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.
![**Problem: Neutralization of Sr(OH)₂ with HNO₃**
**Question 7 of 12**
A 35.0 mL solution of Sr(OH)₂ is neutralized with 29.5 mL of 0.200 M HNO₃. What is the concentration of the original Sr(OH)₂ solution?
**Solution Details:**
To solve this problem, use the concept of neutralization where the number of moles of acid equals the number of moles of base at the equivalence point. The balanced chemical equation for the reaction is:
\[ \text{Sr(OH)}_2 + 2\text{HNO}_3 \rightarrow \text{Sr(NO}_3)_2 + 2\text{H}_2\text{O} \]
From the equation, 1 mole of Sr(OH)₂ reacts with 2 moles of HNO₃.
1. Calculate moles of HNO₃:
- Volume = 29.5 mL = 0.0295 L
- Molarity = 0.200 M
- Moles = Molarity × Volume = 0.200 × 0.0295 = 0.00590 moles
2. Calculate moles of Sr(OH)₂:
- From the equation, moles of Sr(OH)₂ = 0.00590 / 2 = 0.00295 moles
3. Calculate concentration of Sr(OH)₂:
- Volume = 35.0 mL = 0.0350 L
- Concentration = Moles / Volume = 0.00295 / 0.0350 = 0.0843 M
Thus, the concentration of the original Sr(OH)₂ solution is 0.0843 M.
**Note:** For educational purposes, carefully analyze the stoichiometry of the balanced equation to understand the mole relationships.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F803dbeea-4603-428a-b06b-91b3f08051c4%2F1d4662fd-233c-4786-adf0-4c5d1f353f62%2Fbks26t_processed.jpeg&w=3840&q=75)
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