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.
![### Converting pOH to pH and Hydroxide Ion Concentration to pH
**1. Converting pOH to pH:**
\[ \text{pOH} = 9.45 \]
pH and pOH are related through the equation:
\[ \text{pH} + \text{pOH} = 14 \]
To find the pH:
\[ \text{pH} = 14 - \text{pOH} \]
\[ \text{pH} = 14 - 9.45 \]
\[ \text{pH} = 4.55 \]
So, the pH is 4.55 when the pOH is 9.45.
**2. Converting Hydroxide Ion Concentration \([OH^-]\) to pH:**
\[ [OH^-] = 5.76 \times 10^{-8} \]
First, we need to find the pOH using the relationship:
\[ \text{pOH} = -\log[OH^-] \]
Calculating the pOH:
\[ \text{pOH} = -\log(5.76 \times 10^{-8}) \]
Using a calculator:
\[ \text{pOH} \approx 7.24 \]
Now, use the relationship between pH and pOH to find the pH:
\[ \text{pH} = 14 - \text{pOH} \]
\[ \text{pH} = 14 - 7.24 \]
\[ \text{pH} = 6.76 \]
So, the pH is approximately 6.76 when the hydroxide ion concentration is \(5.76 \times 10^{-8}\) M.
This page explains the method to convert pOH to pH and hydroxide ion concentration to pH, showcasing the importance of understanding the logarithmic relationship in acid-base chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2f4e1179-0845-4cce-a522-94afec860b33%2F5a5bf246-83b2-4ac9-85e3-1300ea2001d2%2Fymmx44s_processed.jpeg&w=3840&q=75)
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