Student Name
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
Crystals
Lab Partner
Demonstrator
Lab Section
DATA SHEET
Preparation of a Coordination Compound
Step 1
Copy the balanced equation for the preparation of FeC2O4.2H2O.
Mass taken of
FeSO4(NH4)2SO4.6H2O
or
mol
Mass of H2C2O4.2H2O
or
mol
Limiting reagent is
Theoretical yield of FeC2O4.2H2O
Step 2
mol
Copy the balanced equation for the preparation of K3Fe(C2O4)3.3H2O from
FeC2O4.2H2O.
Theoretical yield of K3Fe(C2O4)3.3H2O
(based on FeC2O4.2H2O as limiting reagent)
and in grams
Mass of watch glass and K3Fe(C2O4)3.3H2O
Mass of watch glass
Yield of K3Fe(C2O4)3.3H2O
Percent Yield of K3Fe(C2O4)3.3H2O
Description of product crystals, i.e. size, colour, shape, etc. :
mol
g
WORK SHEET
Keep extra digits in all calculations when possible. Keep track of the extra digits
by underlining or bracketing them.
Do not show calculations to find molar mass.
Step 1
Calculate moles of FeSO4(NH4)2SO4.6H2O
Calculate moles of H2C2O4.2H2O
Limiting reagent - explain or show mathematically why you choose this to be the LR
(Do not just give the definition of a LR)
Step 2
Calculate the theoretical yield, in grams, of K3Fe(C2O4)3.3H2O
Calculate the percent yield of K3Fe(C2O4)3.3H2O
Prelab Exercise
Name
This exercise reviews the calculations associated with this experiment. It must be
completed before the laboratory period, and handed in before the prelab lecture begins.
(Do not show calculations to find molar masses.)
a.
If you weighed out the following quantities of each reagent, which would be the
limiting reagent in Step 1, the synthesis of FeC2O4.2H2O ? Show and explain
your work.
Ferrous ammonium sulphate hydrate
2.45 g
Oxalic acid hydrate
1.35 g
b.
Using your data from question a, calculate the theoretical yield in grams of the
potassium trioxalatoferrate (III) trihydrate complex.
Student Name
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
NaOH and Unkn
Demonstrator
Lab Section
DATA SHEET
Acid-Base Titration, a Quantitative Analysis
Part 1 Standardization of NaOH solution
Mass of boat and sample
Mass of boat after transfer
Mass of sample transferred
Final burette reading
Initial burette reading
Volume of NaOH
Calculated molarity of NaOH
Lab. average molarity of NaOH (from your demonstrator)
% deviation of your value from lab. average
Part 2 Molar Mass of an Acid
Unknown #
ia =
Mass of boat and sample
Mass of boat after transfer
Mass of sample transferred
Final burette reading
Initial burette reading
Volume of NaOH
Calculated molar mass
Average values for the molar mass of the acid - the averages below will be the same
number but may have different SF
Average molar mass of the acid
( SF method)
Average molar mass of the acid
ssd
(ssd method)
WORK SHEET
Use extra digits in all calculations when possible.
Part 1 Molarity of the NaOH
Calculate the molarity of NaOH solution
equation (3)
Calculate the % deviation of your [NaOH] from the class average value
Part 2 Molar Mass of Unknown Acid - show calculation for one run only
Calculate the molar mass of the acid unknown - use the class average value for the
[NaOH]
equation (3)
Average Molar Mass Of the Unknown Acid - Read the instructions carefully.
List all four values from lowest to highest. You may use all four values to calculate the
average, or you may use the three closest values. Calculate the range of the three
lowest and the range of the three highest. If the ranges are significantly different then
use the three with the smallest range, otherwise use all four. Show the range
calculations and clearly indicate whether you will be using three or four values to
calculate the average and ssd.
Use your calculator to find the average value ( x! ) and sx value (the ssd). The ssd will
always have the same units as the average value. You will record the average value
twice on the data sheet. Once using the correct SF according to the SF method and
once using the ssd to determine the number of SF.
x! value ____________
sx value ( the ssd ) ____________
Prelab Exercise
Name
This exercise reviews the calculations associated with this experiment. It must be
completed before the laboratory period, and handed in before the prelab lecture begins.
a.
A sample weighing 0.3515 g of the primary standard potassium hydrogen
phthalate requires 12.42 mL of NaOH solution for neutralization. Calculate the
molarity of the NaOH solution.
b.
An organic acid has 2 ionizable hydrogen atoms in the molecule. 0.1548 g of
acid is dissolved in water and titrated with the standardized NaOH solution,
question a. The final equivalence point is reached after 15.62 mL of the base
solution have been added. Calculate the molar mass of the acid.
