Measurement Uncertainty
In Chemistry, students often deal with experimental data and theoretical calculations. Most of the data is present in an extremely large number of quantum. This uncertainty in measurement is the range of possible values within which the true/real value of the measurement exists. There are practical ways to handle these figures with convenience and present the given data as realistically as possible.
Scientific Notation
As discussed above, atoms and molecules have very low masses and are present in exceedingly large numbers. We are here dealing with numbers as large as 602,200,000,000,000,000,000,000 for the molecules of just 2 g of H_{2} hydrogen gas and as small as 0.00000000000000000000000166 g which is the mass of a hydrogen atom. On a similar scale exist the values of constants such as the speed of light, Planck’s constant, electric charge of particles, etc.
Thus, when handling numbers involving such scales of zeroes, it becomes extremely difficult for simple calculations of addition, subtraction, multiplication, and division. To solve these issues, scientists have developed a scientific notation for such numbers.
Scientific Notation here is the exponential notation in which one can represent a given number in the form of N Ă— 10^{n}, where N is a digit term that ranges between 1.000… and 9.999…, and n is an exponent of positive or negative values. Accordingly, one can write 2702.0109 as 2.7020109 Ă— 10^{3} in scientific notation. It can be observed that once shifted the decimal point three places to the left and thus added the exponent (3) of 10 to the scientific notation. Similarly, write 0.00001008565 as 1.008565 Ă— 10^{5}. Here, the decimal point is moved to the right by five places as the (5) exponent of 10 is in the scientific notation.
Multiplication and Division
Both Multiplication and Division follow the same rules that exist for exponential numbers. Let’s take a look at some examples to understand how multiplication and division is done,
Example 1: (4.2342 Ă— 10^{19}) Ă— (7.32 Ă— 10^{5})
Solution:
(4.2342 Ă— 10^{19}) Ă— (7.32 Ă— 10^{5})
= (4.2342 Ă— 7.32) Ă— 10^{(19+5)}
= 30.994344 Ă— 10^{24}
= 3.099 Ă— 10^{25}
Example 2: (6.23 Ă— 10^{6}) Ă· (8.33 Ă— 10^{2})
Solution:
(6.23 Ă— 10^{6}) Ă· (8.33 Ă— 10^{2})
= (6.23 Ă· 8.33) Ă— 10^{6(2)}
= (0.74789) Ă— 10^{8}
= 7.4789 Ă— 10^{7}
Addition and Subtraction
For Addition and Subtraction, first, ensure if the numbers are present in the same exponent. After that, the digit terms (coefficients) can be added or subtracted as required.
Example 1: (5.12 Ă— 10^{3}) + (6.84 Ă— 10^{5})
Solution:
(5.12 Ă— 10^{3}) + (6.84 Ă— 10^{5})
= (5.12 Ă— 10^{3}) + (684 Ă— 10^{3})
= (5.12 + 684) Ă— 10^{3}
= 689.12 Ă— 10^{3}
= 6.8912 Ă— 10^{5}
Example 2: (2.57 Ă— 10^{5}) – (9.46 Ă— 10^{3})
Solution:
(2.57 Ă— 10^{5}) – (9.46 Ă— 10^{3})
= (2.57 Ă— 10^{5}) – (0.0946 Ă— 10^{5})
= (2.57 + 0.0946) Ă— 10^{5}
= 2.4757 Ă— 10^{5}
Significant Figures
All experimental measurements have some uncertainty present due to the drawbacks of the measuring instrument and lack of accuracy in observation. For example, when observed the mass of an object to be 15 grams on a platform balance. However, the same object may weigh 15.239 grams on an analytical scale. Thus one can always not correctly tell the exact measurement. This uncertainty in the given experimental or calculated values is shown by the number of significant figures.
Significant Figures are the digits that are known with certainty plus one which is estimated or uncertain. The uncertainty is thus shown by writing certain digits and the last uncertain digit. For example, if the temperature of the room is 35.2 Â°C, consider 35 as certain and 2 as uncertain. The uncertainty in this last digit is +1. If it is not stated, consider +1 in the last digit directly.
Rules for deciding the number of significant figures in a given measurement.
 All Nonzero digits are to be considered significant. For example, 123 has three significant figures, while 0.123 also has three significant figures.
 Zeroes preceding the first nonzero aren’t significant. These zeroes indicate the position of the given decimal point. Thus, 0.02 has one significant figure and 0.000027 also has just two significant figures.
 Zeroes between any two nonzero digits are significant. Thus 9.003 has four significant figures.
 Zeroes at the end or on the right of a number (if they are on the right of the decimal point) are significant. For example, 0.500 ml has three significant figures. However, terminal zeroes are not significant if there isn’t a decimal point. For example, 9000 has only one significant figure, but 9000. has four significant figures, and 9000.0 has five significant figures. These numbers are better off represented in scientific notation. We would rather express 9000 as 9 Ă— 10^{3} for one significant figure or 9.00 Ă— 10^{3} for three significant figures.
