An analytical chemist is titrating 166.5 mL of a 0.6300M solution of hydrazoic acid (HN3) with a 1.000M solution of NaOH. The pK of hydrazoic acid is 4.72. Calculate the pH of the acid solution after the chemist has added 27.27 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. pH = X
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.
need help with this chemistry
![**Titration of Hydrazoic Acid with Sodium Hydroxide**
An analytical chemist is performing a titration process involving hydrazoic acid (HN₃) and sodium hydroxide (NaOH). Here are the specifics of the experiment:
- **Volume of Hydrazoic Acid:** 166.5 mL
- **Concentration of Hydrazoic Acid:** 0.6300 M
- **Concentration of Sodium Hydroxide:** 1.000 M
- **Volume of Sodium Hydroxide added:** 27.27 mL
- **pKa of Hydrazoic Acid:** 4.72
**Objective:**
Calculate the pH of the acid solution after the chemist has added 27.27 mL of the NaOH solution.
**Instructions:**
1. Assume the final volume equals the initial volume of the solution plus the volume of the NaOH solution added.
2. Round your calculated pH to two decimal places.
**Solution Format:**
The solution should be entered where indicated:
\[ \text{pH} = \ _ \]
The steps to compute the pH involve using the concepts of acid-base titration, taking into account the neutralization reaction between the strong base (NaOH) and the weak acid (HN₃). The endpoint of this titration, the volume of titrant added, and the characteristics of the involved chemicals guide the calculation to the resulting pH.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12c0a0e9-4d98-45bb-8c42-bb6fd08d9097%2Fcf52ef38-a61a-49f2-9e4e-5c6b67d6c5bb%2Fc9k8la7_processed.png&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 4 steps with 4 images