Student Name
Lab Partner
Demonstrator
Lab Section
DATA SHEET
Molar Volume of Nitrogen Gas
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
Molar V, Unkn
Part 1 Determination of Molar Volume of N2 (g)
Mass of vial and NaNO2
Mass of vial
Mass of NaNO2
Moles of NaNO2
Moles of N2 gas
Temperature of N2 gas
°C
Temperature of N2 gas
K
Temperature of water
°C
Volume of N2 gas
Atmospheric pressure
Pressure due to H2O vapour
Pressure of N2 (g) alone
Volume of N2 (g) corrected
to reference conditions
L mol!1
Molar volume of N2 (g)
Molar volume of an ideal gas
at 25°C, 100 kPa
% deviation of my measured
molar volume from the ideal
24.789 L mol!1
DATA SHEET
Molar Volume of Nitrogen Gas
Part 2 Determination of mass percent of NaNO2 in Unknown #
Mass of vial and Unknown
Mass of vial
Mass of Unknown
Temperature of N2 gas
°C
Temperature of N2 gas
K
°C
Temperature of water
Volume of N2 gas
Atmospheric pressure
Pressure due to H2O vapour
Pressure of N2 (g) alone
Volume of N2 (g) corrected
to 25°C and 100 kPa
Your Molar Volume of N2 from Part 1
Moles of N2 produced
Moles of NaNO2 in sample
Mass of NaNO2 in sample
% by mass of NaNO2
Average Values for the mass percent of NaNO2 , the two averages below will be the
same number but may have different SF
Average % by mass of NaNO2
(SF method)
Average % by mass of NaNO2
ssd
Additional Calculation - see work sheet
Average % by mass of NaNO2
(SF method)
WORK SHEET
Part 1 Determination of Molar Volume of N2 (g)
Calculate moles of NaNO2 reacted
Calculate pressure of N2 (g) alone, equation (5)
Calculate volume of N2(g) corrected to reference conditions, 298.15 K and 100 kPa,
equation (3)
Calculate molar volume of N2(g), equation (4)
Calculate the % deviation of your experimental molar volume from that of an ideal gas,
24.789 L mol!1
Part 2 Determination of NaNO2 content, show calculations for one run only
Calculate pressure of N2(g) alone
Calculate volume of N2(g) corrected to reference conditions
Calculate moles of N2 produced
Calculate mass of NaNO2 reacted
Calculate % by mass of NaNO2 in the sample
Average value
Write both your % by mass values below and then use your calculator to find the
average value ( x! ) and sx value ( the ssd ) for the % by mass of NaNO2 .
x! value
sx value ( the ssd )
You will record the average value twice on the data sheet. Once using the correct SF
according to the SF method and once using the ssd to determine the number of SF.
Additional Calculation The results for Part 2 could be recalculated using the actual
molar volume of N2(g) , 24.777 L mol-1, instead of your molar volume. An easier way to
get the same average value is to use the formula given below and your average mass
% of NaNO2. Use the value with the SF according to the SF method.
Average Mass % of NaNO2 x
Molar Volume (yours)
Molar Volume (given)
Prelab Exercise
Name
This exercise reviews the important calculations associated with this experiment.
It must be completed before the laboratory period, and handed in before the
prelab lecture begins.
a. When 0.4853 g of NaNO2 is allowed to react with an excess of sulfamic acid
solution, the volume of N2(g) produced is measured by displacement of 163 mL of
water. After the reaction is completed, the temperature of water is 26.0°C and that of
gas is 24.0°C. The atmospheric pressure is 101.56 kPa. Use equations (3, 4 and 5) to
calculate the molar volume of N2 (g) at 25°C and 100 kPa. You may not use PV = nRT.
b. When 0.6087 g of a sample containing NaNO2 and some inert material is allowed to
react with an excess of sulfamic acid solution, 128 mL of dry N2 (g) at 25°C and
100 kPa are obtained. Calculate the percentage by mass of NaNO2 in the sample with
the aid of the molar volume of N2 (g) at 25°C and 100 kPa from question a.
Student Name
Prelab exercise
Lab performance
Sig figs, units
Calculations
Graph
pKa, stock conc.
Lab Partner
Demonstrator
Lab Section
DATA SHEET
Spectrophotometric Determination of the pKa of an Indicator
tube
HIn
acetic acid
acetate
#
mL
mL
mL
1
10.00
2
10.00
9.00
1.00
3
10.00
8.00
2.00
4
10.00
7.00
3.00
5
10.00
6.00
4.00
6
10.00
5.00
5.00
7
10.00
4.00
6.00
8
10.00
3.00
7.00
9
10.00
2.00
8.00
10
10.00
1.00
9.00
11
10.00
pH absorbance
— 10.00 mL HCl —
— 10.00 mL NaOH —
The pH entries above are calculated in the pre-lab exercise.
