Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0017 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. K₂ = 4.3x10-7 Concentration = M
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.
Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0017 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40.
Ka = 4.3×10-7
![**Carbonate Buffers in Blood pH Regulation**
Carbonate buffers play a crucial role in maintaining the pH of blood at 7.40. In this exercise, you will calculate the bicarbonate ion concentration required to achieve this balance. Given that the carbonic acid concentration in a blood sample is 0.0017 M and the dissociation constant \( K_a = 4.3 \times 10^{-7} \), determine the necessary concentration of bicarbonate ions to buffer the blood at pH = 7.40.
**\[ K_a = 4.3 \times 10^{-7} \]**
Concentration = [________] M
- **Buttons:**
- **Submit Answer**: Click this to submit your calculated answer.
- **Try Another Version**: Select this option if you wish to attempt a different version of this problem.
You have 1 item attempt remaining.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F80f9f931-538e-4236-a48b-df7b3d115d0a%2F631334e2-5394-4ff6-81fe-1da1a21f938a%2Fpouk3s_processed.png&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 4 images
