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.
![**Question:**
Which of the following can behave as Brønsted-Lowry acids in aqueous solution?
- [ ] HClO₄
- [ ] NH₄⁺
- [ ] H₃PO₄
- [ ] NO₂⁻
- [ ] None of the Above
**Explanation:**
In the context of Brønsted-Lowry theory, an acid is defined as a species that can donate a proton (H⁺). Consider each option:
- **HClO₄ (Perchloric acid):** A strong acid that dissociates completely in aqueous solution, donating a proton.
- **NH₄⁺ (Ammonium ion):** Can donate a proton to form NH₃ (ammonia).
- **H₃PO₄ (Phosphoric acid):** Weak acid with multiple acidic protons that can be donated in aqueous solution.
- **NO₂⁻ (Nitrite ion):** Typically acts as a base by accepting a proton rather than donating one.
- **None of the Above:** Incorrect as some of the given species are indeed Brønsted-Lowry acids.
Brønsted-Lowry acids in the given list are HClO₄, NH₄⁺, and H₃PO₄.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03ba95c9-584b-483d-8f8a-8f0f9c4c55b7%2F97f446d9-a76a-4e95-a220-3e030007d51f%2Fo1bk83t_processed.png&w=3840&q=75)
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