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 Calculation for Hydroxide Ion Concentration**
*Question 30 of 44*
The pH of a solution is 3.95. What is the OH⁻ concentration in the solution?
*Interface Overview*
The interface provided contains a digital calculation pad which includes the following keys:
- Number keys (0-9)
- A decimal point (.)
- A +/- key for changing the sign
- An 'x 10⁰' button for scientific notation
- A backspace key (⟵)
- A clear button (C)
- A 'M' symbol for inputting values (likely referring to molarity or concentration in moles per liter)
- A submit button at the top right corner
*Introduction to pH and OH⁻ Concentration Calculations*
pH is a measure of the acidity or basicity of an aqueous solution. It is calculated as the negative logarithm of the hydrogen ion concentration:
\[ \text{pH} = -\log [\text{H}^+] \]
The relationship between pH and pOH (the measure of hydroxide ion concentration) in any aqueous solution at 25°C is given by the equation:
\[ \text{pH} + \text{pOH} = 14 \]
To find the hydroxide ion concentration \([ \text{OH}^- ]\), follow these steps:
1. Calculate the pOH:
\[ \text{pOH} = 14 - \text{pH} \]
\[ \text{pOH} = 14 - 3.95 = 10.05 \]
2. Use the pOH to find the hydroxide ion concentration:
\[ [\text{OH}^-] = 10^{-\text{pOH}} \]
\[ [\text{OH}^-] = 10^{-10.05} \]
Using a calculator, this will yield:
\[ [\text{OH}^-] \approx 8.91 \times 10^{-11} \text{M} \]
*Summary*
Given a solution with a pH of 3.95, the concentration of hydroxide ions (OH⁻) in the solution can be calculated to be approximately \( 8.91 \times 10^{-11} \) M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fabf3f71a-8f38-4387-af5c-ba72dda07b09%2F7cfbe3a1-4396-4363-95eb-93432fca7873%2F9jm5m06_processed.png&w=3840&q=75)
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