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 Statement:**
What is the pH of a solution in which 15 mL of 0.21 M NaOH is added to 25 mL of 0.21 M HCl?
**Solution:**
To find the pH of the resulting solution, we follow these steps:
1. **Calculate moles of NaOH and HCl:**
- Moles of NaOH = Volume (L) × Molarity = 0.015 L × 0.21 mol/L = 0.00315 mol
- Moles of HCl = Volume (L) × Molarity = 0.025 L × 0.21 mol/L = 0.00525 mol
2. **Determine the limiting reactant:**
Since moles of NaOH (0.00315 mol) are less than moles of HCl (0.00525 mol), NaOH is the limiting reactant. All NaOH will react with HCl.
3. **Calculate moles of excess HCl:**
Excess HCl = Initial moles of HCl - Moles of NaOH
= 0.00525 mol - 0.00315 mol = 0.00210 mol
4. **Calculate concentration of HCl in the solution:**
Total volume of the solution = 15 mL + 25 mL = 40 mL = 0.040 L
Concentration of excess HCl = moles / volume = 0.00210 mol / 0.040 L = 0.0525 M
5. **Calculate the pH:**
Since HCl is a strong acid, [H⁺] = 0.0525 M.
pH = -log[H⁺] = -log(0.0525) ≈ 1.28
Therefore, the pH of the solution is approximately 1.28.
**Conclusion:**
The solution remains acidic after the reaction, given the excess of HCl.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff2d324e2-7a67-4e3d-bb22-9ad23fbeb72b%2Fb7f62064-ef32-4d3b-b418-4e49940300f1%2Fogx8n1_processed.jpeg&w=3840&q=75)
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