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:**
Determine the pH of a solution that is 0.15 M CH₃COOH and 0.10 M CH₃COONa.
**Solution Explanation:**
This problem involves a buffer solution composed of acetic acid (CH₃COOH) and its salt, sodium acetate (CH₃COONa). To solve this, the Henderson-Hasselbalch equation can be utilized:
\[ \text{pH} = \text{pK}_a + \log \left(\frac{[\text{A}^-]}{[\text{HA}]}\right) \]
Where:
- \([\text{A}^-]\) is the concentration of the acetate ion (\(CH₃COO^-\)).
- \([\text{HA}]\) is the concentration of acetic acid (\(CH₃COOH\)).
- \(\text{pK}_a\) is the negative logarithm of the acid dissociation constant (\(K_a\)) of acetic acid.
The values required for this calculation (e.g., \(K_a\) for acetic acid) would need to be looked up in a reference source.
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Given that
Ka for CH3COOH = 1.8 × 10–5
Concentration of CH3COOH = 0.15 M
Concentration of CH3COO– = 0.10 M
The solution contains weak acid CH3COOH and its conjugate base CH3COO–.
So, this is a buffer solution.
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