A strong acid or base is actually one that is

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A "strong" acid or base is actually one that is unstable and will readily dissociate when added to water. A "weak" acid or base is one that is stable, and does not dissociate in water. If an acid is to be "strong", it must readily dissociate to release hydrogen ions. However, the conjugate base that is formed must also be stable, so that is does not combine back with the released hydrogen ions, making it a weak base.
The Nature of Acids and Bases: Exploring the pH Scale EXPERIMENT 1: PREPARING A BUFFER Data Sheet Table 2: Sodium Acetate Data Sodium Acetate (g) Molarity of Sodium Acetate (M) 4 g 0.48 Mole Table 3: Buffer Solutions and pH Readings Buffer Volume of Acetic Acid (mL) Volume of Sodium Acetate (mL) pH A 5 5 4.1 B 5 1 17.2 C 10 1 2.9 D 1 10 4.7 E 1 5 18.1 Post-Lab Questions 1. Show your calculations for the molarity of sodium acetate (recorded in Table 2).
©eScience Labs, LLC 2015 2. Using the Henderson-Hasselbalch equation, calculate the predicted pH value for each buffer solution based on the volumes given in Table 3. The pKa of acetic acid is 4.75.

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