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.
![**Determining the Acid Ionization Constant (Ka) of a Weak Acid**
**Problem Statement:**
A 0.125 M weak acid (HA) solution has a pH of 2.25. Find the acid ionization constant, Ka.
**Solution:**
Given:
- Concentration of the weak acid ([HA]) = 0.125 M
- pH of the solution = 2.25
**Step 1: Determine the concentration of H⁺ ions.**
pH is defined as the negative logarithm of the hydrogen ion concentration, so we can express this as:
\[ \text{pH} = -\log [\text{H}^+] \]
Given the pH is 2.25, we can find the hydrogen ion concentration by reversing the formula:
\[ [\text{H}^+] = 10^{-\text{pH}} \]
\[ [\text{H}^+] = 10^{-2.25} \]
Using a calculator:
\[ [\text{H}^+] \approx 5.62 \times 10^{-3} \, \text{M} \]
**Step 2: Set up the expression for the ionization of the weak acid.**
The ionization of a weak acid HA in water can be represented as:
\[ \text{HA} \leftrightarrow \text{H}^+ + \text{A}^- \]
At equilibrium, let \( x \) be the concentration of \([ \text{H}^+ ]\) and \([ \text{A}^- ]\), and the concentration of \([ \text{HA} ]\) will reduce by \( x \).
So,
\[ [\text{H}^+] = x \approx 5.62 \times 10^{-3} \, \text{M} \]
\[ [\text{A}^-] = x \approx 5.62 \times 10^{-3} \, \text{M} \]
\[ [\text{HA}] = 0.125 - x \approx 0.125 - 5.62 \times 10^{-3} \approx 0.119 \, \text{M} \]
**Step 3: Write the expression for Ka and plug in the values.**
For a weak acid, the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdabc7e8b-d42d-4c7a-8b8c-eac102cb510a%2F761d406c-c4fa-4a41-bda6-08d39d6598c2%2Fb9wqf8_processed.jpeg&w=3840&q=75)
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