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.
![The image presents a question related to calculating the pH of a solution, accompanied by a basic calculator functionality.
**Question:**
What is the pH of a 3.3 × 10⁻⁴ M CsOH solution?
**Explanation:**
This question requires the calculation of the pH of a solution where the molarity (M) of cesium hydroxide (CsOH) is given. CsOH is a strong base, which means it dissociates completely in water.
**Calculator Functionality:**
To the right side of the question is a calculator interface that includes:
- A numerical keypad with digits from 0 to 9.
- Operations like addition, subtraction, multiplication, and division are not explicitly shown.
- Specific buttons such as “x” for multiplication, “C” for clear, “+/-” for toggling positive and negative signs, “.” for a decimal point, and “x 10” likely used for scientific notation.
**Calculation Method:**
1. CsOH completely dissociates in water to form Cs⁺ and OH⁻ ions. Hence, [OH⁻] = 3.3 × 10⁻⁴ M.
2. The pOH can be calculated using the formula: pOH = -log [OH⁻].
3. After calculating the pOH, the pH can be found using the relation: pH + pOH = 14.
This information might be particularly useful for educational purposes to explain the step-by-step process of finding the pH of a basic solution using a given molarity and utilizing logarithmic functions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabf3f71a-8f38-4387-af5c-ba72dda07b09%2F38283886-d355-444e-83e8-a22af583ccb3%2Fxavoerb_processed.png&w=3840&q=75)
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