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:**
If 25.0 mL of 0.10 M NH₃ (K_b = 1.8 x 10⁻⁵) is used to titrate 0.038 L of 0.30 M HCl, calculate the pH.
**Your Answer:**
[Input Box]
**Answer Button**
**Explanation:**
In this problem, we are asked to find the pH after a titration has been performed. The substances involved are NH₃ (ammonia) with a given base dissociation constant (K_b) and HCl (hydrochloric acid).
- **Volume and concentration of NH₃:** 25.0 mL (0.025 L) of 0.10 M
- **Volume and concentration of HCl:** 0.038 L of 0.30 M
- **K_b for NH₃:** \(1.8 \times 10^{-5}\)
The task involves calculating the pH after the titration is complete. This involves stoichiometric calculations and potentially using the Henderson-Hasselbalch equation.
Students should input their calculated pH value in the input box provided and press the answer button to check their work.
The prompt allows for a hands-on learning approach for calculating the pH during a titration process.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcd4de582-ae97-44e6-a760-e2e9372177a4%2F5923634b-c646-45ad-ad8c-9ee55fb7d4b8%2Foymx97j_processed.jpeg&w=3840&q=75)
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