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 is the solubility of MgCO₃ in a solution that contains 0.085 M Mg²⁺ ions? (Ksp of MgCO₃ is 3.5 × 10⁻⁸)
**Explanation:**
To determine the solubility of magnesium carbonate (MgCO₃) in a solution with a given concentration of magnesium ions (Mg²⁺), we use the concept of the solubility product constant (Ksp). The Ksp represents the equilibrium constant for the dissolution of a sparingly soluble ionic compound. For MgCO₃, the dissolution reaction can be written as:
\[ \text{MgCO}_3 (s) \rightleftharpoons \text{Mg}^{2+} (aq) + \text{CO}_3^{2-} (aq) \]
The Ksp expression for this equilibrium is:
\[ \text{Ksp} = [\text{Mg}^{2+}][\text{CO}_3^{2-}] \]
We are given:
- Ksp of MgCO₃ = 3.5 × 10⁻⁸
- Initial concentration of Mg²⁺ = 0.085 M
The solubility of MgCO₃ can be determined by calculating the concentration of carbonate ions \([\text{CO}_3^{2-}]\) in equilibrium. Given that additional Mg²⁺ ions are already present in the solution, we have the following equilibrium concentrations:
\[ 0.085 + s \approx 0.085 \]
(Where \(s\) is the small increase in \([\text{Mg}^{2+}]\))
Now substitute into the Ksp expression:
\[ 3.5 \times 10^{-8} = 0.085 \times [\text{CO}_3^{2-}] \]
Solving for \([\text{CO}_3^{2-}]\):
\[ [\text{CO}_3^{2-}] = \frac{3.5 \times 10^{-8}}{0.085} \]
Calculate to find the solubility in terms of concentration:
\[ [\text{CO}_3^{2-}] = 4.12 \times 10^{-7} \, \text{M} \]
Thus, the solubility of MgCO₃ in the](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa91f799b-1b33-41a5-8f4e-af83231854b4%2Fa1a764df-f4e7-47fe-b86e-718dc9bcb45d%2Fy8u8p2h_processed.png&w=3840&q=75)
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