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.
![**Problem 3: Calculating pH of a Buffered Solution**
What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? Given that the \( K_a \) for acetic acid is \( 1.8 \times 10^{-5} \).
**Explanation:**
This problem involves calculating the pH of a buffer solution using the Henderson-Hasselbalch equation, which is suitable for solutions comprising a weak acid and its conjugate base. The equation is given by:
\[
\text{pH} = \text{pK}_a + \log \left(\frac{[\text{A}^-]}{[\text{HA}]}\right)
\]
Where:
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate),
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid),
- \(\text{pK}_a = -\log(K_a)\).
**Calculation Steps:**
1. Calculate \(\text{pK}_a\):
\[
\text{pK}_a = -\log(1.8 \times 10^{-5})
\]
2. Apply concentrations to the Henderson-Hasselbalch equation:
\[
\text{pH} = \text{pK}_a + \log \left(\frac{0.75}{0.50}\right)
\]
This method effectively calculates the pH of buffer solutions in which both the acid and base components are present in significant amounts.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd86e2176-2b92-4a94-a128-f6a0aba0ae4d%2Fc6695d75-aba2-469d-80b2-9cf242e5edc8%2Fmro7ihs_processed.jpeg&w=3840&q=75)
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