I need to know how to write an equation showing how a buffer containing ammonia and ammonium chloride neutralizes added acid of HNO3.

Question

I need to know how to write an equation showing how a buffer containing ammonia and ammonium chloride neutralizes added acid of HNO3.

Answer 1

To write an equation showing how a buffer containing ammonia (NH3) and ammonium chloride (NH4Cl) neutralizes added acid HNO3, follow these steps:

Step 1: Write the dissociation of ammonia (NH3) in water:
NH3 + H2O ⇌ NH4+ + OH-

Step 2: Write the dissociation of HNO3 in water:
HNO3 ⇌ H+ + NO3-

Step 3: Write the reaction between the ammonium ion (NH4+) and the acid (H+):
NH4+ + H+ ⇌ NH3 + H2O

Step 4: Combine the equations from steps 1, 2, and 3 to form the net ionic equation:
NH3 + HNO3 ⇌ NH4+ + NO3-

This net ionic equation illustrates how the ammonia and ammonium chloride buffer neutralizes the added acid HNO3, forming the ammonium ion (NH4+) and the nitrate ion (NO3-).

Answer 2

To write an equation showing how a buffer containing ammonia (NH3) and ammonium chloride (NH4Cl) neutralizes added acid HNO3 (nitric acid), you need to understand the concept of acid-base reactions and how buffers function.

A buffer is a solution that resists changes in pH when small amounts of acid or base are added. Buffers are commonly composed of a weak acid (HA) and its conjugate base (A-), or a weak base (B) and its conjugate acid (BH+). In the case of the ammonia-ammonium chloride buffer, ammonia (NH3) acts as a weak base, while ammonium chloride (NH4Cl) acts as a conjugate acid.

Here's how you can write the equation:

1. Start with the balanced equation for the reaction between ammonia (NH3) and water (H2O) to form ammonium hydroxide (NH4OH) and hydroxide ions (OH-):

NH3 + H2O ⇌ NH4+ + OH-

2. Next, consider the reaction of ammonium chloride (NH4Cl) with water (H2O) to produce ammonium hydroxide (NH4OH) and hydrogen ions (H+):

NH4Cl + H2O ⇌ NH4+ + OH- + H+

3. When an acid like HNO3 is added to the buffer solution, it reacts with the hydroxide ions (OH-) present in the buffer:

HNO3 + OH- → H2O + NO3-

4. The ammonia in the buffer acts as a base and reacts with the hydrogen ions (H+) from the acid to form ammonium ions (NH4+):

NH3 + H+ → NH4+

Overall, the reaction can be represented as:

HNO3 + NH3 ⇌ NH4+ + NO3- (buffer neutralization reaction)

Note: The reversible arrows indicate that the reaction can occur in both directions, depending on the relative concentrations of the reactants and products.

So, the equation above illustrates how the buffer containing ammonia and ammonium chloride neutralizes the added acid HNO3 by forming ammonium ions and nitrate ions, thereby helping to maintain a relatively constant pH.

Answer 3

NH3 + H^(from HNO3) ==> NH4^+

The equation you want is the above one.
How it works is below.

pH = pKa + log (NH4^+)/(NH3)
So when HNO3 is added to the solution, the NH3 reacts with it to form NH4^+, it increases NH4^+ and decreases NH3