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.
![### Calculating the Acid Dissociation Constant (Ka) of Chlorous Acid
**Problem Statement:**
The pH of a 0.209 M aqueous solution of chlorous acid is found to be 4.101. Calculate \( K_a \) for chlorous acid using this information.
**Detailed Explanation:**
To determine the acid dissociation constant (\( K_a \)) for chlorous acid, follow these steps:
1. **Understand the pH and Concentration Relationship:**
- The pH of a solution is a measure of its hydrogen ion concentration \([H^+]\).
- The equation relating pH to hydrogen ion concentration is:
\[ \text{pH} = -\log[H^+] \]
2. **Calculate \([H^+]\) from pH:**
- Given: \( \text{pH} = 4.101 \)
- Using the pH formula, solve for \([H^+]\):
\[ [H^+] = 10^{-\text{pH}} = 10^{-4.101} \approx 7.94 \times 10^{-5} \text{ M} \]
3. **Set Up the Equilibrium Expression:**
- Chlorous acid (\( \text{HClO}_2 \)) dissociates in water as follows:
\[ \text{HClO}_2 \leftrightarrow \text{H}^+ + \text{ClO}_2^- \]
- Let the initial concentration of \(\text{HClO}_2\) be \( 0.209 \text{ M} \) and the change in concentration of \([H^+]\) and \([\text{ClO}_2^-]\) be \( x \).
4. **Determine the Equilibrium Concentrations:**
- At equilibrium:
\[ [\text{H}^+] = x = 7.94 \times 10^{-5} \text{ M} \]
\[ [\text{ClO}_2^-] = x = 7.94 \times 10^{-5} \text{ M} \]
\[ [\text{HClO}_2] = 0.209 - x \approx 0.209 \text{ M} \] (since](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F36e576be-50e4-40e4-8c7b-fee84775ba0f%2Fd6fb826e-0de7-4a8f-beec-f8ea0c4c8258%2Fibxt53j_processed.jpeg&w=3840&q=75)
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