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.
![**Question:** What is the \([OH^-]\) of a 3.40 M solution of pyridine (\(C_5H_5N\), \(K_b = 1.70 \times 10^{-9}\))?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0b602486-a9cf-4ba4-b784-d8c4c0a5fe75%2Fb9b84852-072d-40ad-a8a4-a62723f3ae84%2Fhpyknxq_processed.png&w=3840&q=75)
![**Problem Statement:**
An unknown weak base with a concentration of 0.170 M has a pH of 9.60. What is the \( K_b \) of this base?
**Solution Steps:**
1. **Determine the \( [OH^-] \) concentration:**
- Use the pH to find \( pOH \):
\[
pOH = 14 - pH = 14 - 9.60 = 4.40
\]
- Calculate \( [OH^-] \) using:
\[
[OH^-] = 10^{-pOH} = 10^{-4.40}
\]
2. **Set up the equilibrium expression:**
- The ionization of a weak base \( B \) can be represented as:
\[
B + H_2O \rightleftharpoons BH^+ + OH^-
\]
- Establish the equilibrium concentration:
\[
K_b = \frac{[BH^+][OH^-]}{[B]}
\]
3. **Calculate \( K_b \):**
- Assume \( [BH^+] \approx [OH^-] \) since it's a weak base and it dissociates minimally.
- Substitute the known values into the equilibrium expression to calculate the \( K_b \).
This comprehensive approach allows the calculation of the base dissociation constant for any weak base, using its concentration and solution pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0b602486-a9cf-4ba4-b784-d8c4c0a5fe75%2Fb9b84852-072d-40ad-a8a4-a62723f3ae84%2Ftv33k4h_processed.png&w=3840&q=75)
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