Solution Manual For Experiments in Biochemistry: A Hands-on Approach, 2nd Edition

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i
Manual for
Experiments in
Biochemistry:
A Hands On Approach
Shawn O. Farrell
and
Lynn E. Taylor
Colorado State University

ii
Table of Contents
Preface ....................................................................................................................... iii
Technical Support...................................................................................................... iv
Background Information from Textbooks ................................................................. v
General Lab Equipment............................................................................................. vi
Experiment 1 -- Use of pipettors ............................................................................... 1
Experiment 2 -- Preparation of Buffers ..................................................................... 7
Experiment 3 -- Beer's Law and Standard Curves .................................................... 14
Experiment 3a -- Protein Concentration of LDH Fractions ...................................... 20
Experiment 4 -- Purification of LDH (short version) ................................................ 25
Experiment 4a -- Purification of LDH (comprehensive version) .............................. 33
Experiment 5 -- Separation and Identification of Amino Acids ............................... 42
Experiment 5a -- Purification of LDH with Ion Exchange Chromatography ........... 49
Experiment 6 -- Affinity Chromatography of LDH .................................................. 57
Experiment 6a – Affinity Chromatography of LDH ................................................. 61
Experiment 7 -- Gel Filtration Chromatography ....................................................... 69
Experiment 7a -- Gel Filtration Chromatography of LDH........................................ 74
Experiment 8 -- Enzyme Kinetics of Tyrosinase ...................................................... 82
Experiment 8a -- Enzyme Kinetics of LDH .............................................................. 89
Experiment 9 -- Native Gel Separation of LDH Isozymes (short version) ............... 96
Experiment 9a -- Native Gel Separation of LDH Isozymes (comprehensive) .......... 101
Experiment 9b -- SDS-Polyacrylamide Gel Electrophoresis (short)......................... 106
Experiment 9c -- SDS-Polyacrylamide Gel Electrophoresis (comprehensive)......... 112
Experiment 10 -- Western Blots of Serum Proteins .................................................. 119
Experiment 10a -- Western Blot of LDH .................................................................. 127
Experiment 11 -- Analysis of DNA Restriction Fragments ...................................... 134
Experiment 12 -- Cloning and Expression of Barracuda LDH ................................. 141
Experiment 13 -- Polymerase Chain Reaction .......................................................... 158

iii
Preface
This manual is designed to aid the laboratory instructor in preparing for, supervising, and
analyzing experiments in Experimental Biochemistry: A Hands On Approach. The text
was written with the idea of its application to a wide variety of biochemistry lab courses.
Whether your course is for non-majors and meets only once a week for 3 hours, or is a
more intensive course requiring several meetings, you should be able to find the
appropriate length and intensity of experiments. Many of the experiments are suitable for
a survey course and can stand alone. For those interested in a comprehensive approach,
there are groups of experiments that do make an integrated package. Many of the
techniques used offer both types of experiment. For example, chapter 7 involves gel
filtration chromatography. Experiment 7 is a stand alone experiment involving estimating
the molecular weight of myoglobin with Sephadex G-75. Experiment 7a is part of the
comprehensive purification of lactate dehydrogenase and uses gel filtration on Sephadex
G-150 or Sephacryl S-200 as the final purification step.
Each chapter of this manual corresponds to the same chapter in Experiments in
Biochemistry and includes the following:
 Estimated time required by competent and prepared students
 Materials needed for the experiment and sources when necessary
 Hints for the preparation of reagents and equipment, and pitfalls to avoid
 Suggestions for disposal and clean up of experiments
 Sample data the students are likely to see and answers to the end of experiment
calculations
 Answers to the additional problem sets.
We hope that armed with this manual you will find the implementation of the
experiments straight forward. If you ever have trouble, please feel free to contact the
author (see Tech Support).

