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:**
Calculate the molar solubility of gallium hydroxide, Ga(OH)₃ (Kₛₚ = 7.28 x 10⁻³⁶), in a solution that is buffered at pH = 3.59.
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**Detailed Explanation:**
In this problem, we are asked to find the molar solubility of gallium hydroxide, Ga(OH)₃, in a solution with a specific pH value. The provided data includes the solubility product constant (Kₛₚ) for Ga(OH)₃, which is 7.28 x 10⁻³⁶. Additionally, the pH of the solution is given as 3.59.
To solve this problem, we will use the concept of solubility product constant and the relationship between pH and hydroxide ion concentration to determine the molar solubility.
**Steps:**
1. **Determine the hydrogen ion concentration from the pH of the solution:**
\[ \text{pH} = 3.59 \]
\[ \text{[H⁺]} = 10^{-\text{pH}} \]
\[ \text{[H⁺]} = 10^{-3.59} \]
2. **Calculate the hydroxide ion concentration using the water dissociation constant (K_w):**
\[ K_w = [H⁺][OH⁻] = 1 \times 10^{-14} \]
\[ \text{[OH⁻]} = \frac{K_w}{[H⁺]} \]
3. **Set up the expression for the solubility product constant of Ga(OH)₃:**
\[ \text{Ga(OH)₃ (s)} \rightleftharpoons \text{Ga³⁺ (aq)} + 3\text{OH⁻ (aq)} \]
\[ Kₛₚ = [\text{Ga³⁺}][\text{OH⁻}]³ \]
4. **Express the molar solubility (s) in terms of [Ga³⁺] and [OH⁻]:**
Given: \( [\text{Ga³⁺}] = s \) and \( [\text{OH](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fdb02c8bf-339c-4ae2-9d8b-8db604f1f70e%2F06bf6fc1-2588-4ad6-a4a5-a8ecd53a8d77%2Fiv7s7t_processed.jpeg&w=3840&q=75)
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