AP Chemistry 8.3 Weak Acids & Bases

What is the relationship between the strength of an acid and its Ka value?

• Stronger acids have smaller Ka values.

• Stronger acids have larger Ka values.

• The strength of an acid is not related to its Ka value.

• Stronger acids have Ka values equal to 1.

What is the percent ionization of a 0.155 M solution of HF? pKa = 3.14

• 0.68%

• 1.97%

• 3.14%

• 6.8%

What is the pH of a 0.155 M solution of HF, given that pKa is 3.14?

• 1.97

• 3.14

• 0.68

• 2.00

According to the particle view of acids and bases, what happens when a weak acid dissociates?

• It dissociates 100% into its ions.

• It does not dissociate at all.

• It dissociates partially, producing fewer ions.

• It dissociates completely, but reversibly.

What is the expression for Kb in the context of acid-base equilibria?

• Kb = [BH+][OH-] / [B]

• Kb = [H3O+][A-] / [HA]

• Kb = [B-][H+] / [BH]

• Kb = [H+][OH-] / [B]

What does the equilibrium constant Ka represent in the context of acid dissociation?

• The change in molarity values with temperature

• The percentage of ionization of the acid

• The ratio of the concentration of products to reactants at equilibrium

• The change in molarity values when the percentage ionization changes

Tags

NGSS.HS-PS1-6

What is the hydroxide ion concentration for a solution of fluoride ion, F-, with a pH of 8.271?

• 1.87 x 10^-6 M

• 5.72 x 10^-6 M

• 1.87 x 10^-5 M

• 5.72 x 10^-5 M

Estimate the pH range for a 0.10M solution of hydroxylamine, a weak base, at 25°C.

• 4-5

• 5-6

• 9-10

• 11-12