Part A A buffer contains significant amounts of ammonia and ammonium chloride. W

Question

Part A A buffer contains significant amounts of ammonia and ammonium chloride. Write a net ionic equation showing how this buffer neutralizes added acid (HNO3) Express your answer as a chemical equation. Identify all of the phases in your answer. NH, (a)+HNO, (aq) NH NO, (aq) Submit My Answers Give Up Incorrect; Try Again; 4 attempts remaining Part B Write a net ionic equation showing how this buffer neutralizes added base (Ba(OH)2) Express your answer as a chemical equation. Identify all of the phases in your answer. 2NH (a)+Ba(OH) aq)2NH, (a) +2H2O)+ Ba (a Submit My Answers Give Up

Explanation / Answer

A buffer is any type of substance that will resist pH change when H+ or OH- is added.

This is typically achieved with equilibrium equations. Both type of buffer will resist both type of additions.

When a weak acid and its conjugate base are added, they will form a buffer

The equations:

The Weak acid equilibrium:

HA(aq) <-> H+(aq) + A-(aq)

Weak acid = HA(aq)

Conjugate base = A-(aq)

Neutralization of H+ ions:

A-(aq) + H+(aq) <-> HA(aq); in this case, HA is formed, H+ is neutralized as well as A-, the conjugate

Neutralization of OH- ions:

HA(aq) + OH-(aq) <-> H2O(l) + A-(aq) ; in this case; A- is formed, OH- is neutralized as well as HA.

Now,

For the weak base equilibrium:

B(aq) + H2O(l) <-> BH+(aq) + OH-(aq)

Weak base = B;

Conjugate acid = BH+

Neutralization of OH- ions:

BH+(aq) + OH-(aq) <-> B(aq) + H2O(l); in this case, OH- is neutralized by BH+, as well as B is created

Neutralization of H+ ions:

B(aq) + H+(aq) <-> BH+(aq)

for this specific case.

NH3(aq) + HNO3(aq) --> NH4+(aq) + NO3-(aq)

net ionic

NH3(aq) + H+(aq) --> NH4+(aq)

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