1. Consider Ammonia, NH3, with Kb= 1.8x10-5 (a) What is the pH of a buffer solution prepared by adding 13.36g of ammonium chloride (NH4Cl) to .50 L of .400 M (b) What is the pH of the buffer after 100.0 mL of 1.50 M HCl are added to the solution from part (a)? (c) What is the pH of the buffer after 4.00g of NaOH are added to the solution from part (a)? (d) What is the pH of the buffer after 30.0g of NaOH are added to the solution from part (a)?
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.
1. Consider Ammonia, NH3, with Kb= 1.8x10-5
(a) What is the pH of a buffer solution prepared by adding 13.36g of ammonium chloride (NH4Cl) to .50 L of .400 M
(b) What is the pH of the buffer after 100.0 mL of 1.50 M HCl are added to the solution from part (a)?
(c) What is the pH of the buffer after 4.00g of NaOH are added to the solution from part (a)?
(d) What is the pH of the buffer after 30.0g of NaOH are added to the solution from part (a)?
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
