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 pH, [H⁺], and [OH⁻] from pOH
The problem asks you to determine the concentrations of hydrogen ions \([H^+]\), hydroxide ions \([OH^-]\), and the pH of a solution that has a pOH of 3.69 at 25 °C.
Given:
- pOH = 3.69
- Temperature = 25 °C
To solve this, use the following equations and relationships:
1. **Calculate [OH⁻]:**
\[
[OH^-] = 10^{-\text{pOH}}
\]
2. **Calculate pH:**
\[
\text{pH} = 14 - \text{pOH}
\]
3. **Calculate [H⁺]:**
\[
[H^+] = 10^{-\text{pH}}
\]
Fill in the boxes with the calculated values for \([H^+]\), \([OH^-]\), and pH.
**Note:** At 25 °C, the relationship \( \text{pH} + \text{pOH} = 14 \) holds true in water.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a46be85-81d4-49e6-8ea4-5055a0d2528a%2F717e6619-76e8-4fa0-ac48-5ad87cccadff%2Fs79uwei_processed.jpeg&w=3840&q=75)
![**Problem Statement:**
Determine the \([H^+]\), \([OH^-]\), and pOH of a solution with a pH of 6.54 at 25 °C.
**Solution Fields:**
\([H^+]\) = [Enter value here]
\([OH^-]\) = [Enter value here]
pOH = [Enter value here]
---
**Explanation for Educators:**
This question requires students to calculate the hydrogen ion concentration \([H^+]\), hydroxide ion concentration \([OH^-]\), and the pOH of a solution. Given the pH value, you can use the following formulas:
1. **Hydrogen Ion Concentration:**
\[
[H^+] = 10^{-\text{pH}}
\]
2. **pOH Calculation:**
\[
\text{pOH} = 14 - \text{pH}
\]
3. **Hydroxide Ion Concentration:**
\[
[OH^-] = 10^{-\text{pOH}}
\]
These calculations assume standard temperature conditions of 25°C, where the sum of pH and pOH is 14.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4a46be85-81d4-49e6-8ea4-5055a0d2528a%2F717e6619-76e8-4fa0-ac48-5ad87cccadff%2F95a4av_processed.jpeg&w=3840&q=75)
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