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.
![**Calculating the pH of Milk**
To understand the acidity or alkalinity of a solution, we often use the pH scale. The concentration of hydrogen ions (H+) plays a crucial role in determining the pH value of a solution.
In this example, we are provided with the concentration of H+ ions in a glass of milk, which is approximately \(3.2 \times 10^{-7}\).
The pH of a solution is calculated using the formula:
\[ \text{pH} = -\log[H^+] \]
Given:
\[ [H^+] = 3.2 \times 10^{-7} \]
Substituting the given concentration into the pH formula:
\[ \text{pH} = -\log(3.2 \times 10^{-7}) \]
**Step-by-Step Calculation:**
1. Calculate the logarithm of the concentration:
\[ \log(3.2 \times 10^{-7}) = \log(3.2) + \log(10^{-7}) \]
2. Use the properties of logarithms:
\[ \log(3.2 \times 10^{-7}) = \log(3.2) + (-7) \]
3. Approximate the logarithm of 3.2 (usually, \(\log(3.2) \approx 0.51\)):
\[ \log(3.2 \times 10^{-7}) = 0.51 - 7 \]
4. Combine the results:
\[ 0.51 - 7 = -6.49 \]
5. The pH is the negative of this value:
\[ \text{pH} = -(-6.49) = 6.49 \]
Thus, the pH of the milk would be around **6.49** (rounded to the second decimal).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb6399c92-09b4-4305-953f-373fa98e5780%2Fcf0a8825-c06a-4a4e-a5e9-d940992401f7%2Fome66u_processed.jpeg&w=3840&q=75)
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