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Module 1
Biotechnology Basics
Copyright © Texas Education Agency 2009. All rights reserved.
Lessons for Module 1
1.1
1.2
1.3
1.4
1.5
1.6
1.7
Overview of Biotechnology
Cell Structure and Function
DNA Structure and Function
Protein Synthesis
Protein Structure and Function
Math Skills
Lab Overview
Copyright © Texas Education Agency 2009. All rights reserved.
Goals for Lesson 1.5
Identify significant figures
Calculate in scientific notation
Convert numbers in the metric system
Describe units of concentration
Perform calculations necessary for preparing
stock solutions
Calculate parallel dilution formulas
Copyright © Texas Education Agency 2009. All rights reserved.
Significant Figures
All the numbers for which actual
measurements are made plus one
estimated number
1
2
You would estimate this measurement as 1.5
1
2
You would estimate this measurement as 1.48
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Significant Figures
Tells the person interpreting your data about
the accuracy of the measuring instrument used
to obtain the data
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Significant Figures
Rules for counting sig figs
1. Digits other than zero are always significant.
a. 96 = 2 sig figs
b. 61.4 = 3 sig figs
2. Zeroes between 2 other sig figs are always
significant.
a. 5.029 = 4 sig figs
b. 306 = 3 sig figs
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Significant Figures
Rules for counting sig figs
3. Leading zeroes are never significant when they are
to the left of non-zero numbers.
a. 0.0025 = 2 sig figs
b. 0.0821 = 3 sig figs
4. Trailing zeroes are only significant if there is a
decimal present and they are to the right of nonzero
numbers.
a. 100 = 1 sig fig
b. 100.0 = 4 sig figs
c. 0.0820 = 3 sig figs
Copyright © Texas Education Agency 2009. All rights reserved.
Sig Fig Practice
Significant Figures
Rules for calculating with sig figs
1.
In addition and subtraction, the answer should be rounded off
so that it has the same number of decimal places as the
quantity having the least number of decimal places.
a. 1.1 + 225 = 226.1 = 226 (rounded to no decimal places)
b. 2.65 – 1.4 = 1.25 = 1.3 (rounded to 1 decimal place)
2.
In multiplication and division, the answer should have the
same number of significant figures as the given data value
with the least number of significant figures.
a. 4.60  45 = 207 = 210 (rounded to 2 sig figs)
b. 1.956  3.3 = 0.5927 = 0.59 (rounded to 2 sig figs)
Copyright © Texas Education Agency 2009. All rights reserved.
Scientific Notation
A way to write very large and very small
numbers
A number in scientific notation is written in two
parts, the coefficient and an exponent of 10
coefficient
5 x 1022
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exponent of 10
Scientific Notation
Changing standard numbers to scientific notation
1.
Numbers greater than 10
a. Move decimal until only ONE number is to the
left of the decimal.
b. The exponent is the number of places the
decimal has moved and it is POSITIVE.
Ex. 125 = 1.25  102
15,000,000,000 = 1.5  1010
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Scientific Notation
Changing standard numbers to scientific notation
2.
Numbers less than 1
a. Move decimal until only one number is to the
left of the decimal.
b. The exponent is the number of places the
decimal has moved and it is NEGATIVE.
Ex. 0.000189 = 1.89  10-4
0.5476 = 5.476  10-1
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Scientific Notation
Changing standard numbers to scientific notation
3.
To change a number written in incorrect scientific
notation:
a. Move the decimal until only one number is to
the left of the decimal.
b. Correct the exponent. (remember: take away,
add back)
coefficient decreased by 2, so
Ex. 504.2  106 = 5.042  108 The
the exponent must increase by 2
0.0089  10-2 = 8.9  10-5
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The coefficient increased by 3, so
the exponent must decrease by 3
Scientific Notation
Changing numbers in scientific notation to
standard notation
1.
2.
If the exponent is (+) move the decimal to the right
the same number of places as the exponent.
a. 1.65  101 = 16.5
b. 1.65  103 = 1650
If the exponent is (-) move the decimal to the left the
same number of places as the exponent.
a. 4.6  10-2 = 0.046
b. 1.23  10-3 = 0.00123
Scientific Notation Drill
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Scientific Notation
Multiplication and division in scientific notation
1.
