L = 0.0074 mol.
• Moles acetic acid = 0.0074 mol (from the stoichiometry).
• Concentration acetic acid = 0.0074 mol / 0.0175 L = 0.423 M (Molarity).

Therefore, the concentration of acetic acid in the solution is 0.423 M.