A chemist measures the volume of a solution as 25.34 mL using a burette with a precision of ±0.02 mL. They then dilute this solution to a final volume of 250.0 mL using a volumetric flask with a precision of ±0.1 mL. What is the absolute uncertainty in the final concentration of the diluted solution?

What is the area of a disc of radius 1.1 cm?

The value of Avogadro's number is $6.02214076 imes 10^{23}$ $mol^{-1}$. A student experimentally determines Avogadro's number to be $6.022141 imes 10^{23}$ $mol^{-1}$. When reporting this value with the correct number of significant figures reflecting the precision of the experimental result, the student should report:

Taking into account significant figures, what is the value of $9.99 + 0.0099$?

If $L = 2.331\;cm,\;B = 2.1\;cm,$ then L+B=

A student calculates the volume of a sphere to be $4.1887902047863905 imes 10^3 cm^3$. If the radius measurement used in the calculation has only two significant figures, what is the correctly rounded volume?

The speed of light is approximately $299,792,458 \; m/s$. Express this value rounded to three significant figures.

A student performs a titration and calculates the concentration of a solution to be $0.1234567$ M. The burette used has a precision of $\pm 0.02$ mL, and the volumetric flask used to prepare the solution has a precision of $\pm 0.1$ mL. Which is the most accurate way to report the concentration, considering significant figures and uncertainty?

The mass of an electron is approximately $9.1093837 imes 10^{-31}$ kg. If this value is multiplied by the speed of light squared ($c^2 = (2.99792458 imes 10^8 m/s)^2$), what is the correct representation of the resulting energy in joules, considering significant figures?

The length, breadth and thickness of a block are given by $l = 12cm,\;b = 6\;cm\;$ and $\;t = 2.45cm$ The volume of block according to the idea of significant figures should be

If $x = 4.99$ and $y = 0.0099$, what is $x + y$ to the correct number of significant figures?