2. Consider a 200.0 mL solution that is 0.00155 M in HCl and 0.0200 M in HCIO2 ww a) Calculate the pH. b) The amount of NaOH at 0.16 g is added to the solution. (Assume no change in volume) Calculate the pH.
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
Consider a 200.0 mL solution that is 0.00155 M in HCl and 0.0200 M in HClO₂.
a) Calculate the pH.
b) The amount of NaOH at 0.16 g is added to the solution.
(Assume no change in volume)
Calculate the pH.
### Analysis
This problem involves calculating the pH of a mixed acid solution and then determining the change in pH upon the addition of a base, NaOH.
- **Part (a):** Calculate the initial pH, considering the contributions from both hydrochloric acid (HCl) and chlorous acid (HClO₂).
- **Part (b):** Account for the neutralization reaction when NaOH is added, and recalculate the pH.
### Key Concepts
- **pH Calculation:** Use the concentration of hydrogen ions [H⁺] from the acids to find the initial pH.
- **Neutralization Reaction:** Determine how the addition of NaOH, a strong base, affects the concentration of hydrogen ions in the solution.
The challenge is to combine these concepts to solve for the pH before and after the addition of NaOH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F85b22b45-c9bb-4b39-adb5-c159f78f546a%2F2dc87c31-b2d7-4dff-92d9-49ff02dd0f12%2Fy6l1y8e_processed.jpeg&w=3840&q=75)
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