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Answer :
Final answer:
The concentration of the ASA solution is 0.5898 mol/L and the amount of ASA in the tablet is 2.656 grams. The pH at the equivalence point of the titration is above 7 due to the formation of the weakly basic conjugate base of ASA.
Explanation:
Acetylsalicylic acid (ASA), commonly known as aspirin, is a medication for treating pain, fever, and inflammation. In this scenario, we are determining the concentration of the ASA solution, the amount of ASA in an aspirin tablet, and the pH at the equivalence point of the titration.
(a) Determination of the concentration of the ASA solution
The moles of sodium hydroxide (NaOH) used in titration can be calculated using its concentration and volume. Moles of NaOH = 0.15 mol/L * 0.0983 L = 0.014745 moles. Since the reaction between ASA and NaOH is a 1:1 stoichiometry, this is also the moles of ASA. To find the concentration of ASA in the original solution, divide the moles of ASA by the volume of the solution in litres (0.025 L):
Concentration of ASA = 0.014745 moles / 0.025 L = 0.5898 mol/L.
(b) The amount of ASA in the tablet
To find the amount of ASA, we simply multiply the moles of ASA by its molar mass (180.16 g/mol).
Amount of ASA = 0.014745 moles * 180.16 g/mol = 2.656 g.
(c) The pH at the equivalence point
The pH at the equivalence point for the titration of a weak acid with a strong base is greater than 7 due to the production of the conjugate base of the weak acid, which undergoes hydrolysis in water to form OH- ions. To calculate the exact pH, one would need to know the concentration of acetate ions formed and use the hydrolysis and equilibrium equations accordingly.
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