For the following acid-base reaction, predict which side of the equilibrium is favored.
A) favor right side
B) favor left side
C) neither

Question

For the following acid-base reaction, predict which side of the equilibrium is favored. 
A) favor right side 
B) favor left side 
C) neither

Quizplus · Accepted Answer

The reaction involves the reaction of a strong acid (HCl) with a weak base (NH3) to form a weak acid (NH4Cl) and a strong base (OH-). According to Le Chatelier's principle, the reaction will favor the side that opposes an increase in the concentration of the species. Since NH4+ and Cl- are both spectator ions, they will not affect the equilibrium. However, the addition of H+ ions (from HCl) will shift the equilibrium to the right, favoring the formation of NH4+ and OH- ions. Therefore, the right side of the equilibrium is favored.

For the Following Acid-Base Reaction, Predict Which Side of the Equilibrium