3. Prepare 100 mL of 0.200 bicarbonate buffer, pH 10 by calculating the mass of sodium bicarbonate and sodium carbonate. a. Use the Henderson-Hasselbalch equation to calculate the volume of each stock solution needed. pH = pKa + log [conjugate base] / [weak acid]1 %3D
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.
![C. Bicarbonate Buffer
3. Prepare 100 mL of 0.200 bicarbonate buffer, pH 10 by calculating the mass of sodium
bicarbonate and sodium carbonate.
a. Use the Henderson-Hasselbalch equation to calculate the volume of each stock
solution needed.
pH = pka + log [conjugate base]/ [weak acid]1
b. Check your calculations with other students. See the instructor if there is uncertainty.
c. Make the solution and check the pH of a portion of your buffer solution using the pH
%3D
meter.
L= 245µL
%3D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1e74d005-1337-463f-9c97-3fffbdaa320e%2F831424dd-9984-46f9-96f3-cd4c2dea2e7f%2Fej2c8x_processed.png&w=3840&q=75)
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