iv
Technical Support
I have been teaching two levels of biochemistry lab at Colorado State University for the
past 18 years. One is a survey course for non-majors and the other is a comprehensive
course for majors. My position is pure teaching, so I have devoted much time to the
perfection of these experiments.
If you have any questions about how to implement any of these experiments, how to
prepare the reagents, where to get the reagents and equipment, how to optimize the time
you have with your course, or what might have gone wrong, please feel free to contact
me. I am available by phone or e-mail. I would also appreciate any feedback you give me
that would make the labs run smoother. Thank-you and I look forward to hearing from
you.
Dr. Shawn O. Farrell
USA Cycling
1 Olympic Plaza
Colorado Springs, CO 80909
719-866-3364
sfarrell@usacycling.org

v
Background Information from Textbooks
No biochemistry laboratory can stand alone without a supporting lecture class to give the
students the background material. We have attempted to include material in our chapters
that is specific to laboratory techniques. For background material of a broader nature, we
suggest one of the following textbooks -- Biochemistry by Mary K. Campbell and Shawn
O. Farrell or Biochemistry by R.H. Garrett and C.M. Grisham. Of course, any basic
biochemistry book would also do.
Below you will find information about the relevant chapters of the fifth edition of
Campbell and Farrell's Biochemistry and the third edition of Garrett and Grisham's
Biochemistry.
Experiments in Biochemistry Campbell (5th edition) Garrett and Grisham (3rd edition)
Chapter 2 Chapter 2 Chapter 2
Chapter 3 Chapter 5
Chapter 4 Chapters 4,5, 6 Chapters 5,6,13
Chapter 5 Chapter 3 Chapters 4,5
Chapter 6 Chapter 5 Chapter 5
Chapter 7 Chapter 5 Chapter 5
Chapter 8 Chapter 6,7 Chapters 13,14
Chapter 9 Chapter 5,13 Chapter 5
Chapter 10 Chapter 12
Chapter 11 Chapter 13 Chapter 12
Chapter 12 Chapter 13 Chapter 12
Chapter 13 Chapter 13 Chapter 12

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vi
General Lab Equipment
The following chapters contain lists of equipment required for each experiment. There
are certain items that are assumed to be available for all labs, and these will not be
mentioned specifically in the chapters. These items include the following:
Kimwipes
gloves
Pasteur pipets (long and short)
pipet tips (all sizes)
Parafilm
paper towels
soap
vortexers
weigh boats
ice buckets
microcentrifuge tubes
The quantities listed are for each experiment performed. Thus, if you have students work
alone, that would be per student. These are the quantities that I have used. Sometimes they
are overkill, but I prefer to err on the side of making too much of the cheaper chemicals so
that I don't have to make them again later.

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1
Chapter 1 -- Biochemistry Boot Camp
Experiment 1 -- Use of Pipettors
Time Required
This brief experiment should take no more than 30 minutes, usually less if there is ample
equipment.
Materials Required
P-100 or P-200 pipetmen (Rainin, Integrapette, Eppendorf)
P-1000 pipetmen
Top loading balances or others with a sensitivity of at least 0.01g
Deionized water
Hints for Preparation and Implementation
 If equipment is limiting, students can stagger which part they start first to better share
the pipetmen.
 Be sure to give a prelab lecture about how to use a pipettor. Many students, including
grad students, have never received any formal training in this. This lab, though brief,
will establish the quality of results that will be seen for the rest of the semester.
 Make sure that students identify poorly calibrated pipets.
 If a student thinks that their pipettor draws up a low volume, make sure the pipet tips
are on tight, the pipet is set to the correct volume, and that the lower barrel of the
pipettor is screwed on tight. The latter is a common problem with Eppendorf
pipettors.
Waste Disposal
None
Answers to Prelab Questions
1. What is the useable range of a P-1000 Pipetman?
100 to 1000 L

