Significant Figures With Rules in Chemistry
What are Significant Figures? The reliable digits in a number that are known with the certainty are called significant figures. The last digit of measured number is generally considered uncertain by ± 1. For Example : 0.0112g contains three S.F and uncertainty is ± 0.0001 mg. 11/2mg contains three S.F and uncetainty is ± 0.1mg. The uncertainty and the number of S.F do not change when measurement is expressed in sub units. For Example: 0.0112g = 11.2mg in 0.0112g uncertainty is ± 0.0001g and in 11.2 mg uncertainty is ± 0.1mg as 0.0001g = 0.1mg. Therefore uncertainty and number of S.F do not change. Number Of Significant Figures (Digits) Depends Upon : The accurancy of the measuring instrument. The size of the object to be measured. In any series of measurements, the measured numbers are obtained to a certain degree of precision. The precision of measured is indicated by the number of significant figures. Precision : How close a series of measureme