Acid and Base Dissociation Concepts

What is the formula to calculate pKa from Ka?

• pKa = 10^(-Ka)

• pKa = -log10(Ka)

• pKa = Ka + 1

• pKa = log10(Ka)

If a weak acid has a Ka of 1.0 x 10^-5, what is its pKa?

• 6

• 5

• 4

• 7

Define the difference between strong and weak acids.

• Strong acids fully dissociate in solution; weak acids partially dissociate.

• Strong acids have a higher pH than weak acids.

• Weak acids do not dissociate at all in solution.

• Strong acids are always more concentrated than weak acids.

What is the relationship between Ka and Kb for a conjugate acid-base pair?

• Ka - Kb = Kw

• Ka + Kb = Kw

• Ka * Kb = Kw (1.0 x 10^-14) for a conjugate acid-base pair.

• Ka / Kb = Kw

How do you calculate the pH of a solution given its Ka value?

• pH = 14 - log(Ka)

• pH = log(Ka * C)

• pH = sqrt(Ka / C)

• pH = -log(sqrt(Ka * C))

If the pH of a solution is 3, what is the concentration of hydrogen ions?

• 0.1 M

• 0.01 M

• 0.001 M

• 0.0001 M

What is the pKb of a base if its Kb is 1.0 x 10^-6?

• 6

• 5

• 7

• 8

How do you determine if an acid is strong or weak based on its Ka value?

• An acid is strong if its Ka value is greater than 1; it is weak if its Ka value is less than 1.

• An acid's strength is determined solely by its concentration, not its Ka value.

• An acid is strong if its Ka value is equal to 1; it is weak if its Ka value is not equal to 1.

• An acid is strong if its Ka value is less than 1; it is weak if its Ka value is greater than 1.

Calculate the pH of a 0.1 M solution of acetic acid (Ka = 1.8 x 10^-5).

What is the significance of the dissociation constant (Ka) in acid-base chemistry?

• The dissociation constant (Ka) indicates the strength of an acid, with higher values signifying stronger acids.

• Ka is used to determine the volume of a gas produced in a reaction.

• Ka measures the temperature of a solution.

• Ka indicates the color of an acid in solution.