Which of the following solutions can be classified as buffer solutions?

(a) NaBr + HBr, (b) NaHSO₄ + H₂SO₄, (c) HCl + HOCl (d) Na₂HPO₄ + NaH₂PO₄, (e) CH₃CH₂NH₂ + CH₃CH₂NH₃⁺ (f) NaNO₂ + HNO₂, (g) KCN + HCN, (h) Na₂SO₄ + NaHSO₄, (i) NH₃ + NH₄ClO₃, (j) CH₃CO₂H + NaOH.

Addition of which salt will suppress the ionization of HOCl?

1. Na₂SO₄
2. KNO₃
3. NaOCl
4. NaNO₂

A solution of ammonia and ammonium chloride is a common buffer system. Write the corresponding reactions to show how it resists a pH change when an acid or a base is added to it.

Calculate the pH of the buffer solution consisting of 0.75 M NH₃ and 0.95 M NH₄Cl. K_b (NH₃) = 1.8 x 10^-5.

Calculate the pH of the buffer solution which is 1.4 M CH₃COONa and 1.8 M CH₃COOH. K_a (CH₃CO₂H) = 1.7 x 10^-5

Calculate the pH of the buffer solution that is 0.70 M NaCN and 0.55 M HCN. K_a (HCN) = 4.9 x 10^-10

Calculate the pH of the buffer solution that is 0.60 M propionic acid (CH₃CH₂CO₂H) and 0.75 M sodium propionate. K_a (CH₃CH₂CO₂H) = 1.32 x 10^-5

What is the pH of a buffer solution that is 0.85 M pyridine (C₅H₅N) and 1.3 M pyridinium chloride (C₅H₅NHCl)? K_b (C₅H₅N) = 1.7 x 10^-9 16.82

Calculate the pH of a solution that is 0.8 M HF and 2.0 M NaF. K_a (HF) = 6.6 x 10^-4

Calculate the ratio of NaNO₂ to HNO₂ required to create a buffer with pH = 4.00. K_a (HNO₂ = 7.2 x 10^-4)

Assuming no volume change, how many grams of sodium benzoate (C₇H₅O₂Na) needs to be added to 250.0 mL of a 0.25 M benzoic acid (C₇H₅O₂H) solution to prepare a buffer with a pH of 4.60? K_a = 6.46 x 10^-5

How many mL of 0.60 M HF and 0.70 M NaF must be mixed to prepare 1.00 L of a buffer solution at pH of 4.2? pK_a HF = 3.8

What is the concentration of C₆H₅NH₃Cl in the buffer solution with a pH of 4.3 containing 0.50 M C₆H₅NH₂? K_b (C₆H₅NH₂) 3.8 x 10^-10

Which of the following pairs is the best choice to prepare a buffer with pH = 3.2 ?

In what mass ratio would you add the components to prepare the buffer.

a) CH₃COOH and CH₃COONa b) HNO₂ and KNO₂ c) NH₃ and NH₄Cl d) C₅H₅N and C₅H₅NHCl.

What would be the pH of a buffer solution composed of 0.60 M NH₃/0.45 M NH₄Cl after 0.010 mole of gaseous HCl is added to a 400.0 mL solution?

Calculate the pH after 20.0 g NaOH(s) is added to 1.0 L of a buffer solution containing 1.80 M acetic acid and 1.50 M sodium acetate at pH 4.0.

Check Also

• Buffer Solutions
• The Henderson–Hasselbalch Equation
• The pH of a Buffer Solution
• Preparing a Buffer with a Specific pH
• The Common Ion Effect
• The pH and pK_a Relationship
• Strong Acid–Strong Base Titrations
• Titration of a Weak Acid by a Strong Base
• Titration of a Weak Base by a Strong Acid
• Titration of Polyprotic Acids
• Buffer Solutions Practice Problems
• K_sp and Molar Solubility
• The Effect of a Common Ion on Solubility
• The Effect of pH on Solubility
• Will a Precipitate Form? K_sp and Q
• K_sp and Molar Solubility Practice Problems