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Acetylsalicylic acid (ASA) is the pain reliever in Aspirin. ASA is a weak acid with [tex]K_a = 3.2 \times 10^{-4}[/tex]. One Aspirin tablet was ground up and dissolved in 25.0 mL of water. It was titrated using 0.15 mol/L sodium hydroxide. To reach the endpoint, 98.3 mL of base was required.

Determine the concentration of the ASA solution.

Answer :

Final answer:

The concentration was found by dividing the moles of ASA by the volume of the solution, resulting in a concentration of 0.5898 M.

Explanation:

To determine the concentration of the acetylsalicylic acid (ASA) solution, we first recognize that the titration involves a neutralization reaction between ASA, a weak acid, and sodium hydroxide (NaOH), a strong base. Given that the endpoint was reached with 98.3 mL of 0.15 mol/L NaOH, we can calculate the moles of NaOH used in the titration.

Step 1: Calculate the moles of NaOH used.

Moles of NaOH = Volume (L) × Concentration (mol/L)Step 2: Determine the moles of ASA.

Since NaOH and ASA react in a 1:1 molar ratio (as implied by the neutralization reaction), the moles of ASA at the endpoint will equal the moles of NaOH used.

Moles of ASA = 0.014745 mol

Step 3: Calculate the concentration of the ASA solution.

Concentration (mol/L) = Moles of solute / Volume of solution (L)

The original volume of the ASA solution was 25.0 mL (or 0.025 L). Therefore, the concentration of ASA in the solution is:

Concentration of ASA = 0.014745 mol / 0.025 L = 0.5898 mol/L

This calculation reveals that the concentration of the ASA solution was 0.5898 M.

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