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plumhare986Lv1

6 Oct 2020

Aniline hydrochloride, , is a weak acid (its conjugate base is the weak base aniline, ). The acid can be titrated with a strong base such as .

Assume 50.0 mL of 0.100 M aniline hydrochloride is titrated with 0.185 M . (K_a for aniline hydrochloride is 2.4 x 10^-5).

(a) What is the pH of the solution before the titration begins?

(b) What is the pH at the equivalence point?

(c) What is the pH at the halfway point of the titration?

(d) What indicator may be used to detect the equivalence point?

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Brian HingpitLv10

14 Dec 2020

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A titration of 25.00 mL of a solution of the weak base aniline, C₆H₅NH₂ requires 25.67 mL of 0.1750 M HCl to reach the equivalence point.

C₆H₅NH₂ (aq) + H₃O⁺ (aq) C₆H₅NH₃⁺ (aq)+ H₂O (l)

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Sketch the titration curve for a weak base titrated by a strong acid. Weak base–strong acid titration problems also follow a two-step procedure.

What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong acid (HNO₃, for example) reacts to completion with the weak base, B. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH?

Why is pH < 7.0 at the equivalence point of a weak base–strong acid titration? If pH=6.0 at the halfway point to equivalence, what is the K_b value for the weak base titrated? Compare and contrast the titration curves for a strong base–strong acid titration and a weak base–strong acid titration.