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.
![**pH and pOH Calculations in Aqueous Solutions**
**Question:**
The H⁺ concentration in an aqueous solution at 25°C is 1.1 x 10⁻⁴ M. What is [OH⁻]?
**Instructions:**
To find the concentration of hydroxide ions, [OH⁻], use the formula:
\[ \text{[H⁺]} \times \text{[OH⁻]} = 1.0 \times 10^{-14} \, \text{at 25°C} \]
To calculate [OH⁻]:
\[ \text{[OH⁻]} = \frac{1.0 \times 10^{-14}}{\text{[H⁺]}} \]
Using the given [H⁺] concentration:
\[ \text{[OH⁻]} = \frac{1.0 \times 10^{-14}}{1.1 \times 10^{-4}} \]
Perform the calculation to find [OH⁻].
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**Additional Resources:**
For further understanding of the relationship between [H⁺] and [OH⁻] in water at 25°C, review the concept of the water ion product constant (\(K_w\)), and how it affects the pH and pOH of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6895f9cd-8521-4c9a-bc62-df11c4ac3cae%2Fc394de10-ec9b-4942-b9f4-293f11c19a3e%2Fco5ra2l_processed.jpeg&w=3840&q=75)
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