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 Statement:
What concentration ratio of base to acid is necessary to get a buffer solution with a pH of 8.0? The given \( K_b = 1.25 \times 10^{-5} \).
**Instructions:**
Input your answer to three significant figures.
### Explanation:
In this exercise, you are asked to calculate the concentration ratio of a base to an acid required to achieve a buffer solution with a specified pH. This involves understanding the principles of buffer solutions and the relationship between \( pK_a \), \( K_b \), and pH.
For this scenario, you would typically use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pK}_a + \log\left(\frac{[\text{base}]}{[\text{acid}]}\right) \]
Given \( K_b \), you can find \( pK_a \) by using the relation between \( K_w \) (the ion product of water, \( 1.0 \times 10^{-14} \) at 25°C), \( K_a \), and \( K_b \):
\[ K_a \cdot K_b = K_w \]
Calculate \( pK_a \), plug the values into the Henderson-Hasselbalch equation, and solve for the base-to-acid ratio. The answer should be precise to three significant figures as requested.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0d520b33-7440-45bc-bf50-9535ed2d03bc%2F51604c41-3513-461f-92c7-0e36128477ae%2Ff4x17xa_processed.jpeg&w=3840&q=75)
We have to use Henderson Hasselbalch equation to calculate the ratio of base to acid.
For this we would first Calculate pKa and use given pH.
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