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.
![**Buffer Solution Problem**
Consider a buffer made by adding 42.3 grams of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH. The base dissociation constant for (CH₃)₂NH is given as Kb = 5.4 x 10⁻⁴.
*Question:* What is the pH of this buffer?
**Explanation:**
To find the pH of this buffer, apply the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{Base}]}{[\text{Acid}]} \right) \]
1. **Calculate pKa:**
\[\text{pKa} = 14 - \text{pKb}\]
2. **Determine the concentrations of the base and the acid form (CH₃)₂NH₂⁺:**
- The concentration of (CH₃)₂NH can be found from the Molarity given.
- Convert grams of (CH₃)₂NH₂I to moles to find its concentration in the solution.
3. **Substitute the known values into the Henderson-Hasselbalch equation to calculate pH.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff235e0b8-8ad7-4b2b-97d3-ccce9d75e013%2F76fe0ca2-3827-4183-bdd1-f94d56b263ae%2F9mmpmwi_processed.png&w=3840&q=75)
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