pH of weak acids and bases

A solution containing a weak acid will likely have a pH

• approximately 7
• between 8 and 10
• below 7 but higher than 1
• around 1

Which of these solutions, all with a concentration 1 M, will have the highest pH?

• HF (Ka = 7.2 x 10^-4)

• benzoic acid Ka = 6.3 x 10^-5)

• H₂SO₃ Ka = 1.2 x 10^-2)

• H₂CO₃ (Ka = 4.5 x 10^-7)

A solution contains 0.04 M of a weak acid. Calculate the pH of the solution knowing that the Ka for the acid is 1.6 x 10^-7

• It is not possible to solve if the identity of the acid is not known

• 4.1

• 8.1

• 1.0

What is the pH of a solution that has a [H+] concentration of 1x10^-4 ?

• 10

• 4

• .0001

• 7

• [10^-4]

Which of the following would be a weak base?

• 
• 
• 
• 

Which of the following is weak acid?

• H2CO3 (carbonic acid)

• H2SO4 (sulfuric acid)

• NH3 (ammonia)

• NaOH (sodium hydroxide)

pH of 0.1 M of HF solution is not equal with 1 because ....

• It doesn't dissociate to produce H⁺ ion

• It dissociates completely to produce H⁺ ion

• It partially dissociates to produce H⁺ ion

• It dissociates to produce H⁺ ion more than 0.1 M

Which of the following Ka value belongs to the strongest acid?

• 5 x 10^-6

• 1.8 x 10^-5

• 4 x 10^-7

• 6 x 10^-4

What is the molarity of ammonia solution if the pH is 10?

(Kb = 1 x 10^-5)

• 1 x 10^-3

• 4 x 10^-3

• 1 x 10^-4

• 2 x 10^-4