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Buffer, Buffer Work and Henderson Hasselbalch Equation - Practice Exam 3 | Chem 106, Exams of Chemistry

Material Type: Exam; Professor: O'Neal; Subject: Chemistry & Biochemistry; University: University of Mississippi Main Campus; Term: Spring 2009;

Typology: Exams

Pre 2010

Uploaded on 12/19/2009

lbruster
lbruster 🇺🇸

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PracticeExam3
1) Whatisabuffer?
2) Howdobufferswork?
3) Whatmakesagoodbufferintermsoftheselectionofsaltandacidandtheirratios?
4) WhatistheHendersonHasselbalchEquation?
5) WhatisthepHofabufferthatis0.200MHC
2
H
3
O
2
and0.300MNaC
2
H
3
O
2
iftheK
a
ofHC
2
H
3
O
2
is
1.8x10
5
.
6) WhatisthepHofabuffercomposedof0.200MHC
2
H
3
O
2
and0.250MNaC
2
H
3
O
2
in1.00Lthathas
0.020molNaOHaddedtoit?Assumethetotalvolumedoesn’tchange.
7) Whatarethebufferingcapacityandbufferingrangeofabuffer?
8) Whatwoulddestroyabufferintermsofitseffectiveness?
9) Whichoftheweakacidsfromyourtextwouldbethebestchoicetocombinewithitssodiumsaltto
makeabufferwithpH4.80?
10) WhatratioofNaCHO
2
:HCHO
2
wouldberequiredtomakeabufferwithpH4.00?Thepk
a
forFormic
Acidis3.74.
11) Istheequivalencepointlessthan7,7,orgreaterthan7for:
a. Titrationofastrongacidwithastrongbase?
b. Titrationofaweakacidwithastrongbase?
c. Titrationofaweakbasewithastrongacid?
12) WhatisthepHofasolutioncomposedof100mLof0.2MHClthathasbeentitratedwith25mLof
0.3MNaOH?
13) WhatisthepHof150mLof0.100MHCHO
2
beforeithasbeentitrated?Thepk
a
forFormicAcidis
3.74.
14) WhatisthepHof150mLof0.100MHCHO
2
thathasbeentitratedwith50mL0.200MNaOH?
15) WhatisthepHof150mLof0.100MHCHO
2
thathasbeentitratedwith75mL0.200MNaOH?
16) WhatisthepHof150mLof0.100MHCHO
2
thathasbeentitratedwith100mL0.200MNaOH?
17) Howdoindicatorswork?
18) WhatisexpressionforthesolubilityproductconstantforPbCl
2
?
19) CalculatethemolarsolubilityofCa(OH)
2
inpurewaterat25°C.K
sp
=4.68x10
6
.
20) DeterminetheK
sp
ofPbSO
4
ifitsmolarsolubilityinwaterat25°Cis1.35x10
4
M.
21) Howdoyouknowifaprecipitateformswhenyoupourtwosolutionstogether?
22) Whatarecomplexions?
23) Whichofthefollowingcompoundsfromthek
sp
tablefromyourtextwillhavethehighestandwhich
wouldhavethelowestmolarsolubilityinpurewater?
24) WhatistheFirstLawofThermodynamics?
25) Whatdeterminesthespontaneityofareactionorprocess?
26) Whatisareversibleprocess?
27) Whatisenthalpy?
28) Whatisentropy?
29) WhatdoesS=klnWmean?
30) WhatisW?
31) Whatisthedifferencebetweenamicrostateandamacrostate?
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Practice Exam 3

  1. What is a buffer?
  2. How do buffers work?
  3. What makes a good buffer in terms of the selection of salt and acid and their ratios?
  4. What is the Henderson‐Hasselbalch Equation?
  5. What is the pH of a buffer that is 0.200 M HC 2 H 3 O 2 and 0.300 M NaC 2 H 3 O 2 if the K a of HC 2 H 3 O 2 is 1.8 x 10 ‐^5.
  6. What is the pH of a buffer composed of 0.200 M HC 2 H 3 O 2 and 0.250 M NaC 2 H 3 O 2 in 1.00 L that has 0.020 mol NaOH added to it? Assume the total volume doesn’t change.
  7. What are the buffering capacity and buffering range of a buffer?
  8. What would destroy a buffer in terms of its effectiveness?
  9. Which of the weak acids from your text would be the best choice to combine with its sodium salt to make a buffer with pH 4.80?
  10. What ratio of NaCHO 2 : HCHO 2 would be required to make a buffer with pH 4.00? The pk (^) a for Formic Acid is 3.74.
  11. Is the equivalence point less than 7, 7, or greater than 7 for: a. Titration of a strong acid with a strong base? b. Titration of a weak acid with a strong base? c. Titration of a weak base with a strong acid?
  12. What is the pH of a solution composed of 100 mL of 0.2 M HCl that has been titrated with 25 mL of 0.3 M NaOH?
  13. What is the pH of 150 mL of 0.100 M HCHO 2 before it has been titrated? The pk (^) a for Formic Acid is 3.74.
  14. What is the pH of 150 mL of 0.100 M HCHO 2 that has been titrated with 50 mL 0.200 M NaOH?
  15. What is the pH of 150 mL of 0.100 M HCHO 2 that has been titrated with 75 mL 0.200 M NaOH?
  16. What is the pH of 150 mL of 0.100 M HCHO 2 that has been titrated with 100 mL 0.200 M NaOH?
  17. How do indicators work?
  18. What is expression for the solubility product constant for PbCl 2?
  19. Calculate the molar solubility of Ca(OH) 2 in pure water at 25 °C. K (^) sp = 4.68 x 10 ‐ 6 .
  20. Determine the K sp of PbSO 4 if its molar solubility in water at 25 °C is 1.35 x 10 ‐^4 M.
  21. How do you know if a precipitate forms when you pour two solutions together?
  22. What are complex ions?
  23. Which of the following compounds from the k (^) sp table from your text will have the highest and which would have the lowest molar solubility in pure water?
  24. What is the First Law of Thermodynamics?
  25. What determines the spontaneity of a reaction or process?
  26. What is a reversible process?
  27. What is enthalpy?
  28. What is entropy?
  29. What does S = k ln W mean?
  30. What is W?
  31. What is the difference between a microstate and a macrostate?
  1. What are some changes that increase entropy?
  2. Does the entropy increase or decrease for the following processes? a. CH 4 (g) + H 2 O (g) → CO(g) + 3 H 2 (g) b. Na 2 CO 3 (s) + H 2 O(g) + CO 2 (g) → 2 NaHCO 3 (s) c. N 2 (g) + 3 H 2 (g) → 2 NH 3 (g) d. CH 3 OH(l) → CH 3 OH(s)
  3. What is the 2 nd Law of Thermodynamics?
  4. What is ∆ S surroundings is terms of ∆H (^) system?
  5. What is Gibbs Free Energy and what is its equation?
  6. What does ∆G have to be for a process to be spontaneous?
  7. How do you calculate the minimum temperature a process will be spontaneous?
  8. What is the 3 rd^ Law of Thermodynamics?
  9. How does the magnitude of entropy change with: a. Molecular complexity? b. Molar or atomic mass? c. Dissolution? d. Change of state – gas, liquid, solid?
  10. How do you calculate ∆S o , ∆H o , and ∆G o for a reaction?
  11. What is ∆G under nonstandard conditions?
  12. How is ∆G o related to the equilibrium constant?
  13. Calculate the equilibrium constant for a reaction at 298 K that has ∆G o^ = 50,001 J?