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.
![### Show What You Know: pH & pOH
**Question:**
What is the pH of a solution with \([OH^-] = 6.9 \times 10^{-2}\) M? Show your work.
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To solve this problem, you need to follow these steps:
1. Calculate the pOH of the solution using the formula:
\[ \text{pOH} = -\log[OH^-] \]
2. Use the relationship between pH and pOH:
\[ \text{pH} + \text{pOH} = 14 \]
3. Solve for the pH.
### Step-by-step Solution:
1. **Calculate the pOH:**
\[ \text{pOH} = -\log(6.9 \times 10^{-2}) \]
2. **Using a calculator:**
\[ \text{pOH} \approx 1.161 \]
3. **Find the pH:**
\[ \text{pH} + \text{pOH} = 14 \]
\[ \text{pH} = 14 - \text{pOH} \]
\[ \text{pH} = 14 - 1.161 \]
\[ \text{pH} \approx 12.839 \]
### Answer:
The pH of the solution is approximately 12.839.
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Make sure to understand the logarithmic calculations and the relationship between pH and pOH for solving similar problems.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F78b0d0bb-8fd7-4c3f-81b0-257e1cc18a72%2F86f1ffbb-824b-4f37-a168-e795a0b2ecae%2Ff7xmmmk_processed.jpeg&w=3840&q=75)
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