February 14

A very dilute solution of a weak acid has a concentration of 1.3x10^-4 M, the K_a of the weak acid is 1.0x10^-18. What is the pKa of the weak acid?

pKa = -log(Ka)

• 18.0

• 18

• 18.00

• 18.000

A very dilute solution of a weak acid has a concentration of 1.3x10^-4 M, the K_a of the weak acid is 1.0x10^-18. What is the [H⁺] of the solution?

Hint: The H⁺ concentration of water in 1.0x10^-7. Does your answer make sense for an acidic solution?

• 1.000114x10^-7

• 1.3x10^-4

• 1.14018x10^-11

• 1.3x10^-22

What does that make the pH?

What is the H⁺ concentration of a 0.81 M solution of H₂SO₄?

• 0.13 M

• 1.3 M

• 1.0 M

• 0.0 M

What is the pH of a 0.81 M solution of H₂SO₄?

• 9.7

• 9.69

• 9.15

• 9.2

Does a reaction's equilibrium favor strong or weak acids?

• Strong

• Weak

Why does a reaction favor the weak acid/base?

What is the relationship between Kw, Ka and Kb?

• Ka = Kw - Kb

• Ka = Kw/Kb

• Ka = Kb/Kb

Select all the strong acids.

• HF

• HCl

• HBr

• HClO₄

• H₂SO₄

How do you know if a base is a strong base?