Please see attachment and provide work so it can be use as reference!
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 25°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.
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 = ...
The density of chloroform are determined. The density of chloroform using the data in the picture is given.
Solution Properties Examined
Chapter 13 Practice
7. By referring to the figure , determine the mass of each of the following salts required to form a saturated solution in 350 of water at 30 : , ,
10. Calculate the mass percentage of in a solution containing 10.8 in 481 water.
13. An ore contains 2.88 of silver per ton of ore. What is the concentration of silver in ppm?
14. A solution is made containing 14.5 of in 183 .
A. Calculate the mole fraction of .
B. Calculate the mass percent of .
C. Calculate the molality of .
18. What is the molarity of 0.560 in 250.0 of solution? 22.3 in 125 of solution?
22. A sulfuric acid solution containing 571.5 of per liter of solution has a density of 1.329 .
A. Calculate the mass percentage of in this solution.
B. Calculate the mole fraction of in this solution.
C. Calculate the molality of in this solution.
D. Calculate the molarity of in this solution.
31. The density of acetonitrile is 0.786 , and the density of methanol is 0.791 . A solution is made by dissolving 21.0 in 98.5 .
A. What is the mole fraction of methanol in the solution?
B. What is the molality of the solution? Assuming is the solute and is the solvent.
C. Assuming that the volumes are additive, what is the molarity of in the solution?
39. Calculate the number of moles of solute present in each of the following aqueous solutions
A. 700 of 0.250
B. 86.6 of 0.180 ,
C. 122.0 of a solution that is 6.25% glucose by mass.
44. Calculate the vapor pressure of water above a solution prepared by adding 23.0 of lactose to 200.0 of water at 338 . (Vapor-pressure of water at 338 187.5 .)
61. Calculate the freezing and boiling points of each of the following solutions:
A. freezing point of 0.25 glycerol in ethanol
B. boiling point of 0.25 glycerol in ethanol
C. freezing point of 0.240 of naphthalene in 2.65 of chloroform