If the pH = 9, which is true? [H3O+] is 1 x 10-2M and higher than [OH-] [H3O+] is 1 x 10-2M and lower than [OH-] [H3O+] is 1 x 10-5M and higher than [OH-] [H3O+] is 1 x 10-5M and lower than [OH-]
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.
![### Understanding pH and Concentration of Ions
When exploring the pH of a solution, it's essential to understand the relationship between hydrogen ions (\([H^+]\)) or hydronium ions (\([H_3O^+]\)) and hydroxide ions (\([OH^-]\)). The pH is a measure of the acidity or basicity of a solution. It is mathematically defined as the negative logarithm of the hydrogen ion concentration:
\[ \text{pH} = -\log[H^+] \]
For a neutral solution at 25°C, the concentration of hydrogen ions is \(1 \times 10^{-7} \) M, giving a pH of 7.
#### Given Question:
If the pH = 9, which of the following is true?
1. \( [H_3O^+] \) is \( 1 \times 10^{-9} \) M and higher than \( [OH^-] \)
2. \( [H_3O^+] \) is \( 1 \times 10^{-9} \) M and lower than \( [OH^-] \)
3. \( [H_3O^+] \) is \( 1 \times 10^{-5} \) M and higher than \( [OH^-] \)
4. \( [H_3O^+] \) is \( 1 \times 10^{-5} \) M and lower than \( [OH^-] \)
#### Explanation:
For a solution with pH = 9:
- The concentration of \( [H_3O^+] \) (or \( [H^+]\)) can be calculated using the formula:
\[ [H_3O^+] = 10^{-\text{pH}} \]
So,
\[ [H_3O^+] = 10^{-9} \, \text{M} \].
To determine the concentration of \( [OH^-] \), we use the water dissociation constant (\(K_w\)), which is:
\[ K_w = [H_3O^+][OH^-] = 1 \times 10^{-14} \]
Given \( [H_3O^+] = 10^{-9} \, \text{M} \):
\[ [OH^-] = \frac{K_w}{[H_3O^+](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Febe45f5d-5c04-4921-8d3a-3c73b83ec869%2F582deb7a-0c1f-4af8-9790-0b4105048a55%2Fnyrr7cs_processed.jpeg&w=3840&q=75)
Step by step
Solved in 2 steps
