Lab Exercise 1: Length, Temperature, And Mass

Laboratory Techniques and Measurements – Lab Report Assistant
Exercise 1: Length, Temperature, and Mass
Data Table 1. Length Measurements
Object Length (cm) Length (mm) Length (m)
CD or DVD 12 120 .12
Key 3.9 39 .039
Spoon 157. 157 .157
Fork 18 180 .18

Data Table 2. Temperature Measurements
Water Temperature (°C) Temperature (°F) Temperature (K)
Hot from tap 50 122 323.15
Boiling 100 212 373.15
Boiling for 5 minutes 123 253 396.15
Cold from tap 20 66 293.15
Ice water – 1 minute 12 46 283.15
Ice water – 5 minutes 4 39 278.15

Data Table 3. Mass Measurements
Object Estimated Mass (g) Actual Mass (g) Actual mass (kg)
Pen or pencil 4 4.7 .0045
3 Pennies 3 7.5 .0075
1 Quarter 5 6.3 (1964 silver) .0063
2 Quarters, 3 Dimes 13 19.2 .0192…show more content…
Archimedes’ method
Object Mass (g) Mass of Displaced Water (g) Volume of Displaced Water (mL) Density (g/mL)
Metal Bolt 42.5 25 25 25
Magnet 16.2 3.5 3.5 3.5

Questions:
An unknown, rectangular substance measures 3.6 cm high, 4.21 cm long, and 1.17 cm wide. If the mass is 21.3 g, what is this substance’s density (in grams per milliliter)? 1.2 g/ml
A sample of gold (Au) has a mass of 26.15 g. Given that the theoretical density is 19.30 g/mL, what is the volume of the gold sample? 1.35 mL
What would happen if you dropped the object into the beaker while using the Archimedes’ Principle method instead of submerging the object? The measurements would be the same. compare to the density measurement using the calculated volume? Which method might be more accurate? Why? I think Archimedes’ Principle if done properly can be done more accurately because liquid displaces evenly.
You are given a small piece of gold colored material and want to determine if it is actually gold. Using the Archimedes Principle you find that the volume is 0.40 cm3 and the mass is 6.0 g. What conclusions can you reach from your simple density analysis? It isn't gold because gold has a higher density. Exercise 3: Concentration, Solution, and…show more content…
Initial Concentration
Chemical Mass of Graduated Cylinder (g) Mass of Sugar (g) Molar Mass (g) Moles in Graduated Cylinder Total Volume (L) Molarity (mol/L)
Sugar
(C12H22O11) 16.6 10 342.29 .29 .1 .29

Data Table 9. Dilution Series
Dilution Volume (mL) Mass (g) Density (g/mL) Initial Concentration (M) Volume Transferred (mL) Final Concentration (M)
0 25.0 mL 25 25 0 mL 0ml
1 25.0 mL 10 10 .29 2.5 mL 5.4M
2 25.0 mL 15 40 .435 4.5 mL 6.8M
3 25.0 mL 20 45 .58 3.0 mL 9.4M
4 25.0 mL 25 50 7.25 6.0 mL 11.2M Data Table 10. Molarity vs. Density
Molarity vs. Density molarity is the concentration of a solution given in gram moles of solute per liter of solution.

Density is the degree of compactness of a substance.

Questions:
How would you prepare 10 mL of a 0.25M HCl solution if 1M HCl was available? How much 1M HCl is needed? How much distilled water is used? Dilute 2.5ml of 1M solution with 7.5ml of dihydrogen monoxide.
From the graph of Molarity vs. Density, created in Data Table 10, what was the relationship between the molarity of the sugar solution and the density of the sugar solution? Density and molarity are not dependant on each