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 Concentration of Potassium Hydroxide for a Specific pH
To calculate the concentration of potassium hydroxide (KOH) needed to achieve an aqueous solution with a pH of 11.220, follow the steps below:
1. **Understanding pH**: The pH of a solution is a measure of its acidity or alkalinity. A pH of 7 is neutral, below 7 is acidic, and above 7 is basic (alkaline).
2. **Desired pH**: The target pH for this solution is 11.220.
3. **Relationship Between pH and pOH**:
- The sum of pH and pOH for any aqueous solution is always 14.
- Therefore, \( \text{pOH} = 14 - \text{pH} \).
- For a pH of 11.220, \( \text{pOH} = 14 - 11.220 = 2.780 \).
4. **Calculating Hydroxide Ion Concentration**:
- The pOH is related to the concentration of hydroxide ions (OH⁻) in the solution by the equation \( \text{pOH} = -\log[\text{OH}^-] \).
- Rearranging, we get \( [\text{OH}^-] = 10^{-\text{pOH}} \).
- Substituting the value of pOH, \( [\text{OH}^-] = 10^{-2.780} \).
5. **Molarity of Potassium Hydroxide**:
- Since KOH is a strong base and dissociates completely in water, the concentration of KOH is equal to the concentration of OH⁻ ions.
- Therefore, the molarity of potassium hydroxide \( [\text{KOH}] = 10^{-2.780} \) M.
This results in:
**Molarity of potassium hydroxide = (Blank to be filled) M**
Enter the calculated value in the provided blank space for Molarity.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad75d3c3-f925-415c-aa85-2c90219f0688%2F839bab9f-85eb-4d7f-9416-26653a41a8d6%2Fsbi2too_processed.png&w=3840&q=75)
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