techniques and measurements

Write the background on techniques and measurements,write the purpose of experiment, and write the procedure of the lab experiments.(which I have outlined here.) Procedure: Length Measurements
1.gather a metric ruler,cd or dvd,key,spoon,and a fork
2.look at the calibration marks on your ruler to determine the degrees of uncertainty and number of significant figures that can be made when measuring objects with a ruler.
3.measure the length of each of the following objects(cd or dvd,key,spoon,fork) with the ruler in centimeters (cm),to one degree of uncertainty and record in data table 1.
4. measure the length of each of the following objects(cd,dvd,key,spoon,fork) with the ruler in millimeters (mm),to one degree of uncertainty,and record in data table 1.
5.convert the measurements for each of the objects to meters and record in data table 1.
6.gather the 100ml glass beaker,cup,matches or lighter,burner stand,burner fuel,and thermometer.
7.look at the calibration marks on the thermometer to determine the degree of uncertainty and number of significant figures that can be made when measuring temperature.
8.turn on the tap water to hot. Let the water run as hot as possible for approximately 15 seconds.
9.fill the 100ml glass beaker with approximately 75 ml of hot tap water.
10. measure the temperature of the hot tap water with the thermometer in degrees celcius to one degree of uncertainty.Record the measurement in data table 2.
11.place the beaker of water on the wire gauze burner stand.
12.put on safety glasses.
13.remove the cap from the burner fuel and set it aside. Use the matches or lighter to light the fuel and slip it under the burner stand.
14.allow the water to heat until it is at a full boil.As soon as the water is boiling,measure the temperature with the thermometer in degrees celcius to one degree of uncertainty. Record the measurement in data table 2.
15.allow the water to continue boiling for approximately 5 minutes. After 5 minutes, measure the temperature with the thermometer in degrees celcius to one degree of uncertainty.
16. extinguish the burner fuel by placing lid loosely on the can to cut off air supply.
17.allow the 100ml beaker to cool before touching it.
18. turn on the tap water to cold.Let water run for approximately 15 seconds.
19.fill a cup half full with cold tap water.
20.measure temperature of cold tap water in degree celcius. Record measurement in data table 2.
21. add handful of ice cubes to cold tap water and allow them to sit for 1 minute.
22.after 1 minute stir ice water with thermometer.
23.measure temperature of ice water after 1 minute in degree celcius
24.allow the ice to remain in water for additional 5 minutes.
25.after 5 minutes measure with thermometer.
26.measure temperature of ice water after 5 minutes in degree celcius.
27.convert the temperature measurements for each of the 6 water samples from celcius,fahreheit,and kelvin degrees.
28.gather pen or pencil,5 pennies,3 quarters,4 dimes,and a key
29. use digital scale to make mass measurements
30. turn scale on
31.make sure scale is reading grams
32. review different objects listed in data table 3
33. estimate masses for each of the objects in grams
34.tare the scale so it reading 0.0g
35.place the pen or pencil on the scale to measure the mass of the object.
36.repeat steps 33 and 34 for the remaining objects
37. for each object convert actual mass in grams to kiograms
Volume and Density Measurements(liquid)
1. gather a graduated cylinder,distilled water,short step pipet,and isoproply alcohol.
2.place the clean dry,25ml cylinder on tarred scale record mass in grams
3.fill graduated cylinder with 5ml of water measure exactly 5ml of water.
4. place 25ml cylinder with 5ml distilled water on tarred scale record mass of cylinder plus liquid in grams.
5.calculate mass of water by subtracting mass A from mass B
6. pour water down the drain and allow cylinder to dry
7. repeat steps 2 through 6 for isopropyl alcohol
8. calculate the densities of both the water and alcohol
9.the accepted value for the density of water is 1g/ml and the accepted density for isopropyl alcohol is 0.786 g.ml. Determine the percent error between your calculated densities and the accepted values for both water and alcohol. Record percent error in data table 4
Volume and Density Measurements(solid):
10. gather metal bolt ,string,magnet,graduated cylinder beaker, metric ruler,and scale
11. tare the scale so scale reads 0.0g
12. place the magnet on scale to measure its mass
13.use ruler to measure length,width,and height of magnet in centimeters
14. calculate volume multiply length x width x height
15.calculate density of magnet by dividing mass by volume
Water Displacement Method
16.tare the scale so it reads 0.0g
17. place magnet on scal emeasure mass of object
18. fill graduated cylinder with distilled water
19. place magnet into cylinder and read volume and record
20. determine volume by calculating the difference in water displacement
21. calculate density of magnet and record data
22. pour water down drain collect magnet
23.repeat steps 16 through 22 for metal bolt.
24. tare the scale so it reads 0.0g
25.place metal bolt on the scale to measure the mass of the object
26. attach the end of a string to the metal bolt by tying the string to the bolt
27. fill glass beaker 3/4 full with distilled water
28. tare the scale so it reads 0.0g
29.holding onto the string submerge bolt into water so that bolt is fully submerged but not touching any part of the glass beaker.
30. convert the mass of displaced water to volume of displaced water,assuming the density of water is 1g/ml record in data table 7
31.calculate the density of the metal bolt and record in data table 7
32.repeat steps 24 through 31 for the magnet
Exercise 3: Concentration,Solution,and Dilution
1. gather volumetric flask,distilled water,graduated pipet bulb,sugar,scale,glass beaker,cup,scissors,and a sheet of white paper.
2.cut small square of white paper and place it on the scale.
3.tare the scale so scale read 0.0g
4.weight 8.0 grams of sugar.Record mass in data table 8
5.carefully transfer the sugar from the white paper into the volumetric flask.
6.determine the molecular weight of sugar (C12H22O11) assuming the following:C=12.01 grams/mol,H=1.008 grams/mol, and O=15.99 grams/mol
7.record the molecular weight (grams of sugar ) in data table 8, under molecular weight.
8.determine the number of moles of sugar in the volumetric flask (mass/molecular weight) record in data table 8 under “moles in volumetric flask”
9. fill volumetric flask containing the 8.0 g of sugar to the 25 ml mark with distilled water.
10. record total volume in liters in data table 8 Note: you will need to convert the 25 ml to liters to determine this volume.
11.determine the molarity of the sugar solution in the volumetric flask using the following equation: Molarity=moles in volumetric flask(mol)/total volume (L)
12. record the molarity of the sugar solution in three places: in data table 8,under molarity in data table 9 under final concentration” in the “dilution O” column, and in data table 9 under “initial concentration” in the “dilution 1” column.
13. swirl the volumetric flask until the sugar is completely dissolved in the water. It will take a few minutes of swirling,but will completely dissolve.
14.place the clean dry, glass beaker on the scale and tare the scal eso scal ereads 0.0g
15. carefully pour the sugar solution from the volumetric flask into the beaker on the scale. Record mass of sugar solution in data table 9 for “dilution O”.
16. calculate the density of the sugar solution and record in data table 9 for “dilutioin O”.
17. rinse volumetric flask with distilled water and dry flask.
18.use the volumetric pipet to transfer 2.5 ml of the sugar solution from dilution O (which is in the glass beaker) into the volumetric flask.
19.carefully pour the remainder of the “dilution O” sugar solution down the drain
20. rinse the glass beaker with distilled water and dry.
21. fill the volumetric flask to the 25ml mark with distilled water. Use the short stem pipet to help fill the flask to exactly 25ml.
22. swirl the volumetric flask to thoroughly mix the sugar solution with the distilled water.
23. place clean dry, glass beaker on scale tare scale so it reads 0.0g
24. carefully pour the sugar solution from the volumetric flask into the beaker on the scale. Record mass of sugar solutioin and record in data table 9 for “dilution 1”
25. calculate the density of the sugar solution and record in data table 9 for “dilutioin 1”
26. determine the final concentration (m) for dilution 1 using the following equation”M1xV1=M2xV2
in this equation:M=initial concentration, V=volume transferred,V=25ml, M2= “final concentration”.
28. repeat steps 17 through 27 for the remaining 3 dilutions (4.5ml,3ml, and 6ml) in data table 9
29. create an excel chart displaying the relationship netween molarity and density for the sugar solution. The x axis on the chart will be the density, and the y axis on the chart will be molarity include the chart in essay.

