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01.07 laboratory techniques

08/01/2021 Client: saad24vbs Deadline: 2 Day

Copyright 2019 - Hands-On Labs | http://holscience.com 1 / 14


Student Name


Mohammed Alnaimi


Student ID 48408 Lesson Laboratory Techniques and Measurements Institution Ocean County College Session 2019L2 CHEM 181 DL1 Course CHEM 181 DL1 Instructor Lea Stage


Final Report


Exercise 1


CHEM 181 DL1 Laboratory Techniques and Measurements


The reason could be atmospheric pressure changes with the higher sea levels, decreasing the degree at which it takes water to boil.


1. Water boils at 100°C at sea level. If the water in this experiment did not boil at 100°C, what could be the reason?


100(102-100)/100=2% error


100(99.2-100)/100=-0.8% error


2. While heating two dif f erent samples of water at sea level, one boils at 102°C and one boils at 99.2°C. Calculate the percent error f or each sample f rom the theoretical 100.0°C.


Copyright 2019 - Hands-On Labs | http://holscience.com 2 / 14


Data Table 1: Length Measurements


Data Table 2: Temperature Measurements


Length (cm)


CD or DVD


Key


Spoon


Fork


Length (mm)


CD or DVD


Key


Spoon


Fork


Length (m)


CD or DVD


Key


Spoon


Fork


12


5.5


18


18


120


55


180


180


0.12


0.055


0.18


0.18


Temperature (°C)


Hot from Tap


Boiling


35


Copyright 2019 - Hands-On Labs | http://holscience.com 3 / 14


Boiling for 5 minutes


Cold from Tap


Ice Water - 1 minute


Ice Water - 5 minutes


Temperature (°F)


Hot from Tap


Boiling


Boiling for 5 minutes


Cold from Tap


Ice Water - 1 minute


Ice Water - 5 minutes


Temperature (K)


Hot from Tap


Boiling


Boiling for 5 minutes


Cold from Tap


Ice Water - 1 minute


Ice Water - 5 minutes


85


100


20


2


-1


95


185


212


68


35.6


30.2


308.15


358.15


373.15


293.15


275.15


271.15


Copyright 2019 - Hands-On Labs | http://holscience.com 4 / 14


Data Table 3: Mass Measurements


Estimated Mass (g)


Pen or Pencil


3 Pennies


1 Quarter


2 Quarters, 3 Dimes


4 Dimes, 5 Pennies


3 Quarters, 1 Dime, 5 Pennies


Key


Key, 1 Quarter, 4 Pennies


Actual Mass (g)


Pen or Pencil


3 Pennies


1 Quarter


2 Quarters, 3 Dimes


4 Dimes, 5 Pennies


3 Quarters, 1 Dime, 5 Pennies


Key


Key, 1 Quarter, 4 Pennies


Actual Mass (kg)


Pen or Pencil


4


8


4


12


21


30


7


18


5.6


7.5


5.6


18


22.1


32.3


7.7


24


Copyright 2019 - Hands-On Labs | http://holscience.com 5 / 14


Exercise 2


3 Pennies


1 Quarter


2 Quarters, 3 Dimes


4 Dimes, 5 Pennies


3 Quarters, 1 Dime, 5 Pennies


Key


Key, 1 Quarter, 4 Pennies


0.0056


0.0075


0.0056


0.018


0.0221


0.0323


0.0077


0.024


Density= mass/ volume


Volume= length x width x height


Volume= 3.6 x 4.21 x 1.17= 17.73 cm


Density= 21.3/17.73= 1.20 g/mL


1. An unknown, rectangular substance measures 3.60 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)?


3


Copyright 2019 - Hands-On Labs | http://holscience.com 6 / 14


Density= mass/volume


Volume= mass/ density


Volume= 26.15/19.30= 1.35 mL Au


2. 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?


If you dropped the object into the beaker then the scale would measure the mass of the object instead of the mass of the displaced water and the measurements would be thrown off.


3. What would happen if you dropped the object into the beaker while using the Archimedes’ Principle method instead of submerging the object?


How the magnets density measurement using the Archimedes principles compare to the density measurement using the calculated volume is that the magnets density measurement during the Archimedes was higher than the density measurement using the calculated volume. I think that the Archimedes principle method might be more accurate because with the calculated volume there is more room for error as I made the measurements.


4. How did the magnet’s density cdalculation using the Archimedes’ Principle compare to the density calculation using the direct measurement method? Which technique might be more accurate? Why?