 Exact numbers can be represented in infinite significant figures. Like 50 can be written as 50.0000000 or 734 can be written as 743.000000000 and so on. In scientific notation, all digits are significant. For example, 3.545 Ă— 10^{2} has four significant figures while 9.43 Ă— 10^{6} has three significant figures.
Accuracy and Precision
Precision stands for the closeness of different measurements for the same quantity. Accuracy is the consensus of a particular value to the true value of the measurement.
For example, suppose three students Alex, Bob, and Carol are measuring the length of the physics textbook. The true length that is known of the book is 29.5 cm. Alex measures and reports two values 28.0 cm and 28.2 cm. Both these values are precise as they are close to each other but not accurate. Bob measures and reports two values 28.5 cm and 30.5 cm. The average of these values is the true value but this observation though accurate is not precise. Carol repeats this experiment and measures 29.4 cm and 29.6 cm. Both these values are precise and accurate as they are close to each other and the average is the true value.
True Value = 29.5 cm 


1st Observation 
2nd Observation 
Average of both 
Precise 
Accurate 

Alex 
28.0 cm 
28.2 cm 
28.1 cm 
Yes 
No 
Bob 
28.5 cm 
30.5 cm 
29.5 cm 
No 
Yes 
Carol 
29.4 cm 
29.6 cm 
29.5 cm 
Yes 
Yes 
Sample Problems
Question 1: What is Dimensional Analysis? Give an example.
Answer:
When dealing with calculations, we often need to convert units from one system to another. The method to do so is called factor label method or unit factor method or dimensional analysis.
For example, to find the length of a pen of 5 inches in cm.
By convention, 1 inch = 2.54 cm.
From this equivalence, write 1 inch / 2.54 cm = 1 = 2.54 cm / 1 inch. This means that both these are unit factors and are here considered equal to 1. Thus, now multiply 5 inches to this to calculate the measurement in cm.
Therefore, 5 Ă— (2.54 cm / 1 inch) = 12.7 cm.
Thus, the length of the pen in cm is 12.7 cm.
Question 2: What is Scientific notation? Write 7654630000210000 in scientific notation.
Answer:
Scientific Notation is the exponential notation in which we can represent a given number in the form of N x 10^n, where N is a digit term that ranges between 1.000… and 9.999…, and n is an exponent of positive or negative values.
For example, we can write 7630210000 as 7.653021 Ă— 10^{9} in scientific notation.
Question 3: What is the difference between Precision and Accuracy?
Answer:
Precision stands for the closeness of different measurements for the same quantity. Accuracy is the consensus of a particular value to the true value of the measurement. Thus, precision means how close the measurements are and accuracy stands for how correct the values are.
Question 4: The exact weight of an object is 2.50 kg. A student named David measured 2.46 kg, 2.49 kg, and 2.52 kg respectively. Comment.
Answer:
David’s measurements are 2.46 kg, 2.49 kg and 2.52 kg. The average of these values is 2.49 kg. Considering the true value being 2.50 kg, we can comment that the measurements are accurate, but not precise as 2.46 kg and 2.52 kg are not close values.
Question 5: Multiply 4.3545 Ă— 1.9. Calculate the answer in terms of significant figures.
Answer:
4.3545 Ă— 1.9 = 8.27355.
However, when considered in terms of significant figures, in these operations, the result must be reported with no more significant figures as in the measurement with the few significant figures.
Thus, one can have maximum only two significant figures as 1.9 has only two significant figures.
Therefore, 4.3545 Ă— 1.9 = 8.2, where 8.2 has only 2 significant figures.
Question 6: Calculate the number of seconds in 3 days.
Answer:
By convention, 1 day = 24 hours.
From this equivalence, write 1 day / 24 hours = 1 = 24 hours / 1 day. This means that both these are unit factors and are here considered equal to 1.
Similarly, find the equivalence from hours to seconds.
Therefore,
3 days = (3 days Ă— (24 hours / 1 day) Ă— (60 min / 1 hour) Ă— (60 s / 1 min)) seconds
3 days = (3 Ă— 24 Ă— 60 Ă— 60) seconds
3 days = 259200 seconds
3 days = 2.592 Ă— 10^{5 }seconds.
Thus, 3 days have 2.592 Ă— 10^{5} seconds.
Question 7: Are zeroes considered significant numbers?
Answer:
Zeroes preceding the first nonzero aren’t significant. These zeroes indicate the position of the given decimal point. Thus, 0.02 has one significant figure and 0.000027 also has just two significant figures. Zeroes between any two nonzero digits are significant. Thus 9.003 has four significant figures. Zeroes at the end or on the right of a number (if they are on the right of the decimal point) are significant.
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