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 pH of a Solution
In this exercise, we will determine the pH of a solution based on its hydrogen ion concentration \([H^+]\).
#### Question:
What is the pH of a solution with a hydrogen ion concentration \([H^+]\) = \(1 \times 10^{-6}\) M?
#### Solution:
To find the pH of a solution, we use the following formula:
\[ \text{pH} = -\log[H^+] \]
Given:
\[ [H^+] = 1 \times 10^{-6} \text{ M} \]
Now, calculate the pH:
\[ \text{pH} = -\log(1 \times 10^{-6}) \]
Using the properties of logarithms:
\[ \text{pH} = -\log(10^{-6}) \]
\[ \text{pH} = -(-6) \]
\[ \text{pH} = 6 \]
#### Answer:
The pH of the solution is 6.
This calculation follows the logarithmic relationship between the hydrogen ion concentration and pH, which is essential in determining the acidity or basicity of a solution. A pH of 6 indicates a slightly acidic solution, considering that the neutral pH is 7.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2d4c5a9e-ae57-4a9b-bcac-2cfb7874c09d%2F8245645c-d69e-4578-947e-86213625a913%2Fe6uxugr_processed.jpeg&w=3840&q=75)
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