Multiple Choice
Which of the following best explains why all living cells need pH buffers?
18. Aqueous Equilibrium
Intro to Buffers
Back18. Aqueous Equilibrium
Intro to Buffers
- Multiple ChoiceWhy are buffers important in living organisms?
- Multiple ChoiceWhich statement is true about pH buffers?
- Multiple Choice
Which one of the following combinations does not create a buffer?
- Multiple Choice
Which of the following combinations can result in the formation of a buffer?
- Multiple Choice
Which of the following combinations can result in the formation of a buffer?
- Multiple Choice
A buffer solution is comprised of 50.0 mL of a 0.100 M HC2H3O2 and 60.0 mL of a 0.100 M NaC2H3O2. Which of the following actions would completely destroy the buffer?
- Multiple Choice
Calculate the pH of a solution formed by mixing 200 mL of a 0.400 M C2H5NH2 solution with 350 mL of a 0.450 M C2H5NH3+ solution. (Kb of C2H5NH2 is 5.6 x 10 -4).
- Multiple Choice
Determine how many grams of sodium acetate, NaCH3CO2 (MW:82.05 g/mol), you would mix into enough 0.065 M acetic acid CH3CO2H (MW:60.05 g/mol) to prepare 3.2 L of a buffer with a pH of 4.58. The Ka is 1.8 x 10-5.
- Multiple Choice
A buffer solution is made by combining a weak acid with its conjugate salt. What will happen to the pH if the solution is diluted to one-fourth of its original concentration?
- Multiple ChoiceWhich of the following statements is true about a solution prepared with equal amounts of HNO2 and NaNO2?
- Multiple ChoiceThe addition of which of the following would destroy a 1.0 L buffer that is 0.50 M HC2H3O2 and 0.40 M NaC2H3O2?
- Multiple ChoiceWhich of the following would produce a buffer?
- Multiple ChoiceWhat is the pH of a 1.0 L buffer solution containing 0.500 M HF and 0.300 M NaF. Ka for HF = 3.5 × 10−4.
- Multiple ChoiceDetermine the pH of a 1.0 L buffer prepared by adding 0.100 moles of NaOH to 0.250 moles of HF. Ka for HF = 3.5 × 10−4.