This is a summary practice problem set on buffer solutions aimed to help identify buffers, calculating the pH of a buffer solution prepared from a weak acid and its conjugate base or vice versa.
The links to the corresponding topics are given below:
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?
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. Kb (NH3) = 1.8 x 10-5.
Calculate the pH of the buffer solution which is 1.4 M CH3COONa and 1.8 M CH3COOH. Ka (CH3CO2H) = 1.7 x 10-5
Calculate the pH of the buffer solution that is 0.70 M NaCN and 0.55 M HCN. Ka (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. Ka (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)? Kb (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. Ka (HF) = 6.6 x 10-4
Calculate the ratio of NaNO2 to HNO2 required to create a buffer with pH = 4.00. Ka (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? Ka = 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? pKa HF = 3.8
What is the concentration of C6H5NH3Cl in the buffer solution with a pH of 4.3 containing 0.50 M C6H5NH2? Kb (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.
- 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 pKa 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
- Ksp and Molar Solubility
- The Effect of a Common Ion on Solubility
- The Effect of pH on Solubility
- Will a Precipitate Form? Ksp and Q
- Ksp and Molar Solubility Practice Problems