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.
![### Identifying Strong Acids
When studying acids and bases, specifically in chemistry, it is important to differentiate between strong and weak acids. The strength of an acid is determined by its ability to dissociate completely in water. A strong acid will fully dissociate, releasing all of its hydrogen ions (H⁺) into the solution. Weak acids only partially dissociate.
#### Question:
Which one of the following is a strong acid?
A) HNO₂
B) HF
C) HClO₄
D) HC₂H₃O₂
**Answer: C) HClO₄**
**Explanation:**
- **HNO₂ (Nitrous acid):** This is a weak acid, meaning it does not completely ionize in water.
- **HF (Hydrofluoric acid):** Despite being highly reactive and dangerous, HF is also considered a weak acid because it does not fully ionize in aqueous solutions.
- **HClO₄ (Perchloric acid):** This is a strong acid. Perchloric acid is known for its complete dissociation in water, making it one of the strongest acids.
- **HC₂H₃O₂ (Acetic acid):** This is also a weak acid and is the main component of vinegar.
Understanding the distinction between strong and weak acids is fundamental in chemistry, particularly when dealing with pH calculations, reaction mechanisms, and titrations.
Remember, strong acids completely dissociate in water:
\[ HClO₄ (aq) \rightarrow H^+ (aq) + ClO₄^- (aq) \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9b712500-b2ac-4dfb-be2f-1c8b439ce3a4%2F283626d7-422a-42f8-adef-a3502bc369d0%2F22vqh8f_processed.jpeg&w=3840&q=75)
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