Common Ion Effect in Equilibrium

In this video, Sarin explains the common ion effect, which occurs when an ion already present in a solution is increased, causing a shift in equilibrium. The video provides an example using NH4Cl and NaCl, demonstrating how adding more Cl- ions affects the equilibrium, shifting it back towards the reactants. The video concludes with a request for viewers to like and subscribe.

What is the main topic discussed in the video?

• Chemical bonding

• Acid-base reactions

• The periodic table

• The common ion effect

What does the common ion effect state?

• Equilibrium is unaffected by ion concentration

• Removing ions will stabilize equilibrium

• Adding more of the same ion will shift equilibrium

• Adding a different ion will shift equilibrium

In the example given, what happens when NaCl is added to the solution?

• It decreases the concentration of Cl- ions

• It removes NH4+ ions

• It has no effect on Cl- ions

• It increases the concentration of Cl- ions

What is the dissociation product of NH4Cl in the example?

• Na+ and Cl-

• NH3 and HCl

• NH4+ and Cl-

• NaCl and H2O

What principle is referenced to explain the shift in equilibrium?

• Boyle's Law

• Le Chatelier's Principle

• Avogadro's Law

• Dalton's Law

What is the effect of adding excess products to a reaction in solution?

• It shifts equilibrium towards the reactants

• It shifts equilibrium towards the products

• It stabilizes the equilibrium

• It has no effect on equilibrium

What happens to the equilibrium when more Cl- ions are added?

• Equilibrium shifts towards reactants

• Equilibrium shifts towards products

• Equilibrium remains unchanged

• Equilibrium is destroyed

What is the purpose of the video?

• To explore acid-base reactions

• To discuss the common ion effect

• To teach chemical bonding

• To explain the periodic table

What does the narrator ask viewers to do at the end of the video?

• Share the video

• Like and subscribe

• Watch another video

• Comment below