Data Table 1: Length measurements.
Object Length (cm) Length (mm) Length (m)
CD or DVD
Key
Spoon
Fork
Data Table 2: Temperature measurements.
Water Temperature (°C) Temperature (°F) Temperature (K)
Hot from tap
Boiling
Boiling for 5 minutes
Cold from tap
Ice water – 1 minute
Ice water – 5 minutes
Data Table 3: Mass measurements.
Object Estimated Mass (g) Actual Mass (g) Actual Mass (kg)
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
Data Table 4: Liquid measurements.
Mass A Mass B Mass B – A

Liquid
Volume
(mL)
Graduated
Cylinder (g) Graduated
Cylinder
with liquid (g)

Liquid (g) Density

g/mL
% Error

Water

Isopropyl alcohol
Data Table 5: Magnet – Measurement Method.

Object: Mass
(g) Length
(cm) Width
(cm) Height
(cm) Volume
(cm3) Density
(g/cm3)
Magnet
Data Table 6: Displacement Method.

Object
Mass
(g) Initial volume of graduated cylinder (mL) Final volume of graduated cylinder (mL) Object Volume (mL)
Density
(g/mL)
Magnet
Metal bolt
Data Table 7: Archimedes’ Method.

Object
Mass
(g) Mass of Displaced Water (g) Volume of Displaced Water (mL)
Density (g/mL)
Metal Bolt
Magnet
Data Table 8: Initial Concentration.

Chemical
Mass
(g) Molecular Weight (g) Moles in Volumetric Flask Total Volume (L)
Molarity
(mol/L)
Sugar

(C12H22O11)
Data Table 9: Dilution Series.

Dilution
Volume
(mL)

Mass (g)
Density (g/
mL) Initial Concentration (M) Volume Transferred (mL) Final Concentration (M)
0 25 mL 0 mL
1 25 mL 2.5 mL
2 25 mL 4.5 mL
3 25 mL 3 mL
4 25 mL 6 mL
(These are the questions in order down below)
A. 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?
B. While heating two different samples of water at sea level, one boils at 102°C and one boils at
99.2°C. Calculate the percent error for each sample from the theoretical 100.0°C.
C. 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)
D. 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?
E. What would happen if you dropped the object into the beaker while using the Archimedes’
Principle method instead of submerging the object
F. How did the magnet’s density measurement using the Archimedes’ Principle compare to the density measurement using the calculated volume? Which method might be more accurate? Why?
G. 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?
H. 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?

I. From the Excel chart of Molarity vs. Density, what was the relationship between the molarity of the sugar solution and the density of the sugar solution?