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.
![**Question:**
What is the pH of a 0.555M solution of NaF?
**Explanation:**
This question requires determining the pH of a sodium fluoride (NaF) solution with a given molarity. NaF is a salt that completely dissociates in water to form sodium ions (Na⁺) and fluoride ions (F⁻).
**Steps to Solution:**
1. **Understand the Base Reaction:** NaF dissociates in water, allowing the fluoride ion (F⁻) to act as a weak base. The fluoride ion reacts with water to form hydrogen fluoride (HF) and hydroxide ions (OH⁻):
\[ \text{F}^- + \text{H}_2\text{O} \rightarrow \text{HF} + \text{OH}^- \]
2. **Determine Kb:**
We need the base dissociation constant (Kb) for F⁻, which is related to the acid dissociation constant (Ka) of HF:
\[ K_{\text{a}}(\text{HF}) \times K_{\text{b}}(\text{F}^-) = K_{\text{w}} \]
\( K_{\text{w}} \) is the ion-product constant of water (\(1.0 \times 10^{-14} \, \text{at 25°C}\)).
3. **Calculate Hydroxide Concentration:**
Use the Kb value and the initial concentration of F⁻ to find OH⁻ concentration. Use the formula:
\[ [OH^-] = \sqrt{K_{\text{b}} \times [F^-]} \]
4. **Convert to pH:**
Calculate pOH from OH⁻ concentration:
\[ \text{pOH} = -\log[OH^-] \]
Then, convert to pH using:
\[ \text{pH} = 14 - \text{pOH} \]
These calculations will provide the pH of the 0.555M NaF solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5b8356a3-8ffd-4b0d-99e3-2fe5523dae0d%2F66f7570d-7eb0-45f5-a202-c85dfd7f9242%2F14ureqq_processed.jpeg&w=3840&q=75)
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