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.
![**Transcription: Educational Website Content**
The value of \( K_a \) for acetylsalicylic acid (aspirin) is \( 3.00 \times 10^{-4} \).
What is the value of \( K_b \) for its conjugate base, \( \text{C}_9\text{H}_7\text{O}_4^- \)?
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**Explanation:**
This text addresses the relationship between the acid dissociation constant (\( K_a \)) of acetylsalicylic acid and the base dissociation constant (\( K_b \)) of its conjugate base. The relationship between \( K_a \) and \( K_b \) for a conjugate acid-base pair can be expressed through the ion product constant for water (\( K_w \)), which at 25°C is \( 1.00 \times 10^{-14} \). The equation is:
\[ K_a \times K_b = K_w \]
Given \( K_a \) of acetylsalicylic acid (\( \text{aspirin} \)) is \( 3.00 \times 10^{-4} \), the calculation for \( K_b \) would be required using the above relationship.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0e109430-7b34-4d38-8cab-38f4ccc5aed5%2F34fe11ac-a285-4354-9358-217b5c48078b%2Fubqhj8z_processed.jpeg&w=3840&q=75)
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