Prelab
1. How many significant figures does 0.00210 have?
2. How many significant figures does 5300 have?
3. Near the end of the semester, you may be asked to calculate the molarity of a solution made by
putting 3.4 moles NaCl into a beaker and adding water to make 1.5 L of NaCl solution. How many
significant figures should the answer be rounded to if the molarity equation is Molarity = mole / L?
4. Add the following volumes and report the final answer to the right number of significant figures: 2.46
L + 3.1 L + 4.2269 L = ?
5. If a graduated cylinder is divided into tenths, how far should you bring your measurement?
6. Density is calculated mass divided by volume. If you rearrange to solve for mass, the formula is Density
× volume. What is the mass of a substance if you have 3.0 cm3 of a metal with a density of 2.70 g/cm3?
7. A thermometer is marked off into one degree increments. If the alcohol inside the thermometer rises
halfway between 32 and 33 degrees Celsius, how would you report the temperature?
8. Using proper significant figure rules, calculate the average density of the following values: 3.893 g/mL,
3.792 g/mL, 3.54 g/mL, and 3.900 g/mL.
9. When calculating an average, three numbers were added, then divided by 3. The number 3 in this
calculation is only one significant figure, so the answer must be rounded to one significant figure. Is this
statement True or False? Why?
10. When converting between standard notation and scientific notation, you should keep the same
number of significant figures. Convert 9.52 × 103 into standard form with the correct number of
significant figures.
1. How many significant figures does 0.00210 have?
2. How many significant figures does 5300 have?
3. Near the end of the semester, you may be asked to calculate the molarity of a solution made by
putting 3.4 moles NaCl into a beaker and adding water to make 1.5 L of NaCl solution. How many
significant figures should the answer be rounded to if the molarity equation is Molarity = mole / L?
4. Add the following volumes and report the final answer to the right number of significant figures: 2.46
L + 3.1 L + 4.2269 L = ?
5. If a graduated cylinder is divided into tenths, how far should you bring your measurement?
6. Density is calculated mass divided by volume. If you rearrange to solve for mass, the formula is Density
× volume. What is the mass of a substance if you have 3.0 cm3 of a metal with a density of 2.70 g/cm3?
7. A thermometer is marked off into one degree increments. If the alcohol inside the thermometer rises
halfway between 32 and 33 degrees Celsius, how would you report the temperature?
8. Using proper significant figure rules, calculate the average density of the following values: 3.893 g/mL,
3.792 g/mL, 3.54 g/mL, and 3.900 g/mL.
9. When calculating an average, three numbers were added, then divided by 3. The number 3 in this
calculation is only one significant figure, so the answer must be rounded to one significant figure. Is this
statement True or False? Why?
10. When converting between standard notation and scientific notation, you should keep the same
number of significant figures. Convert 9.52 × 103 into standard form with the correct number of
significant figures.
