# Density of Chloroform

Please see attachment and provide work so it can be use as reference!

Density

1- Calculate the density of chloroform using the data in the picture below.

2- A glass sample bottle weighs 24.225 g when empty. When filled with carbon tetrachloride, CCl4, it weighs 28.715. If the density of carbon tetrachloride is 1.5842 g/mL, what is the volume of the sample bottle in milliliters?

3- An empty vial weighs 61.29 g.

(a) If the vial weighs 180.77 g when filled with liquid mercury (d = 13.53 g/cm3), what is its volume?

(b) How much would the vial weigh if it were filled with water (d = 0.997 g/cm3 at 25Â°C)?

When determining sigfigs, assume the same balance is being used for both parts.

4- What is the density (g/ml) of a 100 ml sample of water that has 25 grams of NaCl added to it. (assume no volume change). Round your answer to two decimal places, do not include units in your answer.

5- A block of metal weighs 27.0 g and has a volume of 10.0ml. Calculate the density, and then using the table in the lab, what is the metal most likely to be? Spelling counts. If there are multiple spellings, we will be using the spelling and naming conventions found in your text. Do not include the density in your answer, only the name of the metal.

https://brainmass.com/chemistry/stoichiometry/density-chloroform-525500

## SOLUTION This solution is **FREE** courtesy of BrainMass!

Firstly, let's lay out the mathematical expression of density, defined as the amount of mass per unit volume:

d = m / V

(typically in kg/L or g/mL)

1) The picture tells us 3 things:

Mass of cylinder + liquid = 145.10g

Mass of cylinder = 85.16g

Volume of liquid = 40.5mL

From this we can get that the mass of the liquid is 145.10 - 85.16 = 59.94g

We know the volume is 40.5mL, so density is:

d = 59.94g / 40.5mL = 1.48g/mL

2) Empty glass = 24.225g

Glass + CCl4 = 28.715g

d = 1.5842g/mL

V = ?

We simply need to rearrange the density equation:

d = m / V, V = m / d = (28.715 - 24.225) / 1.5842 = 2.8342mL

3) Empty vial = 61.29g

Vial + Hg = 180.77g

d(Hg) = 13.53g/cm^3

(cm^3 describes a volume since it describes a 1cm x 1cm x 1cm cube of space. It just so happens that 1cm^3 = 1mL)

V = ?

V = m /d = (180.77 - 61.29) / 13.53 = 8.831mL

How much would the vial weigh if water of d = 0.997g/cm^3 fills the vial?

This is a trickier question. Firstly, we have to remember that what we calculated above for the volume of mercury is really the total volume the vial can hold, and is now the volume of water. From this information, plus the density of water, we can calculate the mass of water. Then we can add this to the known weight of the empty vial and have the total mass:

Mass of water = density x volume = 0.997 x 8.831 = 8.804g

Total mass = 61.29 + 8.804 = 70.09g

4)

V = 100mL water

25g NaCl added (but no volume change)

Density = ?

Adding salt to a volume of water (without changing the volume) works to change the density of the fluid via changing the mass of the solution of water plus salt. The dnesity of this new fluid will be:

Density = Total mass of solution / Total volume of solution

Density = Mass of water + mass of NaCl / 100mL

We can get the mass of water by remembering that the density of water is 1g/mL. Since we had 100mL of water to begin with, we must also have had 100g of water. Therefore:

Density = 100 + 25 / 100mL = 1.25g/mL

5)

Mass of block - 27.0g

Volume = 10.0mL

Density = mass / volume = 27/10 = 2.7g/mL

I don't really have the table your question refers to. However a quick search on Google makes me suspect that the metal is likely Aluminium.

(Which is spelled at least two different ways!)

Hope that helps!

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