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.
![### Neutralization Calculation Problem
**Problem Statement:**
6. What volume of a 0.100 M solution of sodium hydroxide is necessary to neutralize 100.0 mL of a 0.0500 M H₂SO₄ solution?
**Explanation:**
This problem requires a calculation of the volume of sodium hydroxide (\( NaOH \)) solution needed to completely neutralize a given volume of sulfuric acid (\( H₂SO₄ \)) solution. This is typical of stoichiometry problems in chemistry where a strong acid neutralizes a strong base.
To find the volume of \( NaOH \) required, we need to understand the neutralization reaction between \( H₂SO₄ \) and \( NaOH \). The balanced chemical equation is:
\[ H_2SO_4 + 2 NaOH \rightarrow Na_2SO_4 + 2 H_2O \]
From the equation, it can be observed that 1 mole of \( H_2SO_4 \) reacts with 2 moles of \( NaOH \).
1. First, calculate the moles of \( H_2SO_4 \):
\[ \text{Moles of } H_2SO_4 = Molarity \times Volume = 0.0500 \, M \times 0.100 \, L = 0.005 \, \text{moles} \]
2. Based on the stoichiometry of the reaction, calculate the moles of \( NaOH \) needed:
\[ \text{Moles of } NaOH = 2 \times \text{Moles of } H_2SO_4 = 2 \times 0.005 = 0.010 \text{ moles of } NaOH \]
3. Finally, using the molarity of the \( NaOH \) solution, calculate the volume of \( NaOH \) required:
\[ \text{Volume of } NaOH = \frac{\text{Moles of } NaOH}{\text{Molarity}} = \frac{0.010 \, \text{moles}}{0.100 \, M} = 0.100 \, L \text{ or } 100.0 \, mL \]
So, 100.0 mL of a 0.100 M sodium hydroxide solution is necessary to neutralize](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fff83a82c-1f8f-42f7-ab52-a9459a07e641%2F31a72ef2-7d76-4d5c-bdec-82ee8e743a91%2Fbnwr5vk_processed.png&w=3840&q=75)
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