To multiply numbers in scientific notation
a. Multiply the coefficients.
b. Add the exponents.
c. Convert the answer to correct scientific
notation.
Ex: (2  109) x (4  103) = 8 x 1012
Copyright © Texas Education Agency 2009. All rights reserved.
Scientific Notation
Multiplication and division in scientific notation
2.
To divide numbers in scientific notation
a. Divide the coefficients.
b. Subtract the exponents.
c. Convert the answer to correct scientific
notation.
Ex: (8.4  106)  (2.1  102) = 4 x 104
Multiplying and Dividing in Scientific Notation
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Scientific Notation
Addition and Subtraction in Scientific Notation
1. Before numbers can be added or subtracted, the
exponents must be equal.
Ex. (5.4  103) + (6.0  102)
= (5.4  103) + (0.6  103)
= 6.0  103
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Metric System
Unit
Unit
Unit
Unit
Unit
of
of
of
of
of
length…..meter (m)
mass ……gram (g)
volume …liter (L)
time …….second (s)
temperature…degrees Celsius (°C)
Copyright © Texas Education Agency 2009. All rights reserved.
Metric System
The metric system is based on units of 10.
Prefix symbol
Prefix name
Prefix value
Fraction or Multiple
Power
G
giga
one billion
1,000,000,000
109
M
mega
one million
1,000,000
106
k
kilo
one thousand
1000
103
1
10
BASIC UNIT: m, g, L,
d
deci
1/10
0.1
10-1
c
centi
1/100
0.01
10-2
m
milli
1/1000
0.001
10-3
µ
micro
1/1,000,000
0.000 001
10-6
n
nano
1/1,000,000,000
0.000 000 001
10-9
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Metric System
 Converting measurements within the metric system is a
simple matter of multiplying or dividing by 10, 100,
1000, etc.
 Even simpler, it is a matter of moving the decimal point
to the left or right.
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Metric System
 One way to know where to place the decimal is to draw a "metric
line" with the basic unit in the center, marking off six units to the
left and six units to the right.
 To convert from one unit to another simply count the number of
places to the left or right, and move the decimal in that direction
that many places.
Ex. 3 L = 0.003 kL
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Ex. 3 mg = 3000 µg
Units of Concentration
A solution is a homogeneous
mixture of one substance (the
solute) dissolved in another
substance (the solvent).
Concentration is a ratio of the
amount of solute to the amount
of solvent.
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Units of Concentration
Molarity (M) is the most common unit of
concentration
Molarity is an expression of moles/Liter of
the solute.
Copyright © Texas Education Agency 2009. All rights reserved.
Units of Concentration
A mole is the SI unit of number of particles and
can be used as an expression of the molecular
weight of a substance.
The formula weight of an
element is expressed as
grams/mole
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Units of Concentration
The molar mass of a compound can be
calculated by adding the molar mass of the
individual elements.
22.99 + 35.45 = 58.44 g/mol
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Making Solutions
You just calculated the molar mass of sodium
chloride to be 58.44 g/mol.
To determine how to make a stock solution of
sodium chloride, use the formula:
g = M x L x molar mass
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Making Solutions
 How many grams of NaCl would you need to prepare
500 mL of a 1 M solution?
g = M x L x molar mass
g = (1mol/L) (0.5L) (58.44g/mol)
g = 29.22 g
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Making a Solution
Diluting Solutions
Once you have made a stock solution, you
often will need to dilute it to a working
concentration.
To determine how to dilute the stock
solution, use the formula:
C1V1 = C2V2
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C1
C2
V1
V2
– concentration of stock
- concentration of diluted solution
– volume needed of stock
– final volume of dilution
Diluting Solutions
How many milliliters of a 1 M stock
solution of NaCl are needed to prepare
100 ml of a 0.05 M solution?
C1 V1 = C2 V2
(1)V1 = (0.05)(100)
V1= 5 ml
Dilutions Tutorial
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Resources
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