are this 2 equations the same NIE? and if not how come?

Write a net ionic equation for the reaction that occurs when aqueous solutions of ammonia and acetic acid are combined.

Write a net ionic equation for the reaction that occurs when aqueous solutions of acetic acid and ammonia are combined

Yes, they are the same.

well how do you work them out?

Please help me! i have no clue how to do this and its for my hw!

To determine if the two equations are the same net ionic equation (NIE), we need to understand the rules for writing net ionic equations and compare the two equations accordingly.

Net ionic equations represent only the species that participate in a chemical reaction in their ionic form. To write a net ionic equation, we follow these steps:

1. Write the balanced chemical equation for the reaction.
2. Break down all soluble ionic compounds into their respective ions.
3. Exclude spectator ions, which are ions that are present on both sides of the equation and do not participate actively in the reaction.
4. Write the net ionic equation by combining the remaining ions.

Now, let's examine the two given equations and determine if they are the same NIE. We will start by writing the balanced chemical equations for each reaction:

Equation 1:
NH₃(aq) + CH₃COOH(aq) → NH₄CH₃COO(aq)

Equation 2:
CH₃COOH(aq) + NH₃(aq) → NH₄CH₃COO(aq)

Both equations seem to represent the formation of the same product, NH₄CH₃COO, so they might appear to be the same. However, to confirm if they are the same NIE, we need to break down the compounds into their respective ions and identify any spectator ions.

In this case, both NH₃ and CH₃COOH are weak bases and weak acids, respectively. Hence, they do not completely dissociate into ions. So, we can write the equations as follows:

Equation 1 (broken into ions):
NH₄⁺(aq) + CH₃COO⁻(aq) → NH₄CH₃COO(aq)

Equation 2 (broken into ions):
CH₃COOH(aq) + NH₄⁺(aq) → NH₄CH₃COO(aq)

Upon comparing the broken-down equations, we can see that they are indeed the same net ionic equation. The spectator ions, NH₄⁺ and CH₃COO⁻, are common to both equations and do not participate in the overall reaction.

Therefore, the two equations represent the same net ionic equation, showing that the reaction between ammonia and acetic acid (or acetic acid and ammonia) results in the formation of NH₄CH₃COO.

1. Write and balance the molecular equation.

2. Separate the molecular equation into ions using the following rules:

a) gases are written as molecules.
b) insoluble materials are written as molecules.
c) weak electrolytes are written as molecules.
d) all others are written as ions.

From above:
Step 1. NH3 + CH3COOH ==> CH3COONH4
Step 2. NH3 + CH3COOH ==> CH3COO^- + NH4^+
Note: I like to see the phases included although the problem doesn't ask for that.
NH3(aq) + CH3COOH(aq) ==> CH3COO^-(aq) + NH4^+(aq)