A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCI solution?
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.
![### Titration Problem
**Problem Statement:**
A student titrates 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution?
**Detailed Explanation:**
In this titration problem, the student is working with the following:
- **Volume of HCl (acid)**: 25 mL
- **Volume of KOH (base)**: 35 mL
- **Molarity of KOH**: 0.890 M
The goal is to determine the pH of the HCl solution at the equivalence point.
#### Steps to Solve:
1. **Moles of KOH**:
Calculation:
\[ \text{moles of KOH} = \text{Molarity} \times \text{Volume} \]
\[ \text{moles of KOH} = 0.890 \, \text{M} \times 0.035 \, \text{L} = 0.03115 \, \text{moles} \]
2. **At equivalence point**:
The moles of KOH will equal the moles of HCl, because KOH and HCl react in a 1:1 molar ratio:
\[ \text{moles of HCl} = 0.03115 \, \text{moles} \]
3. **Molarity of HCl**:
Calculation:
\[ \text{Molarity of HCl} = \frac{\text{moles of HCl}}{\text{Volume of HCl in Liters}} \]
\[ \text{Molarity of HCl} = \frac{0.03115 \, \text{moles}}{0.025 \, \text{L}} = 1.246 \, \text{M} \]
4. **pH of HCl solution**:
Since HCl is a strong acid, it fully dissociates in water:
\[ \text{pH} = -\log[\text{H}^+] \]
Given the concentration of HCl is equal to \([\text{H}^+]\):
\[ \text{pH}](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa9e8573f-552b-4431-b931-fec80f931989%2F887353dc-5a34-481d-8225-998ce07fc4a6%2F26prisk_processed.png&w=3840&q=75)
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