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
**What is the percent ionization of a 0.75 M solution of ammonia?**
**Given:**
\[ K_b(\text{NH}_3) = 1.8 \times 10^{-5} \]
### Solution Input
\[
\text{Percent Ionization} = \boxed{ \ ] \%
\]
### User Interaction
- **Input Box**: Below the problem statement, there is an input box labeled “% Ionization” where the user can enter their answer.
- **Submit Button**: There is an "Enter" button next to the input box to submit the answer for evaluation.
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This question involves calculating the percent ionization of ammonia in a solution.
Percent ionization is found using the formula:
\[ \text{Percent Ionization} = \left( \frac{[\text{OH}^-]_{\text{equilibrium}}}{[\text{NH}_3]_{\text{initial}}} \right) \times 100\]
Where:
- \([\text{OH}^-]_{\text{equilibrium}}\) is the concentration of hydroxide ions at equilibrium.
- \([\text{NH}_3]_{\text{initial}}\) is the initial concentration of ammonia.
This calculation typically involves setting up an ICE (Initial, Change, Equilibrium) table and using the base dissociation constant \(K_b\) to find the equilibrium concentration of ions in the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa4c65346-a6bd-47be-a891-a239e86f6fd1%2F3472e038-5c81-4461-b6f3-96bd854b9626%2Fdbhzdjh_processed.jpeg&w=3840&q=75)
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