Multiple Choice
What mass of NaC2H3O2 (molar mass = 82.03 g/mol) would need to be added to 0.450 moles of HC2H3O2 to prepare a 1.0 L buffer with a pH = 4.95. Ka for HC2H3O2 = 1.8 × 10−5.
18. Aqueous Equilibrium
Intro to Buffers
Back18. Aqueous Equilibrium
Intro to Buffers
- Multiple Choice1.0 L of a buffer is prepared to produce a solution that is 0.400 M in HF and 0.250 M in LiF. What is the pH after the addition of 2.5 g of KOH? Assume no volume change.
Ka for HF = 3.5 × 10−4. - Multiple Choice
Which pairs of compounds are capable of making a buffer? Select all that apply.
a) 1.3 M LiOH and 1.7 M HCOOH c) 0.35 M CH3CO2H and 0.35 M NaOH
b) 0.784 M NH4+ and 0.800 M HClO4 d) 0.80 HNO3 and 0.15 MgO
- Multiple Choice
Determine which of the following actions will destroy a buffer composed of 0.50 L of 1.44 M H3PO4 and 0.60 L of 1.25 M NaH2PO4−.
a) Addition of 1.45 moles of KH2PO4
b) Addition of 0.85 moles of HCl
c) Addition of water
d) Addition of 0.30 moles of Ca(OH)2
e) Addition of 0.70 moles of HIO4
- Open Question
A buffer resists change in ph when ___________ amount of acid or base is added to it.
- Open QuestionWhich of the following solutions represents a good buffer system?
- Open Question
A solution that resists a change in ph when an acid or base is added to it is a(n) __________.
- Open Question
Select the statement that best describes a buffer. see concept 3.3 (page)
- Open Question
A(n) is a substance or a mixture of substances that act to resist changes in pH.
- Open Question
Which of the following is a means of creating a buffer of H2CO3/NaHCO3₃?
- Open QuestionWhich of the following solutions is a good buffer system?
- Open QuestionWhich of the following aqueous solutions are good buffer systems?
- Multiple ChoiceA buffer solution is prepared by adding 9.04 mL of 1.27 M HBr to 190.0 mL of 0.11 M methylamine solution. The buffer is allowed time to establish. Then, 0.005 mol of a strong base is added. What is the pH of the resulting solution? Round your answer to 2 decimal places.
- Multiple ChoiceA 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 0.150 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10^-4.
- Multiple ChoiceA 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. The Ka for HF is 3.5 × 10⁻⁴.