In an aqueous solution of a certain acid the acid is 0.083% dissociated and the pH is 4.20. Calculate the acid dissociation constant K, of the acid. Round your answer to 2 significant digits. K = 0 0 10
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:**
In an aqueous solution of a certain acid, the acid is 0.083% dissociated and the pH is 4.20. Calculate the acid dissociation constant \( K_a \) of the acid. Round your answer to 2 significant digits.
**Answer Box:**
\[ K_a = \quad \text{(textbox where the answer is to be entered)} \]
**Additional Tools:**
- Check box labeled with \( \times 10 \)
- Three option buttons labeled with an "X" (to cancel), a "↻" symbol (likely to reset), and a "?" (for help).
**Explanation:**
To solve this, use the following steps:
1. **Calculate the concentration of \( \text{H}^+ \) ions:**
\[
\text{pH} = -\log[\text{H}^+]
\]
Rearrange the equation to find \( [\text{H}^+] \):
\[
[\text{H}^+] = 10^{-\text{pH}} = 10^{-4.20}
\]
2. **Determine the degree of dissociation (\( \alpha \)):**
\[
\alpha = \frac{0.083}{100} = 0.00083
\]
3. **Relate the degree of dissociation to the initial concentration \( C_0 \):**
\[
[\text{H}^+] = \alpha \cdot C_0
\]
Thus, \( C_0 \):
\[
C_0 = \frac{[\text{H}^+]}{\alpha}
\]
4. **Substitute all known values:**
\[
K_a = \alpha \cdot C_0^2
\]
5. **Round the final answer to 2 significant digits.**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1c542873-90da-4d8f-af03-4e4a6198699f%2Fc6f8628f-1963-4d53-ac2e-b579180a4038%2Fewrupgn_processed.jpeg&w=3840&q=75)
Step by step
Solved in 2 steps with 1 images
