Acid Dissociation Constant Concepts

The video tutorial explains how to calculate the concentrations of components in a 0.1 M chloroacetic acid solution that is 11% ionized. It introduces the ICE method to determine initial, change, and equilibrium concentrations. The tutorial walks through the calculation of ionization changes and equilibrium concentrations, leading to the determination of the acid dissociation constant, Ka.

What is the initial concentration of chloroacetic acid in the solution?

• 0.11 M

• 0.01 M

• 0.1 M

• 1 M

What does the ICE method stand for in equilibrium calculations?

• Initial, Concentration, Equilibrium

• Ionization, Concentration, Equilibrium

• Initial, Change, Equilibrium

• Ionization, Change, Equilibrium

How much of the chloroacetic acid is ionized in the solution?

• 1%

• 10%

• 0.11%

• 11%

What is the change in concentration of H+ ions due to ionization?

• 0.11 M

• 0.011 M

• 0.1 M

• 0.001 M

What is the equilibrium concentration of the undissociated chloroacetic acid?

• 0.011 M

• 0.1 M

• 0.089 M

• 0.9 M

What is the equilibrium concentration of the conjugate base?

• 0.089 M

• 0.1 M

• 0.011 M

• 0.001 M

What is the equilibrium concentration of H+ ions?

• 0.011 M

• 0.1 M

• 0.089 M

• 0.001 M

What is the formula used to calculate the acid dissociation constant (Ka)?

• Difference of products and reactants

• Sum of products and reactants

• Reactants over products

• Products over reactants

What is the calculated value of the acid dissociation constant (Ka) for chloroacetic acid?

• 1.4 x 10^-3

• 1.36 x 10^-3

• 1.4 x 10^-2

• 1.36 x 10^-2

What is the rounded value of the acid dissociation constant (Ka) for chloroacetic acid?

• 1.36 x 10^-2

• 1.4 x 10^-2

• 1.36 x 10^-3

• 1.4 x 10^-3