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 2: Solubility of BaF₂ with the Addition of a Strong Acid**
*How would the solubility of BaF₂ change with the addition of a strong acid? Explain your answer.*
When explaining the effect of adding a strong acid on the solubility of barium fluoride (BaF₂), consider the following chemical principles:
1. **Dissolution Reaction:** BaF₂ dissolves in water according to the following equilibrium reaction:
\[
\text{BaF}_2(s) \rightleftharpoons \text{Ba}^{2+}(aq) + 2\text{F}^-(aq)
\]
2. **Addition of a Strong Acid:** When a strong acid (e.g., HCl) is added to the solution, it dissociates completely into H⁺ and the corresponding anion (Cl⁻ in the case of HCl). The increase in H⁺ ions in the solution will react with F⁻ ions to form HF (hydrofluoric acid):
\[
\text{H}^+(aq) + \text{F}^-(aq) \rightarrow \text{HF}(aq)
\]
3. **Le Chatelier's Principle:** According to Le Chatelier's Principle, the removal of F⁻ ions (due to the formation of HF) shifts the dissolution equilibrium of BaF₂ to the right, causing more BaF₂ to dissolve in an attempt to restore the equilibrium concentration of F⁻ ions.
4. **Increased Solubility:** Therefore, with the decrease in F⁻ concentration due to the formation of HF, more BaF₂ will dissolve, thus increasing its solubility in the presence of a strong acid.
In summary, the addition of a strong acid to a solution containing BaF₂ will increase its solubility due to the removal of F⁻ ions from the solution, shifting the equilibrium toward the dissolution of more BaF₂.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F24666b77-75da-49bd-bf84-8c4674dedd2c%2Ff275cd78-0e17-43ba-99bb-95f51c543c3e%2Fbt3xv9.png&w=3840&q=75)
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