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.
![### Determining the Ka of a Weak Acid
#### Problem Statement
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid.
#### Instruction
Based on the given values, fill in the ICE (Initial, Change, Equilibrium) table to determine concentrations of all reactants and products.
#### Reaction
HA(aq) + H2O(l) ⇌ H3O+(aq) + A−(aq)
#### ICE Table Framework
| | HA(aq) | H2O(l) | H3O+(aq) | A−(aq) |
|-----------------------|-------------------|----------------|----------------|----------------|
| **Initial (M)** | | | | |
| **Change (M)** | | | | |
| **Equilibrium (M)** | | | | |
#### Explanation
- **Initial Concentration (M):** This is the initial molarity of each species before the reaction begins. Initially, [HA] is 0.1000 M, while [H3O+] and [A−] are 0 M as the reaction has not proceeded yet.
- **Change in Concentration (M):** Indicates the change in concentration as the reaction reaches equilibrium. Since HA is 3.0% dissociated, the change is 3% of 0.1000 M for HA, and the same amount will appear as products H3O+ and A−.
- **Equilibrium Concentration (M):** The remaining concentration of each species at equilibrium. This is calculated based on the changes from the initial concentrations.
Fill in this table using these details to find the equilibrium concentrations and then calculate the acid dissociation constant, Ka, using the formula:
\[ \text{Ka} = \frac{[\text{H}_3\text{O}^+][\text{A}^-]}{[\text{HA}]} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc276033a-7e95-4c42-bb2e-bc19111e69ab%2Fe9057eb3-1d67-425e-8af3-271f5c1be4f9%2Fazlanyd_processed.png&w=3840&q=75)
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