16.7
حسابات المعايرة: حمض ضعيف-قاعدة ضعيفة
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Q1: How do you calculate the initial pH of a weak acid before titration begins?
The initial pH is calculated using the Ka (acid dissociation constant) and an ICE table, since the weak acid is the main pH contributor. For example, a 0.10 M acetic acid solution has an initial pH of 2.87. This method applies whenever a weak acid or base dominates the pH before any titrant is added.
Q2: What happens to the pH when you add sodium hydroxide to a weak acid solution?
When sodium hydroxide is added to a weak acid, hydroxide ions react with the acid to form its conjugate base, creating a buffer solution. The pH can be calculated using the henderson hasselbalch equation calculating buffers. As more base is added, the buffer resists pH change until the equivalence point is reached.
Q3: Why does the pH equal the pKa at the half-equivalence point?
At the half-equivalence point, exactly half of the weak acid has been neutralized to form its conjugate base. Since the concentrations of weak acid and conjugate base are equal, the Henderson-Hasselbalch equation simplifies to pH = pKa. For acetic acid titration, this occurs at 12.50 mL of added sodium hydroxide.
Q4: What is the pH at the equivalence point for a weak acid-strong base titration?
At the equivalence point, all weak acid has been converted to its conjugate base, which is basic. The pH is calculated using the Kb of the conjugate base and an ICE table. For acetic acid titrated with sodium hydroxide, the equivalence point pH is 8.72, significantly higher than 7 due to the basic nature of acetate ions.
Q5: How do you find the Kb of a conjugate base from the Ka of the weak acid?
The relationship between Ka and Kb is given by Kw = Ka × Kb, where Kw is the water ionization constant (1.0 × 10⁻¹⁴). Rearranging gives Kb = Kw / Ka. For acetate ion, Kb = 1.0 × 10⁻¹⁴ / 1.8 × 10⁻⁵ = 5.6 × 10⁻¹⁰.
Q6: What determines the pH after the equivalence point in a weak acid-strong base titration?
After the equivalence point, excess strong base (sodium hydroxide) is present in solution. The strong base is a much stronger contributor to pH than the conjugate base, so the final pH is determined by the concentration of excess hydroxide ions. For example, adding 70 mL of 0.10 M NaOH results in a pH of 12.22.
Q7: How does the titration curve for a weak acid-strong base differ from a strong acid-strong base titration?
In weak acid-strong base titrations, the equivalence point occurs in the basic region (pH > 7) because the conjugate base is basic. The initial pH is higher, and a buffer region exists before the equivalence point. This contrasts with titration calculations strong acid strong base, where the equivalence point is at pH 7.