33. Write a chemical equation using Lewis structures for the reaction of water with ammonia. Identify the Brønsted-Lowry acid and base in the reaction.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
I need help on my homework with number 33. See attached:
![**Reactivity of Water with Ammonia:**
**Objective:** Illustrate the chemical reaction of water (\(H_2O\)) with ammonia (\(NH_3\)) using Lewis structures. Further, identify the Brønsted-Lowry acid and base in the reaction.
**Instructions:**
1. **Lewis Structures:**
- **Water (H₂O):**
- Consists of an oxygen atom bonded to two hydrogen atoms.
- Oxygen has two lone pairs of electrons.
- **Ammonia (NH₃):**
- Consists of a nitrogen atom bonded to three hydrogen atoms.
- Nitrogen has one lone pair of electrons.
2. **Chemical Equation:**
- The reaction can be shown as:
\[
\text{H}_2\text{O} + \text{NH}_3 \rightarrow \text{OH}^- + \text{NH}_4^+
\]
3. **Brønsted-Lowry Acid and Base:**
- **Acid:** Water (\(H_2O\)) acts as the Brønsted-Lowry acid, donating a proton (\(H^+\)) to ammonia.
- **Base:** Ammonia (\(NH_3\)) acts as the Brønsted-Lowry base, accepting a proton from water.
**Concept Review:**
- In the Brønsted-Lowry theory, acids are proton donors and bases are proton acceptors.
Understanding this reaction is fundamental in exploring acid-base chemistry and interaction of basic solutions in various chemical applications.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F80366bbd-a758-40e7-b9ec-8d2e3445db54%2Fb3457c66-dcbd-4d99-930a-b142692bd230%2Fy1h4in_processed.png&w=3840&q=75)
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