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.
![### Determining the pH of a Strong Acid Solution
**Problem Statement:**
What is the pH of a \(3.48 \times 10^{-2}\) M solution of the strong acid \(HClO_4\)?
**Chemical Equation:**
\[ \text{HClO}_4(aq) + \text{H}_2\text{O}(l) \rightarrow \text{ClO}_4^{-}(aq) + \text{H}_3\text{O}^+(aq) \]
**Initial Concentration:**
\[ [\text{HClO}_4]_0 = 3.48 \times 10^{-2} \, \text{M} \]
**Calculation:**
To determine the pH of this solution, we first need to recognize that \(HClO_4\) is a strong acid, which means it dissociates completely in water. Therefore, the concentration of \(H_3O^+\) ions (hydronium ions) in the solution will be equal to the initial concentration of the acid.
The pH of a solution can be calculated using the formula:
\[ \text{pH} = -\log[\text{H}_3\text{O}^+] \]
Since the concentration of the \(H_3O^+\) ions is \(3.48 \times 10^{-2} \, \text{M}\):
\[ \text{pH} = -\log(3.48 \times 10^{-2}) \]
**Interactive Features:**
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This exercise teaches how to calculate the pH of a solution of a strong acid, emphasizing the complete dissociation property of strong acids and the use of the pH formula.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F848b3b37-0e47-4626-8c62-5eaa520ec29b%2F23400175-b8eb-4460-abed-0c50e70c31c8%2Fua9fsn9_processed.jpeg&w=3840&q=75)
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