Name Mass Formula Mass moles Draw v Calculations T Read aloud Ba(OH)₂ + 2Na₂SO4 → BaSO+2NaOH 1200g 171.34 g/mol 2500g 142.04 g/mol A 233.39 g/mol 40.00 g/mol
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.
![### Chemical Reaction: Barium Hydroxide and Sodium Sulfate
In this experiment, we observe the chemical reaction between barium hydroxide and sodium sulfate:
\[ \text{Ba(OH)}_2 + 2\text{Na}_2\text{SO}_4 \rightarrow \text{BaSO}_4 + 2\text{NaOH} \]
#### Reactants and Products Information
1. **Ba(OH)₂**:
- **Mass**: 1200 g
- **Formula Mass**: 171.34 g/mol
2. **2Na₂SO₄**:
- **Mass**: 2500 g
- **Formula Mass**: 142.04 g/mol
3. **BaSO₄**:
- **Formula Mass**: 233.39 g/mol
4. **2NaOH**:
- **Formula Mass**: 40.00 g/mol
#### Moles Calculation
- Use the formula:
\[
\text{Moles} = \frac{\text{Mass}}{\text{Formula Mass}}
\]
Complete calculations based on the formula mass and given mass of each substance.
#### Explanation
This setup helps in understanding stoichiometry by calculating the moles of each reactant and product. The reaction showcases the formation of barium sulfate (a precipitate) and sodium hydroxide from the reaction of barium hydroxide with sodium sulfate.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F14b65783-eb23-4822-951c-32d4f7635fee%2F226e6f56-6f6e-4ac0-9418-696a5a8092b3%2Fk30ax32_processed.jpeg&w=3840&q=75)
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