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2
2. What is the difference between accuracy and precision?
Accuracy is the relationship between the number you read and the true value. In
other words, if you try to pipet 1 mL and you actually pipet 0.99 mL, then the
pipetting was accurate. Its error was only 1%. Precision is how reproducible the
numbers are, so if you try to pipet 1 mL five times and you pipet 0.70, 0.70, 0.70,
0.70, and 0.70, then your pipetting was very precise although it was also very
inaccurate.
3. What should 100 L of water weigh?
Since water weighs 1 g/mL, the weight would be calculated thusly:
1 g/mL x 0.1 mL = 0.1 g
4. What should 1000 L of water weigh?
The answer is 1 g, since 1000 L is the same as 1 mL.
Sample Data and Analysis of Results
Part A -- Precision of P-100 or P-200 pipettors
1. Record the weight you measured for the three trials of 100 L:
Weight #1 (x1) 0.09
Weight #2 (x2) 0.09
Weight #3 (x3) 0.11
2. Average the three weights.
Average of three trials: 0.097
3. Calculate the % error between the average of the three trials and the true
value.
% error = │ 0.097 - 0.100 g│ x 100 = 3 %
0.1 g
4. Calculate the mean deviation for the three trials:
mean deviation = │ xi - xavg │ =
3
[-(0.09-0.097)+-(0.09-0.097)+(0.11-0.097)]/3 = 0.009

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3
Part B -- Precision of P-1000 pipettors
1. Record the weight you measured for the three trials of 1000 L:
Weight #1 (x1) 0.99
Weight #2 (x2) 1.05
Weight #3 (x3) 0.97
2. Average the three weights.
Average of three trials: 1.00
3. Calculate the % error between the average of the three trials and the true
value:
% error = │ avg. weight - 1.00 g│ x 100 = 0
1.00 g
4. Calculate the mean deviation for the three trials:
mean deviation = │ xi - xavg │ =
3
[-(0.99-1.00)+(1.05-1.00)+-(0.97-1.00)]/3
= 0.03
5. Record the weight you measured for the three trials of 100 L using the P-
1000:
Weight #1 (x1) 0.09
Weight #2 (x2) 0.08
Weight #3 (x3) 0.12
6. Average the three weights.
Average of three trials: 0.10
7. Calculate the % error between the average of the three trials and the true
value:
% error = │ avg. weight - 0.10 g│ x 100 = 0
0.10 g

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4
8. Calculate the mean deviation for the three trials:
mean deviation = │ xi - xavg │ =
3
[-(0.09-0.10)+-(0.08-1.00)+ (0.12-0.10)]/3
= 0.02
Part C – Pipettors in the Lab
1. Which of the two pipettors you used was the more accurate?
The % error is the measure of the accuracy of a pipetman. From the data presented,
the P-1000 would appear to be the more accurate, since it had the smallest % error.
2. Which of the two pipettors you used was the more precise?
This is the trickier question. If you just look at the mean deviations, it appears that
the P-1000 has the larger mean deviation of 0.02 when compared to the 0.009 of the
P- 100, when both were used to pipet 100 L. However, one must bear in mind that
the total weight expected is also important. For the pipetting of 1000 L, if you
calculated a % mean deviation by dividing by the expected weight and multiplying
by 100, the P-1000 would, once again, have the smaller number.
3. What are the take-home messages from this exercise?
Take your pick from any of the following:
 There are different types of pipetmen that you must learn to use.
 Pipetmen are precise in the hands of a trained user, but not necessarily accurate.
 The accuracy of a pipet should be checked frequently.
 It is easy to check the accuracy and precision by doing a water weight test.
 Pipetmen have a range outside of which they are not accurate.
 You should learn what the correct volume of solution looks like in a pipet tip.
 Others that you can think of.
4. Without checking the accuracy of a given Pipetman, would you predict that it is
better to use a P-200 or P-1000 to pipet 100 μL? Why?
It is generally better to use a liquid transfer device closer to its maximum volume, so
using the P-200 would be better.

