The hydroxide ion concentration in an aqueous solution at 25°C is 0.076 M. The hydronium ion concentration is M. The pH of this solution is The pOH is
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.
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![**Aqueous Solution Ion Concentrations**
The hydroxide ion concentration in an aqueous solution at 25°C is 0.076 M.
**Hydronium Ion Concentration:**
The hydronium ion concentration is [ ] M.
**pH of the Solution:**
The pH of this solution is [ ].
**pOH:**
The pOH is [ ].](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e7279b6-864f-464c-a490-1592f397f56d%2F1170f48f-6a5c-4e4c-9179-0470a0c30f07%2Femd31rq_processed.png&w=3840&q=75)
![**The pOH of an aqueous solution at 25°C was found to be 11.00.**
- The pH of this solution is [____].
- The hydronium ion concentration is [____] M.
- The hydroxide ion concentration is [____] M.
**Explanation:**
To find the pH from the pOH, use the relationship:
\[ \text{pH} + \text{pOH} = 14 \]
Given pOH = 11.00,
\[ \text{pH} = 14 - 11.00 = 3.00 \]
For the hydronium ion concentration \([\text{H}_3\text{O}^+]\):
\[ [\text{H}_3\text{O}^+] = 10^{-\text{pH}} \]
\[ = 10^{-3.00} = 1.0 \times 10^{-3} \, \text{M} \]
For the hydroxide ion concentration \([\text{OH}^-]\):
\[ [\text{OH}^-] = 10^{-\text{pOH}} \]
\[ = 10^{-11.00} = 1.0 \times 10^{-11} \, \text{M} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e7279b6-864f-464c-a490-1592f397f56d%2F1170f48f-6a5c-4e4c-9179-0470a0c30f07%2Fkpg24z6_processed.png&w=3840&q=75)
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