1.5 Uncertainty in Measurement There are two kinds of numbers in scientific work: exact numbers (those whose values are known exactly) and inexact numbers (those whose values have some uncertainty). Most of the exact numbers have defined values. For example, there are exactly 12 eggs in a dozen, exactly 1000 g in a kilogram, and exactly 2.54 cm in an inch. The number 1 in any conversion factor between units, as in 1 m 100 cm or 1 kg 2.2046 lb, is also an exact number. Exact numbers can also result from counting numbers of objects. For example, we can count the exact number of marbles in a jar or the exact number of people in a classroom. Numbers obtained by measurement are always inexact. There are always inherent limitations in the equipment used to measure quantities (equipment errors), and there are differences in how different people make the same measurement (human errors). Suppose that 10 students with 10 different balances are given the same dime to weigh. The 10 measurements will vary slightly. The balances might be calibrated slightly differently, and there might be differences in how each student reads the mass from the balance. Counting very large numbers of objects usually has some associated error as well. Consider, for example, how difficult it is to obtain accurate census information for a city or vote counts for an election. Remember: Uncertainties always exist in measured quantities. Precision and Accuracy The terms precision and accuracy are often used in discussing the uncertainties of measured values. Precision is a measure of how closely individual measurements agree with one another. Accuracy refers to how closely individual measurements agree with the correct, or "true," value. The analogy of darts stuck in a dartboard pictured in Figure 1.25 illustrates the difference between these two concepts. In the laboratory we often perform several different "trials" of the same experiment. We gain confidence in the accuracy of our measurements if we obtain nearly the same value each time. Figure 1.25 should remind us, however, that precise measurements can be inaccurate. For example, if a very sensitive balance is poorly calibrated, the masses we measure will be consistently either high or low. They will be inaccurate even if they are precise. 
Figure 1.25 The distribution of darts on a target illustrates the difference between accuracy and precision. 
Significant Figures Suppose you weigh a dime on a balance capable of measuring to the nearest 0.0001 g. You could report the mass as The notation (read "plus or minus") expresses the uncertainty of a measurement. In much scientific work we drop the notation with the understanding that an uncertainty of at least one unit exists in the last digit of the measured quantity. That is, measured quantities are generally reported in such a way that only the last digit is uncertain. Figure 1.26 shows a thermometer with its liquid column between the scale marks. We can read the certain digits from the scale and estimate the uncertain one. From the scale marks, we see that the liquid is between the and marks. We might estimate the temperature to be being somewhat uncertain of the second digit of our measurement. 
Figure 1.26 A thermometer whose markings are shown only every 5°C. The temperature is between 25°C and 30°C and is approximately 27°C. 
All digits of a measured quantity, including the uncertain one, are called significant figures. A measured mass reported as 2.2 g has two significant figures, whereas one reported as 2.2405 g has five significant figures. The greater the number of significant figures, the greater is the certainty implied for the measurement. 
SAMPLE EXERCISE 1.5 What is the difference between 4.0 g and 4.00 g? Solution Many people would say there is no difference, but a scientist would note the difference in the number of significant figures in the two measurements. The value 4.0 has two significant figures, while 4.00 has three. This implies that the first measurement has more uncertainty. A mass of 4.0 g indicates that the mass is between 3.9 and 4.1 g; the mass is 4.0 0.1 g. A measurement of 4.00 g implies that the mass is between 3.99 and 4.01 g; the mass is 4.00 0.01 g. PRACTICE EXERCISE A balance has a precision of A sample that weighs about 25 g is weighed on this balance. How many significant figures should be reported for this measurement? Answer: 5, as in the measurement 24.995 g 
In any measurement that is properly reported, all nonzero digits are significant. Zeros, however, can be used either as part of the measured value or merely to locate the decimal point. Thus, zeros may or may not be significant, depending on how they appear in the number. The following guidelines describe the different situations involving zeros:
The use of exponential notation (Appendix A) eliminates the potential ambiguity of whether the zeros at the end of a number are significant (rule 4). For example, a mass of 10,300 g can be written in exponential notation showing three, four, or five significant figures: (three significant figures) (four significant figures) (five significant figures) In these numbers all the zeros to the right of the decimal point are significant (rules 1 and 3). (All significant figures come before the exponent; the exponential term does not add to the number of significant figures.) Exact numbers can be treated as if they have an infinite number of significant figures. This rule applies to many definitions between units. Thus, when we say, "There are 12 inches in 1 foot," the number 12 is exact and we need not worry about the number of significant figures in it. 
