Question

In: Chemistry

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.

(c) CH3COOH/NH3

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 2 years ago
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