Lab 2.2 Water, Water, Everywhere

  • Due No Due Date
  • Points 10
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2: Type your answers for each question.  Type your work where necessary.

In this activity you will determine the density of a sample of water.  Each lab team will perform two trials.  Be sure to record units for all measurements and use proper significant figures.

 

PROCEDURE:

  1. Find the mass of an empty 50 mL graduated cylinder and record to 0.01 g.
  2. Place a sample of tap water (between 10 and 40 mL) into the graduated cylinder and record the volume to the correct number of significant figures.
  3. Find the mass of the water and graduated cylinder and record to 0.01 g.
  4. Calculate the mass of the water.
  5. Repeat for another sample of water with a different volume.
  6. Calculate the density for each sample of water, then find the average density for water. 

 

DATA TABLE:             

 

Trial #1

Trial #2

Mass of graduated cylinder + water (g)

 

 

Mass of empty graduated cylinder (g)

 

 

Mass of water (g)

 

 

Volume of water (mL)

 

 

Density of water (g/cm3)

 

 

Average density of water (g/cm3)

 

 

 

QUESTIONS:  TYPE all work including formulas, units, and significant figures.

  1. We all know that ice (density = 0.90 g/cm3) floats in water.  Suppose an ice cube was placed in a beaker of ethyl alcohol (density = 0.79 g/cm3).  Would the ice cube float or sink?  Justify your response.

 

 

 

  1. Acetone, the solvent in nail polish remover, has a density of 0.791 g/mL.  What is the volume of 25.0 g of acetone?

 

 

 

  1. “Liquid X” has a greater density than “Liquid Y”. If 10.0 grams of “Liquid X” completely fills a test tube, can an identical test tube contain 10.0 grams of “Liquid Y”?  
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