A solution is prepared that is initially 0.49M in pyridine (C5H₂N), a weak base, and 0.40M in pyridinium chloride (C5H5NHC1). Complete the reaction table below, so that you could use it to calculate the pH of this solution. Use x to stand for the unknown change in OH. You can leave out the M symbol for molarity. [C,H.N] [C₂H₂NH*] [OH-] initial 00 0 change 0 0 final 0 0 0 0 00
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.
![## Reaction Table Preparation for pH Calculation of Pyridine Solution
### Problem Statement
A solution is prepared that is initially 0.49 M in pyridine (C₅H₅N), a weak base, and 0.40 M in pyridinium chloride (C₅H₅NHCl). Complete the reaction table below, so that you could use it to calculate the pH of this solution.
Use \( x \) to stand for the unknown change in \( \left[ \text{OH}^- \right] \). You can leave out the \( M \) symbol for molarity.
### Reaction Table
| | [C₅H₅N] | [C₅H₅NH⁺] | [OH⁻] |
|:---------------------:|:-------:|:---------:|:-----:|
| **Initial** | 0.49 | 0.40 | 0 |
| **Change** | -x | +x | +x |
| **Final** | 0.49 - x| 0.40 + x | x |
This table represents the concentrations of pyridine (\( \text{C}_5\text{H}_5\text{N} \)), pyridinium ion (\( \text{C}_5\text{H}_5\text{NH}^+ \)), and hydroxide ion (\( \text{OH}^- \)) as they change throughout the reaction. Initially, there are 0.49 M of pyridine and 0.40 M of pyridinium ion, with no hydroxide ions present. As the reaction proceeds, the concentrations change by \( x \), resulting in final concentrations of \( 0.49 - x \) for pyridine, \( 0.40 + x \) for pyridinium ion, and \( x \) for hydroxide ions.
This table will aid in calculating the equilibrium concentrations of the species involved, which can then be used to determine the pH of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7c14a699-de9b-4c1d-9356-4bb35f1041ad%2F4f7b231e-c562-4302-9ba2-45b90ccafb76%2Fx2q5qb_processed.jpeg&w=3840&q=75)
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