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 shows a series of exercises related to the calculation of hydroxide ion concentration \([OH^-]\) and hydrogen ion concentration \([H^+]\) from given pOH values. This is useful for understanding acid-base chemistry.
1. **Exercise 1**
- Given: pOH = 10.65
- Tasks:
- Calculate \([OH^-]\) in molarity (M).
- Calculate \([H^+]\) in molarity (M).
- A "Show Hint" option is available to assist with calculations.
2. **Exercise 2**
- Given: pOH = 4.28
- Tasks:
- Calculate \([OH^-]\) in molarity (M).
- Calculate \([H^+]\) in molarity (M).
- A "Show Hint" option is available to assist with calculations.
3. **Exercise 3**
- Given: pOH = 3.76
- Tasks:
- Calculate \([OH^-]\) in molarity (M).
- Calculate \([H^+]\) in molarity (M).
- A "Show Hint" option is available to assist with calculations.
These exercises require knowledge of the relationships between pOH, pH, and the concentrations of \([OH^-]\) and \([H^+]\), using the formulas:
- pH + pOH = 14
- \([OH^-] = 10^{-\text{pOH}}\)
- \([H^+] = 10^{-\text{pH}}\)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeff28e9-0e92-48ca-8dfe-2106a0442205%2F7125c329-c922-41b9-8ada-b74efd1e2e7c%2F3f4odu_processed.jpeg&w=3840&q=75)
![**Question 3**
Calculate the molar concentrations of \( \text{H}^+ \) and \( \text{OH}^- \) in solutions that have the following pOH values. Enter values in scientific notation, for example, 0.0010 would be \( 1.0 \times 10^{-3} \).
- **pOH = 12.27**
\([ \text{OH}^- ] =\) \_\_\_\_\_\_\_\_\_ M
\([ \text{H}^+ ] =\) \_\_\_\_\_\_\_\_\_ M
- **pOH = 6.14**
\([ \text{OH}^- ] =\) \_\_\_\_\_\_\_\_\_ M
\([ \text{H}^+ ] =\) \_\_\_\_\_\_\_\_\_ M
**SHOW HINT**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Faeff28e9-0e92-48ca-8dfe-2106a0442205%2F7125c329-c922-41b9-8ada-b74efd1e2e7c%2F31u98f_processed.jpeg&w=3840&q=75)
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