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 pH of a 0.240 M solution of aniline (C₆H₅NH₂, Kb = 4.3 × 10⁻¹⁰)?
**Explanation:**
To find the pH of aniline, which is a weak base, you can use the formula for the base dissociation constant (Kb) to determine the concentration of hydroxide ions (OH⁻). Then, convert the OH⁻ concentration to pOH, and finally to pH.
1. **Calculate OH⁻ Concentration:**
For a weak base like aniline (C₆H₅NH₂), use the equation:
\[
Kb = \frac{[C₆H₅NH₃⁺][OH⁻]}{[C₆H₅NH₂]}
\]
Assume that the change in concentration \([OH⁻] = x\), then:
\[
Kb = \frac{x^2}{[0.240 - x]} \approx \frac{x^2}{0.240}
\]
Solve for \( x \) knowing \( Kb = 4.3 \times 10^{-10} \).
2. **Calculate pOH:**
\[
pOH = -\log[OH⁻]
\]
3. **Calculate pH:**
\[
pH = 14 - pOH
\]
Use these steps to find the pH of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F3523b6f7-3769-45b8-98d5-cc26f8ce7a3b%2F05067b64-354d-4ac0-8fbd-1f25643cf5e4%2Fwo3smgo_processed.jpeg&w=3840&q=75)
Step by step
Solved in 3 steps with 3 images
