Equilibrium Concentrations and Formation Constants

The video tutorial explains the stepwise formation of complex ions Ag(NH3)+ and Ag(NH3)2+ with given formation constants. It covers writing equations for these formations, calculating the overall formation constant, and determining equilibrium concentrations using a BCA table. The tutorial also demonstrates how to write equilibrium expressions and verify calculations using different methods.

What are the formation constants for Ag(NH3)+ and Ag(NH3)2+?

• 2100 and 8200

• 5000 and 1000

• 1000 and 5000

• 8200 and 2100

Which ligand is involved in the formation of Ag(NH3)+?

• Ammonia

• Water

• Chloride

• Hydroxide

How is the overall formation constant (Kf) calculated?

• Product of K1 and K2

• Difference of K1 and K2

• Sum of K1 and K2

• Quotient of K1 and K2

What is the initial concentration of silver in the BCA table?

• 1.0 M

• 2.5 M

• 0.08 M

• 0.04 M

Why is the reaction considered to go to completion?

• Low Kf value

• High Kf value

• Presence of a catalyst

• Low temperature

What is the equilibrium concentration of NH3 after the reaction?

• 2.5 M

• 2.42 M

• 0.08 M

• 0.04 M

Which expression represents the equilibrium constant for the reaction?

• Difference of products and reactants

• Reactants over products

• Sum of products and reactants

• Products over reactants

What is the equilibrium concentration of Ag+?

• 3.966 x 10^-10 M

• 2.02 x 10^-6 M

• 2.42 M

• 0.04 M

How is the concentration of Ag(NH3)+ verified?

• Using K1 only

• Using neither K1 nor K2

• Using K2 only

• Using both K1 and K2

What is the final concentration of Ag(NH3)2+?

• 0.04 M

• 2.42 M

• 2.02 x 10^-6 M

• 3.966 x 10^-10 M