A 0.0015 M solution of a weak base has a pH of 9.84. Calculate Kb. Fill in reaction > Initial concentration Change in concentration Equilibrium concentration
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.
![**Week 9 - CHM 2046 Chapter 16 Quiz**
**Name:______________________________**
**Problem Statement:**
A 0.0015 M solution of a weak base has a pH of 9.84. Calculate \( K_b \).
**Table Details:**
The table below is designed to organize the solution data for further analysis:
| | |
|-------------------------------|-------------------------------|
| **Fill in reaction →** | |
| **Initial concentration** | |
| **Change in concentration** | |
| **Equilibrium concentration** | |
### Explanation:
- **Fill in reaction →**: This row is for detailing the chemical reaction of the weak base.
- **Initial concentration**: Here, you denote the starting concentration of the weak base before any dissociation.
- **Change in concentration**: This row captures the change in molarity as the reaction approaches equilibrium.
- **Equilibrium concentration**: In this row, you calculate and fill in the concentrations of reactants and products at equilibrium.
The task involves using the equilibrium expression for \( K_b \) calculation, likely employing the formula:
\[
K_b = \frac{[OH^-][BH^+]}{[B]}
\]
Utilizing the pH value provided to find the \( pOH \), and subsequently, the \( [OH^-] \) concentration for the computation of \( K_b \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03f6db9d-3538-45fb-b2ce-99c5cf80bdb2%2F907dd487-088f-42bf-b364-02fc1187d218%2Fj1w3xic_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 4 steps
