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.
![**Problem Statement:**
For a solution of 2.5 M H₂CO₃ (Kₐ = 4.4 × 10⁻⁷), calculate:
(a) [H⁺]
___ M
(b) pH
___
(c) Percent ionization
___ %
**Instructions for Calculations:**
1. **[H⁺] Concentration:**
- Use the formula for the dissociation of a weak acid: H₂CO₃ ⇌ H⁺ + HCO₃⁻
- Apply the equilibrium expression: \( Kₐ = \frac{[H⁺][HCO₃⁻]}{[H₂CO₃]} \)
2. **pH Calculation:**
- Calculate pH using the formula: \( \text{pH} = -\log[H⁺] \)
3. **Percent Ionization:**
- Calculate percent ionization using:
\( \text{Percent Ionization} = \left( \frac{[H⁺] \text{ at equilibrium}}{\text{Initial } [H₂CO₃]} \right) \times 100\% \)
Fill in the calculations and solutions for each part as requested.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F738db1e2-4aa5-4874-9af6-830a7bc8f2f5%2F14d74790-b33f-4ce4-94f1-e63b98acb9f7%2Fazzbvd_processed.jpeg&w=3840&q=75)
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