buffer solution practice problems with answers

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| By Catherine Halcomb
Catherine Halcomb
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  • 1/15 Questions

    Which of the following is TRUE?

    • A buffer cannot be destroyed by adding too much strong base. it can only be destroyed by too much strong acid.
    • An effective buffer has a [base]/[acid] ratio the range of 10 -100
    • An effective buffer has very small absolut concentrations of acid and conjugate base 
    • A buffer is most resistant to PH  change when [acid] = [conjugate base]
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About This Quiz

How good are you at solving buffer solution practice problems? Here, we have a few questions with answers based on the buffer solution in the quiz below. Give it a try and check how good your problem-solving skills are. A buffer solution is an aqueous solution consisting of a weak acid and its conjugate base. The quiz below will ask you to calculate the pH of chemical compounds using the Henderson–Hasselbalch equation. Can you do so? Play the quiz and assess yourself.

Buffer Solution Practice Problems With Answers - Quiz

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  • 2. 

    In a water molecule, hydrogens are partially ___, oxygens are partially  ____

    • Negative ; positive 

    • Positive ;  positive 

    • Positive ; negative 

    • Negative ; negative 

  • 3. 

    Which of these non-covalent bonds in biological systems is usually the weakest? 

    • Van der waals interactions 

    • Ion-dipole interaction

    • Hydrogen bond

    • Hydrophobic interaction

  • 4. 

    Which of the following would be the strongest acid?

    • Succinic acid, a diprotic acid with pk=4.21 and 5.64

    • Acetic acid pk=4.76

    • Formic acid pk=3.75

    • Ammonium ion pk=9.25

  • 5. 

    Calculate the pH of the following aqueous solutions: 1*10^-3M HCl

    • PH =4.6

    • PH =3.7

    • PH =3

    • PH =11

  • 6. 

    Calculate the pH of the aqueous solutions 1*10^-4M NaOH

    • PH=6,7

    • PH=11

    • PH=10

    • PH=8

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  • 7. 

    An aqueous solution containing a concentration of 2.5*10^-8 M NaOH will have a pH; which of the following?

    • 6.42

    • 6.40

    • 6.43

    •  642

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  • 8. 

    Using the Henderson - Hasselbalch Equation, Convince yourself that the proper ratio of A / HA for pH 7.00 PKA =7.20 calculate [HPO4^-2]/[h2po4-]

    • 0.76

    • 0.63

    • 1

    • 0.93

  • 9. 

    Using the henderson-hasselbalch equation calculate pH when 0.7 mol of NaOH is added pka=4.76 , 0.7 mol of acetic acid react  

    • 3.81

    • 4.39

    • 5.13

    • 6.15

    Rate this question:

  • 10. 

    All of the above examples on buffer in vitro except? 

    • TRIS

    • Zwitterions

    • Phosphate buffer system

    • Carbonic acid

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  • 11. 

    Which of the following statements is FALSE?

    • The hydrogen end of water molecules is attracted toward Cl- ions

    • Hydration is a special of solvation in which the solvent is water 

    • Dipole-induced dipole interactions are referred to as london-dispersion forces 

    • The oxygen end of water molecules is attracted toward ca2+ ions

  • 12. 

    Using the Henderson-Hasselbalch equation, calculate pH when 0.5 mol of NaOH is added pka=4.76 , 0.5 mol of acetic acid react  

    • 3.81

    • 4.39

    • 4.76

    • 5.13

    Rate this question:

  • 13. 

    Using the Henderson-Hasselbalch equation calculate pH when 0.3 mol of NaOH is added pka=4.76 , 0.3 mol of acetic acid react  

    • 3.81

    • 4,76

    • 4.39

    • 5.71

    Rate this question:

  • 14. 

    Which of the following identifies a good buffer?

    • Small amount of both a weak acid and its conjugate base 

    • Significant amount of both a weak acid and its conjugate base 

    • Significant amounts of both a weak acid and strong acid

    • Significant amounts of both a strong acid and strong base 

  • 15. 

    Using the Henderson-Hasselbalch equation calculate pH when 0.1 mol of NaOH is added pka=4.76 , 0.1 mol of acetic acid react  

    • 3.81

    • 4.39

    • 4,76

    • 5.71

    Rate this question:

Quiz Review Timeline (Updated): Dec 12, 2023 +

Our quizzes are rigorously reviewed, monitored and continuously updated by our expert board to maintain accuracy, relevance, and timeliness.

  • Current Version
  • Dec 12, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Aug 01, 2022
    Quiz Created by
    Catherine Halcomb
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