SAMPLE EXERCISE 1.6 How many significant figures are in each of the following numbers (assume that each number is a measured quantity): (a) 4.003; (b) (c) 5000? Solution (a) Four; the zeros are significant figures. (b) Four; the exponential term does not add to the number of significant figures. (c) One, two, three, or four. In this case the ambiguity could have been avoided by using exponential notation. Thus has only one significant figure, whereas has three. PRACTICE EXERCISE How many significant figures are in each of the following measurements: (a) 3.549 g; (b) (c) 0.00134 m^{3}? Answers: (a) four; (b) two; (c) three 
Significant Figures in Calculations When carrying measured quantities through calculations, observe these points: (1) The least certain measurement used in a calculation limits the certainty of the calculated quantity. (2) The final answer for any calculation should be reported with only one uncertain digit. To keep track of significant figures in calculations, we will make frequent use of two rules. The first involves multiplication and division, and the second involves addition and subtraction. In multiplication and division the result must be reported with the same number of significant figures as the measurement with the fewest significant figures. When the result contains more than the correct number of significant figures, it must be rounded off. For example, the area of a rectangle whose measured edge lengths are 6.221 cm and 5.2 cm should be reported as 32 cm^{2} even though a calculator shows the product of 6.221 and 5.2 to have more digits: We round off to two significant figures because the least precise number—5.2 cm—has only two significant figures. In rounding off numbers, look at the leftmost digit to be dropped:
The guidelines used to determine the number of significant figures in addition and subtraction are different from those for multiplication and division. In addition and subtraction the result can have no more decimal places than the measurement with the fewest number of decimal places. In the following example the uncertain digits appear in color: 

SAMPLE EXERCISE 1.7 The width, length, and height of a small box are 15.5 cm, 27.3 cm, and 5.4 cm, respectively. Calculate the volume of the box using the correct number of significant figures in your answer. Solution The volume of a box is determined by the product of its width, length, and height. In reporting the product, we can show only as many significant figures as given in the dimension with the fewest significant figures, that for the height (two significant figures): When using a calculator, the display first shows 2285.01, which we must round off to two significant figures. Because the resulting number is 2300, it should be reported in standard exponential notation, to clearly indicate two significant figures. Notice that we round off the result at the end of the calculation. PRACTICE EXERCISE It takes 10.5 s for a sprinter to run 100.00 m. Calculate the average speed of the sprinter in meters per second, and express the result to the correct number of significant figures. Answer: 9.52 ms (3 significant figures) 
SAMPLE EXERCISE 1.8 A gas at 25 C fills a container previously determined to have a volume of cm^{3}. The container plus gas are weighed and found to have a mass of 837.6 g. The container, when emptied of all gas, has a mass of 836.2 g. What is the density of the gas at 25C? Solution To calculate the density we must know both the mass and the volume of the gas. The mass of the gas is just the difference in the masses of the full and empty container: In subtracting numbers, we determine significant figures by paying attention to decimal places. Thus the mass of the gas, 1.4 g, has only two significant figures, even though the masses from which it is obtained have four. Using the volume given in the question, cm^{3}, and the definition of density, we have In dividing numbers, we determine the number of significant figures in our result by considering the number of significant figures in each factor. There are two significant figures in our answer, corresponding to the smaller number of significant figures in the two numbers that form the ratio. PRACTICE EXERCISE To how many significant figures should the mass of the container be measured (with and without the gas) in Sample Exercise 1.8 in order for the density to be calculated to three significant figures? Answer: 5 (In order for the difference in the two masses to have three significant figures, there must be two decimal places in the masses of the filled and empty containers.) 
When a calculation involves two or more steps and you write down answers for intermediate steps, retain at least one additional digit—past the number of significant figures—for the intermediate answers. This procedure ensures that small errors from rounding at each step do not combine to affect the final result. When using a calculator, you may enter the numbers one after another, rounding only the final answer. Accumulated roundingoff errors may account for small differences between results you obtain and answers given in the text for numerical problems. 
*Your instructor may wish you to use a slight variation on the rule when the leftmost digit to be removed is exactly 5, with no following digits or only zeros. One common practice is to round up to the next higher number if that number will be even, and down to the next lower number otherwise. Thus, 4.7350 would be rounded to 4.74, and 4.7450 would also be rounded to 4.74. 