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5
5. Is a Pipetman more like a serological pipet or a Mohr pipet? Why?
It is more like a serological pipet, as you expel the liquid completely out of it all the
way to the tip.
6. If you are trying to pipet an unknown liquid with a Pipetman and the liquid
keeps running out of the tip before you can transfer it, what are two possible
reasons for this? What can you do to remedy the situation?
One reason might be that the tip is not on tightly. In that case, just tighten the tip.
Another might be that the liquid is an organic solvent, which might have a very low
surface tension. To remedy that, draw up the liquid into the tip and then expel it.
Then draw up the solution again. It usually will hold in the tip the second time after
pre-wetting the tip.
7. How do you make 200 mL of a 0.1 M solution of a substance that has a
molecular weight of 121.1 g/mol?
You need 0.2 liters of a 0.1 mole/liter solution or 0.02 moles of the solute. If the
MW is 121.1 g/mol, you need 0.02 x 121.1 or 2.4 grams of solute. Thus, you weigh
2.4 grams of solute into a vessel and bring the volume up to 200 mL.
8. If you take 10 mL of the solution you made in Question 7, add 90 mL of water,
mix, and then take 5 mL of the mixture and bring it to 25 mL, what will be the
concentration of the final solution in molar, millimolar, and micromolar?
The first dilution is a 10 to 1, since you start with 10 mL and end with 100 mL. The
second dilution is a 5 to 1, since you took 5 mL and brought the volume to 25. Thus,
the total dilution factor is 50 to 1. Since you started with 0.l M, the final
concentration in molar is 0.1/50 or 0.002 M. this is 2 mM and 2000 μM.
Answers to Additional Problem Set
1. How many grams of solid NaOH are required to prepare 200 mL of a 0.05 M
solution?
0.4 g
2. What would be the concentration from Problem 1 expressed in % w/v?
0.2 % w/v
3. How many mL of 5M NaCl are required to prepare 1500 mL of 0.002 M
NaCl?
0.6 mL

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6
4. What would be the concentration of the diluted solution from Problem 3
expressed in mM, M, and nM?
2 mM, 2000 M, 2 x 106 nM
5. A solution contains 15 g of CaCl2 in a total volume of 190 mL. Express the
concentration in terms of g/L, % w/v, M, and mM.
79 g/L, 7.9 % w/v, 0.71 M, 710 mM
6. Given stock solutions of glucose (1M), Asparagine (100 mM) and NaH2PO4 (50
mM), how much of each solution would you need to prepare 500 mL of a
reagent which contains 0.05 M glucose, 10 mM Asparagine and 2 mM
NaH2PO4?
25 mL glucose, 50 mL Asparagine, 20 mL sodium phosphate
7. Calculate the number of millimoles in 500 mg of each of the following amino
acids: alanine (MW = 89), leucine (131), tryptophan (204), cysteine (121), and
glutamic acid (147).
5.6 mmol Ala, 3.8 mmol Leu, 2.5 mmol Trp, 4.1 mmol Cys, 3.4 mmol Glu
8. What molarity of HCl is needed so that 5 mL diluted to 300 mL will yield 0.2
M?
12 M
9. How much 0.2 M HCl can be made from 5.0 mL of 12.0 M HCl solution?
300 mL
10. What weight of glucose is required to prepare 2 L of a 5% w/v solution?
100 g
11. How many mL of an 8.56% solution can be prepared from 42.8 g of sucrose?
500 mL
12. How many mL of CHCl3 are needed to prepare a 2.5% v/v solution in 500 mL
of methanol?
12.5 mL
13. If a 250 mL solution of ethanol in water is prepared with 4 mL of absolute
ethanol, what is the concentration of ethanol in % v/v?
1.6 % v/v

