4. Explain why each of the following would or would not be a good buffer system....

4. Explain why each of the following would or would not be a good buffer system.

a. HCl/NaCl

b. NH4Cl/NH3

c. HC2H3O2/NH3

e. HONH3Br/HONH2

Solutions

Expert Solution

A "buffer" is a mixture of two compounds that protects the pH of a solution from undergoing large changes when small amounts of acid (in the form of hydroxonium ion [H₃O⁺]) or base (in the form of hydroxide ion [OH^-]) are added. Buffers usually contain a weak acid and its conjugate base or a weak base and its conjugate acid. One of the two compounds in a buffering system acts as a proton donor, releasing H⁺ when pH rises, and the other as a proton acceptor, taking up H⁺ when pH drops.

(a)

Since HCl is a strong acid - it would not make a buffer solution.

(b) NH₄Cl/NH₃

NH₃ is a weak acid and NH₄Cl is its conugated acid. - Hence buffer system.

CH₃COOH is a weak acid and NH₃ is a base. Wouldn't be a good buffer

(e) HONH₃Br/NH₂OH

Hydroxylammonium bromide is an acid salt formed by hydroxylamine (HONH2) and hydrobromic acid (HBr).

In the solution first it dissociates;
HONH₃Br(aq) HONH₃⁺(aq) + Br^-(aq)

Then, HONH₃⁺ ions hydrolyze;
HONH₃⁺(aq) + H₂O HONH₂ + H₃O⁺(aq)

Dissocaiation of HONH₂;
HONH₂(aq) + H₂O(l) HONH₃⁺(aq) + OH^-(aq)

So a buffer system.

queen_honey_blossom answered 1 year ago

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