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.
![### Understanding the \( K_a \) Reaction of HCN
**What is the \( K_a \) reaction of HCN?**
- **\( K_a \) Reaction:**
- [This section contains an empty box for input, indicating where the user is expected to provide the chemical equation or description of the acid dissociation reaction for HCN.]
**Calculating \( K_b \) for CN\(^-\) at 25 °C**
- The \( K_a \) of HCN is \( 6.2 \times 10^{-10} \). What is the \( K_b \) value for CN\(^-\) at 25 °C?
- **\( K_b = \)**
- [This section contains an empty box for input, suggesting where the user should calculate and enter the base dissociation constant for the cyanide ion (CN\(^-\)).]
### Explanation for Educational Context
This section is designed to guide students in understanding and calculating the chemical equilibrium constants related to the dissociation of hydrocyanic acid (HCN) and its conjugate base (CN\(^-\)). The \( K_a \) (acid dissociation constant) and \( K_b \) (base dissociation constant) are important in understanding the strength and behavior of acids and bases in solution.
Students need to:
1. Write the appropriate \( K_a \) reaction for HCN.
2. Use the provided \( K_a \) value to calculate the \( K_b \) for CN\(^-\) using the relationship: \( K_w = K_a \times K_b \), where \( K_w \) is the ion-product constant of water at 25 °C (\( 1.0 \times 10^{-14} \)).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0e989a36-a976-4f9a-8f93-2801096d9bdd%2F317eca9d-1473-43d1-ac49-73907c02dedd%2Fpca88xu_processed.png&w=3840&q=75)
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