Calculate the hydroxide ion concentration of an aqueous solution of 0.505 M acetylsalicylic acid (aspirin). (Assume that Ka (HC9H7O4) = 3.0 × 10-4.) [OH-] = M
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.
![### Calculating Hydroxide Ion Concentration of Acetylsalicylic Acid Solution
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**Problem Statement:**
Calculate the hydroxide ion concentration (\([OH^-]\)) of an aqueous solution of 0.505 M acetylsalicylic acid (aspirin). Assume that the acid dissociation constant (\(K_a\)) for acetylsalicylic acid (\(\text{HC}_9\text{H}_7\text{O}_4\)) is \(3.0 \times 10^{-4}\).
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**Formula and Key Data:**
- **Acid Dissociation Constant (Ka):** \( K_a (\text{HC}_9\text{H}_7\text{O}_4) = 3.0 \times 10^{-4} \)
- **Concentration of acetylsalicylic acid solution:** 0.505 M
\[ [OH^-] = \_\_\_\_\_\_ \text{ M} \]
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**Steps to Follow:**
1. **Determine the \( [H^+] \) concentration:**
a. Use the formula of \( K_a \) and the concentration of the acid:
\[
K_a = \frac{[H^+][A^-]}{[HA]}
\]
Here, \( [HA] \) represents the initial concentration of acetylsalicylic acid, which is 0.505 M.
2. **Calculate the \( [OH^-] \):**
Knowing the relationship between \( [H^+] \) and \( [OH^-] \) in water:
\[
K_w = [H^+][OH^-] = 1.0 \times 10^{-14}
\]
Solve for \( [OH^-] \):
\[
[OH^-] = \frac{K_w}{[H^+]}
\]
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