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7
Chapter 2 – Acids, Bases, and Buffers
Experiment 2 – Preparation of Buffers
Time Required
1.5 to 2 hours if there is no equipment constraint.
Materials Required
pH meters, preferably digital
NaOH, 1 M 15 mL
HCl, 1 M 15 mL
NaAcetate 1 g
CAPS “
HEPES “
Na2HPO4 “
Tricine “
TRIS “
NaCitrate “
NaH2PO4 unknowns,0.1 M, pH 5.6 5 ml
NaH2PO4 unknowns,0.1 M, pH 7 “
NaH2PO4 unknowns,0.1 M, pH 8 “
Sources for key ingredients
None of the chemicals used for this experiment need to be particularly pure. Use the
cheapest source you can find. For the buffer compounds, it does not matter if you use the
acid form or the basic form, as the students will adjust the pH anyway when making up the
buffer. Sigma and VWR offer good sources of these compounds. For convenience, the
Sigma materials are listed below:
Compound Catalog # Price (2004)
Acetate (sodium salt) Sigma 24,124-5 $64.30 per Kg
CAPS Sigma C 2632 $243 per Kg
Citrate (sodium salt) Sigma C 3674 $27.60 per Kg
HEPES (sodium salt) Sigma H 7006 $216.50 per 500 g
Tricine Sigma T 0377 $86 per 250 g
TRIS (Trizma base) Sigma T 1503 $84 per Kg

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8
Hints for Preparation and Implementation
This is a fast lab that usually only slows down due to the logistics of acquiring the materials
and using the balances and pH meters.
 Make sure all available pH meters and balances are ready to go.
 Dispense the dry buffer powders so that there are several locations or several containers
students can use to avoid a big line of students waiting to get started.
 Dispense unknowns in large test tubes with about 10 mL each.
Waste Disposal
All unknowns can be dumped down the sink at the week’s end. Save the HCl and NaOH
for future labs. Discard or save dry buffers depending on quality and quantity.
Answers to Prelab Questions
1. Calculate the weight of buffer you would use to make the buffer for part A for
the six possibilities:
0.1 mol/liter x 0.1 liters = 0.01 moles. You need 0.01 moles of the buffer. Moles x
MW = grams.
Acetate 136.1 g/mol x 0.01 mol = 1.36 g
CAPS 221.3 g/mol x 0.01 mol = 2.21 g
Citrate 294.1 g/mol x 0.01 mol = 2.94 g
HEPES 238.3 g/mol x 0.01 mol = 2.38 g
Phosphate 142.0 g/mol x 0.01 mol = 1.42 g
Tricine 179.2 g/mol x 0.01 mol = 1.79 g
TRIS 121.1 g/mol x 0.01 mol = 1.21 g
2. If we give you HEPES in the basic form and ask you to make a buffer of pH
8.0, will you add HCl or NaOH to adjust the pH? Why?
Calculate what would be the initial pH of a solution of HEPES base. Using the
formula:
pH = (pKa + 14 + log[base])/2 = (7.55 + 14 + log[0.1])/2 = 10.28
We can see that the pH will be more basic than the desired 8.0. Therefore, we will
have to add acid. In general, anytime you make up a buffer in its basic form, you
will need to add acid to get to a useable buffer pH. This question could be answered
philosophically as well. A buffer always needs to be a combination of the acid and
basic form of the buffer. If we start with just the basic form of a buffer, we will
always need to create the acidic form, so we would need to add HCl.

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9
Sample Data and Analysis of Results
Data
Part A
Buffer #1: phosphate grams: 1.42 Original pH: 5.4
Buffer #2: Tricine grams: 1.79 Original pH: 10.2
Part B
Buffer #1 pH of 0.1 M 8.10 pH of 0.01 M 8.40 pH of 0.001 M 8.75
Buffer #2 pH of 0.1 M 8.10 pH of 0.01 M 7.99 pH of 0.001 M 7.95
Part C
Distilled water pH: 5-9 (depending on water source and cleanliness of beakers
Unknown # 21 pH: 7.0
Unknown # 36 pH: 5.6
Part D
Buffer chosen: Tricine pH: 8.10 pKa: 8.15
Acid or base added: NaOH
pH after adding acid or base: 8.18
pH of 50 mL of water: 7.0
pH after adding acid or base: 12.0
Calculations
1. (a)What is the ratio of A-/HA in your buffer after you adjusted its pH to the
required value?
This will depend on which buffer you used and at what pH. A good buffer was
defined as one with a pH that was at most 1 pH unit away from the pKa.

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