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.
![**Buffer Solution pH Calculation**
If a buffer solution is 0.140 M in a weak acid (\(K_a = 5.4 \times 10^{-5}\)) and 0.500 M in its conjugate base, what is the pH?
**pH =** [Calculate here]
This question involves determining the pH of a buffer solution using the concentrations of a weak acid and its conjugate base. The acid dissociation constant (\(K_a\)) is provided. To find the pH, use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pK}_a + \log \left(\frac{[\text{A}^-]}{[\text{HA}]}\right) \]
Where:
- \([\text{HA}]\) is the concentration of the weak acid (0.140 M).
- \([\text{A}^-]\) is the concentration of the conjugate base (0.500 M).
- \(\text{pK}_a = -\log K_a\).
**Graph/Diagram Explanation**
There are no graphs or diagrams present in the image. The space provided is intended for the calculation of the pH value based on the given data.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F00154cd9-82c7-455b-845c-02cf21fdb65c%2F1556dbb7-b63f-4e8e-b0c6-35a46862ce81%2F8jnsl7x_processed.jpeg&w=3840&q=75)
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