Copyright 2019 - Hands-On Labs | http://holscience.com 7 / 14


Data Table 4: Liquid Measurements


The conclusions I can reach from the simple density analysis is that is could not actually be gold because pure gold is 19.32 g/cm .


5. You are given a small piece of gold colored material and want to determine if it is actually gold. Using the Archimedes Principle you f ind that the volume is 0.40 cm and the mass is 6.0 g. What conclusions can you reach f rom your simple density analysis?


3


3


Water


Mass A: Graduated Cylinder (g)


Volume (mL)


Mass B: Graduated Cylinder with Liquid (g)


Mass B-A: Liquid (g)


Density (g/mL)


Percent Error (%)


Isopropyl Alcohol


Mass A: Graduated Cylinder (g)


Volume (mL)


Mass B: Graduated Cylinder with Liquid (g)


Mass B-A: Liquid (g)


Density (g/mL)


Percent Error (%)


19.3


5


24.4


5.1


1.00


26.4%


19.3


5


23.6


4.3


0.786


22.3%


Copyright 2019 - Hands-On Labs | http://holscience.com 8 / 14


Data Table 5: Magnet - Direct Measurement Method


Data Table 6: Water Displacement Method


Magnet


Mass (g)


Length (cm)


Width (cm)


Height (cm)


Volume (cm )


Density (g/cm )


4.2


2.5


0.5


2.5


3 3.125


3 1.344


Copyright 2019 - Hands-On Labs | http://holscience.com 9 / 14


Data Table 7: Archimedes' Method


Magnet


Mass (g)


Initial Volume of Graduated Cylinder (mL)


Final Volume of Graduated Cylinder (mL)


Object Volume (mL)


Density (g/mL)


Metal Bolt


Mass (g)


Initial Volume of Graduated Cylinder (mL)


Final Volume of Graduated Cylinder (mL)


Object Volume (mL)


Density (g/mL)


4.3


6


6.5


0.5


8.6


8


6


7


1


8


Copyright 2019 - Hands-On Labs | http://holscience.com 10 / 14


Exercise 3


Magnet


Mass (g)


Mass of Displaced Water (g)


Volume of Displaced Water (mL)


Density (g/mL)


Metal Bolt


Mass (g)


Mass of Displaced Water (g)


Volume of Displaced Water (mL)


Density (g/mL)


4.3


121.4


121.4


1


8


121.8


121.8


1


Copyright 2019 - Hands-On Labs | http://holscience.com 11 / 14


Data Table 8: Initial Concentration


1% x V1 = 2% x 2V


0.25 x 10 = 1 x 2V


V2= 0.25 x10/1


V2= 2.5mL


How I would prepare 10 mL of a 0.25% HCl solution if 1% HCl available is dilute the 1% in water to get a less concentrated .25% HCl. Then determine the amount of moles by multiplying 0.01 and .25 which equals 0.0025 moles HCl. Then, you prepare 10 mL containing 2.5 mL of 1% HCl.


1. How would you prepare 10 mL of a 0.25% m/v HCl solution if 1% m/v HCl was available? How much 1% m/v HCl is needed? How much distilled water is used?


The relations between the concentration of the sugar solution and the density of the sugar solution is that the density is a lot higher than the comcentration.


2. From the graph of Density vs. Concentration, created in Graph 1, what was the relationship between the concentration of the sugar solution and the density of the sugar solution?


Copyright 2019 - Hands-On Labs | http://holscience.com 12 / 14


Data Table 9: Solutions


Sugar (C H O )


Mass of Volumetric Flask (g)


Mass of Sugar (g)


Total Volume (mL)


Concentration (% m/V)


12 22 11


19.3


8


0.025


0.92%


Solution Volume (mL)


0 25.00 mL


1 25.00 mL


2 25.00 mL


3 25.00 mL


4 25.00 mL


Solution Mass (g)


0


1


2


3


4


Solution Density (g/mL)


0


1


26.5


25.3


25.4


25.4


25.5


1.06


Copyright 2019 - Hands-On Labs | http://holscience.com 13 / 14


2


3


4


Solution Initial Concentration (% m/v)


0


1


2


3


4


Solution Volume Transferred (mL)


0


1


2


3


4


Solution Final Concentration (% m/v)


0


1


2


3


1.012


1.016


1.016


1.02


0.92%


2.9%


2.9%


2.9%


0


2.5


4.5


3


6


0.925


2.9%


13.05%


Copyright 2019 - Hands-On Labs | http://holscience.com 14 / 14


Graph 1: Density versus Concentration


4


8.7%


17.4%

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