A hypothetical weak base has K = 5.0 × 108. Calculate the equilibrium concentrations of the base, its conjugate acid, and OH in a 0.15 M solution of the base. What is the pH of the solution? [B] = mol/L [HB*] = [OH-] = pH = mol/L mol/L
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.
![A hypothetical weak base has K = 5.0 × 10-8. Calculate the equilibrium concentrations of the base, its conjugate
acid, and OH in a 0.15 M solution of the base.
What is the pH of the solution?
[B] =
mol/L
[HB]=
[OH-] =
pH
=
=
mol/L
mol/L](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb33d4b5a-214d-4055-b538-8d489e592410%2Fe7c7bcd5-4c5d-40c5-8937-2b2df0d38e55%2Fqlsyhj_processed.jpeg&w=3840&q=75)
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
