Buffers and Titrations

If a strong acid and a strong base are titrated with one another what will the pH at the equivalence point be?

If a strong acid is titrated with a weak base what will the pH at the equivalence point be?

If you titrate a weak acid with a weak base what will the pH at the equivalence point be?

If you titrate HCl with NaCH₃COO what will the pH be at the equivalence point?

If you titrate NaOH with hexanoic acid what will the pH at the equivalence point be?

Two mols of base was titrated with a solution of HCl to reach the equivalence point. How many mols of acid are present in the solution?

0.5 L of 0.04 M acetic acid was titrated with an unknown solution of base in order to reach the equivalence point. How many moles of base does the unknown solution contain?

A 0.6 M solution of HCl was added to 25 mL of an ammonia solution. If it took 500 mL of the HCl solution to reach the equivalence point what was the original concentration of the ammonia solution?

A tris buffer (pKa=8.1) could effectively buffer a solution within what pH range?

A scientist is attempting to evaluate the function of a protein at a pH of 6. Which of the following buffers should the experiment be carried out in?

Which of the following buffers would be suitable for conducting an experiment at pH 9?

Which of the following buffers could effectively buffer a solution at a pH of 5?

A buffer is created from acetic acid (pKa =4.8) and its conjugate base acetate and adjusted to a pH of 5.8. Which of the following is true about the solution?

A buffer is created out of benzoic acid (pKa = 4.2) and its conjugate base, benzoate, and adjusted to a pH of 2.2. Which of the following is true of the solution?

A buffered solution contains 0.2 M of CHOOH (pKa = 3.7) and 0.002 M of CHOO^–. What will the pH of the buffer be? 

A buffered solution contains 0.02 M of CHOOH (pKa = 3.7) and 0.002 M of CHOO^–. What will the pH of the buffer be? 

A solution of 0.003M H₂S and 3M HS^– would have a pH of:

(Note: H₂S pKa = 7.01)

A buffered solution of acetic acid (pK_a =4.8) and acetate is adjusted to a pH of 6.8. What is the ratio of acetic acid to acetate in solution?

A buffered solution of carbonic acid (pK_a = 6.4) and bicarbonate was created and adjusted to a pH of 5.4. By what factor is the carbonic acid concentration increased in comparison to bicarbonate concentration in the buffer solution?

A buffered solution containing 0.5 M acetic acid and 0.05 M acetate has a pH of 3.4. What is the pKa of acetic acid?

A solution containing 20mL of 2M carbonic acid (pKa = 6.4) and 40 mL of 1M bicarbonate would have a pH of: