Analytical chemistry 2 , Lecture 2

According to the Bronsted-Lowry definition, an acid is a substance that:

• Accepts a proton

• Donates a proton

• Accepts an electron pair

• Donates an electron pair

Which equation represents the law of mass action for a monoprotic acid (HAc)?

• Ka = [H+][Ac-] / [HAc]

• Ka = [HAc] / [H+][Ac-]

• Ka = [H+][HAc] / [Ac-]

• Ka = [H+][HAc] / [Ac-]

in an acidic solution, which of the following is true?

• [H+] = [OH-]

• [H+] > [OH-]

• [H+] < [OH-]

• pH is more than 7

What is the relationship between pH and pOH?

• pH + pOH = 10

• pH - pOH = 7

• pH + pOH = 14

• pH × pOH = 14

Which of the following is NOT a property of a strong acid?

• Completely ionizes in solution

• Has a high Ka value

• Has a low Ka value

• Forms a weak conjugate base

Which of the following compounds can act as an acid but does NOT contain hydrogen?

• NaOH

• H2O

• BCl3

• NH3

the pH of acidic buffer =

• pH = pKa + log [salt] / [base]

• pH = pKb + log [salt] / [base]

• pH = pKa + log [salt] / [acid]

• pH = pKa - log [salt] / [acid]

Maximum Buffer Capacity occurs when:

• [acid]= [base]

• pH = Pka

• pH < Pka

• pH = pKa ± 1