The K₂ of a monoprotic weak acid is 0.00493. What is the percent ionization of a 0.103 M solution of this acid? 21.9 percent ionization: Incorrect %
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.
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![**Problem:** The \( K_a \) of a monoprotic weak acid is 0.00493. What is the percent ionization of a 0.103 M solution of this acid?
**Answer Box (Incorrect Submission):**
- **percent ionization:** 21.9 %
**Feedback:**
- **Status:** Incorrect
When working on this problem, use the percent ionization formula for weak acids, which is:
\[ \text{Percent Ionization} = \left( \frac{[\text{H}^+]}{[\text{HA}]} \right) \times 100\]
Where:
- \( [\text{H}^+] \) is the concentration of hydrogen ions after ionization.
- \( [\text{HA}] \) is the initial concentration of the weak acid solution.
Further steps typically involve setting up an equilibrium expression involving \( K_a \) and solving for the concentration of ionized acid.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3f33cc2f-0221-41a8-a3a2-cc96bc7960a2%2Fbef97222-3845-4aa6-8f2e-47e986c15ddf%2Fa5bbmoa_processed.png&w=3840&q=75)
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