Acid - Base Equilibrium

Consider the general equation for an acid in water:
HA(aq) + H₂O ↔ H₃O⁺ + A^-
If there is a lot of product, what does that tell you about the acid?

• K_a > 1  Strong acid
• K_a > 1  Weak acid
• K_a < 1  Strong acid
• K_a < 1  Weak acid

Which of the following is a conjugate acid/base pair?

• HCl/OCl^-
• H₂SO₄/SO₄^2-
• NH₄⁺/NH₃
• H₃O⁺/OH^-

Which of the following is not a strong acid?

• nitric
• sulfuric
• perchloric
• hydrofluoric

Which of the following is the conjugate acid of HCO₃^-1?

• H₂CO₃
• CO₃^-2
• H₂CO_3^-1
• CO₃^-1

The pH at the equivalence point of the titration of a strong acid with a strong base is:

• 3.9
• 4.5
• 7.0
• 8.2

The pH of a solution at 25^ₒC in which [OH-] = 3.9 x 10^-5M is:

• 4.41
• 3.90
• 9.59
• 4.80

• Is the dissociation constant of weak acid reaction.

• Is the dissociation constant of weak base reaction. 

• Is the dissociation constant of the Auto Ionization of water. 

• Is the dissociation constant of any equilibrium reaction. 

Acidic buffer is made up of

• weak acid and weak base
• weak acid and its conjugate salt
• weak acid and its conjugate base
• strong acid and its conjugate base

a buffer solution is made by mixing HA, a weak acid, with salts containing A^- ions.

HA ↔ H⁺ + A^-

a formula that can be used for the calculation of the pH of this buffer solution is

• 
• 
• 
• 

a buffer solution is made of mixture of aqueous ethanoic acid, CH₃COOH, with aqueous potassium ethanoate, KCH₃COO.

the equilibrium reaction takes place in buffer solution is :

CH₃COOH ↔ CH₃COO^- + H⁺

small amount of HCl is then added to that buffer solution.

What reaction take places at the buffer solution to resist change of pH caused by addition of acid?

• CH₃COO^- + H⁺ → CH₃COOH

• CH₃COO^- + OH^- → CH₂COO^2- + H₂O

• CH₃COOH + H⁺ → CH₃COOH₂

• CH₃COOH + OH^- → CH₃COO^- + H₂O