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.
![**Question 5 of 40**
A 15.0 mL solution of Ba(OH)₂ is neutralized with 29.0 mL of 0.200 M HCl. What is the concentration of the original Ba(OH)₂ solution?
**Explanation:**
In this problem, we are given the volumes and concentration of a hydrochloric acid (HCl) solution used to neutralize a barium hydroxide [Ba(OH)₂] solution. The task is to find the concentration of the original Ba(OH)₂ solution.
**Approach:**
1. **Identify the Reaction:**
The chemical reaction between HCl and Ba(OH)₂ is as follows:
\[
2 \text{HCl} + \text{Ba(OH)}_2 \rightarrow 2 \text{H}_2\text{O} + \text{BaCl}_2
\]
2. **Calculate Moles:**
- **Moles of HCl**:
Volume of HCl = 29.0 mL = 0.0290 L
Concentration of HCl = 0.200 M
\[
\text{Moles of HCl} = 0.200 \, \text{mol/L} \times 0.0290 \, \text{L} = 0.0058 \, \text{mol}
\]
- **Moles of Ba(OH)₂**:
From the stoichiometry of the reaction, 2 moles of HCl react with 1 mole of Ba(OH)₂. Hence, the moles of Ba(OH)₂ is half the moles of HCl.
\[
\text{Moles of Ba(OH)}_2 = \frac{0.0058}{2} \, \text{mol} = 0.0029 \, \text{mol}
\]
3. **Determine the Concentration of Ba(OH)₂**:
Volume of Ba(OH)₂ = 15.0 mL = 0.0150 L
\[
\text{Concentration of Ba(OH)}_2 = \frac{0.0029 \, \text{mol}}{0.0150 \, \text{L}} = 0.193 \](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1e4f7fd3-dbae-49c8-b999-a719c9747eb1%2F59de6ce9-7e7f-4580-a876-6523a08f9d17%2Fz0uoxv6_processed.png&w=3840&q=75)
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