Ammonia (NH3) is an example of a Brønsted-Lowry Base. i. Define the Brønsted-Lowry acid-base theory. ii. What’s the pH of a solution of ammonia that has a concentration of 0.335 M? The Kb of ammonia is 1.8 × 10–5 . First complete the ICE chart. HA H3O+ A- Initial change Equlibrium iii. Calculate the pH. Please show all work
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.
Ammonia (NH3) is an example of a Brønsted-Lowry Base.
i. Define the Brønsted-Lowry acid-base theory.
ii. What’s the pH of a solution of ammonia that has a concentration of 0.335 M? The Kb of ammonia is
1.8 × 10–5
. First complete the ICE chart.
| HA | H3O+ | A- | |
| Initial | |||
| change | |||
| Equlibrium |
iii. Calculate the pH. Please show all work
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x=0.002447
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