Model of Spectronic 20 used, analog or digital
Indicator concentration, sample tube
Indicator concentration, stock solution
Calculated absorbance AK for [HIn] = [In2]
pKa of bromocresol green
Ka of bromocresol green
colour
WORK SHEET
Use the absorption constant, ,, for the In2 ion and path length R, given in the strategy
and procedure, to calculate the indicator concentration in the sample tube
equation (3)
Calculate the indicator concentration in the stock solution - before dilution
Calculate the absorbance AK , for [HIn] = [In2]
equation (4)
Find the pKa of bromocresol green indicator from your graph, read to 2 decimal places,
label AK and pKa on the graph.
pKa =
Ka =
Prelab Exercise
Name
This exercise consists of important calculations required for this experiment. It must be
completed before the laboratory period, and handed in before the prelab lecture begins.
You will need these data for your graph !
a. Calculate the pH of 10.00 mL of 0.100 M HCl after adding 10.00 mL of indicator
solution. Round the pH to three significant figures.
Calculate the pH of 10.00 mL of 0.100 M NaOH after adding 10.00 mL of indicator
solution. Round the pH to three significant figures.
b. Calculate the pH of the nine buffer solutions made by mixing 1.10 M acetic acid and
0.900 M sodium acetate solutions according to the following proportions.
The pKa for acetic acid, CH3COOH, is 4.745. See Introduction for information on
SF and log functions.
mL 1.10M HAc
9.00
8.00
7.00
6.00
5.00
4.00
3.00
2.00
1.00
mL 0.900M Ac2
1.00
2.00
3.00
4.00
5.00
6.00
7.00
8.00
9.00
pH ( 3 SF )
Show a detailed calculation for one mixture only. The pKa for acetic acid is 4.745.
Student Name
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
Graphs
Unknown
Lab Partner
Demonstrator
Lab Section
DATA SHEET
Thermochemistry
Part 1 Determination of the Heat Capacity of the Calorimeter
Mass of calorimeter dry
Mass of calorimeter plus cold water
Temperature of cold water + calorimeter
Temperature of hot water
Final mass of calorimeter plus water
Mass of cold water
Mass of hot water
Extrapolated temperature, To
)T for hot water, To ! Thot
K
)T for cold water and calorimeter, To ! Tcold
K
Heat capacity of calorimeter, Ccal
The temperature chart and all grey areas must be filled in and checked by the TA
before you leave the lab.
DATA SHEET
DATA FOR COOLING CURVES
(Use ink)
TIME
min
Part 1
Temp °C
Part 2
Temp °C
Part 3
Temp °C
extra
Temp °C
extra
Temp °C
0.5
1.0
1.5
2.0
2.5
3.0
3.5
4.0
4.5
5.0
5.5
6.0
6.5
7.0
REMEMBER !
WEIGH THE CALORIMETER AND SOLUTION AT THE END OF EVERY RUN.
DATA SHEET
Part 2 The Heat of Neutralization of a Strong Base With a Strong Acid
Molarity of standard HCl
Final burette reading
Initial burette reading
Volume of standard HCl used
Mass of calorimeter plus final solution
Mass of dry calorimeter
Mass of final solution
Initial temperature of HCl
Initial temperature of NaOH
Avg temperature of HCl and NaOH, Taverage
Extrapolated temperature, To
)T, To – T average
Specific heat of NaCl solution, cs
Heat absorbed by calorimeter + solution
Heat of reaction
Moles of H+ reacted
)Hneut
Average value of )Hneut
K
DATA SHEET
Part 3
Determination of the Concentration of Strong Acid Solution #
Final burette reading
Initial burette reading
Volume of unknown HCl used
Mass of calorimeter plus final solution
Mass of dry calorimeter
Mass of final solution
Initial temperature of HCl solution
Initial temperature of NaOH solution
Avg temperature of HCl and NaOH, Taverage
Extrapolated temperature, To
)T, To – Taverage
K
Specific heat of NaCl solution, cs
Heat absorbed by calorimeter and solution
Heat of reaction
Average Heat of neutralization ( from Part 2 )
Moles of HCl used
Molarity of Unknown HCl solution
Avg Molarity of Unknown HCl solution
( SF method )
Avg Molarity of Unknown HCl solution
ssd
Additional Calculation
Avg Molarity of Unknown HCl solution
( SF method )
(ssd method)
WORK SHEET
Part 1 The Heat Capacity of the Calorimeter
Calculate the heat capacity of calorimeter
equation (4)
If your value of Ccal is negative, check for mathematical errors first, then use
Ccal = 0 J K21 in all subsequent calculations.
Part 2 The Heat of Neutralization of a Strong Acid With a Strong Base
show calculations for one run only
Calculate heat absorbed by calorimeter + solution,
qabs = [ Ccal ( To – Tavg ) + ms cs ( To – Tavg ) ]
= [ Ccal + ms cs] ( To – Tavg )
equation (5)
Heat of reaction = q rxn =
Calculate moles of H+ reacted - the limiting reagent
Calculate )Hneut
Write both your values and then calculate the average value of )Hneut,
x! value
equation (6)
Part 3 Determination of the Concentration of Strong Acid Solution
show calculations for one run only
Calculate heat absorbed by calorimeter + solution,
qabs = [ Ccal ( To – Tavg ) + ms cs ( To – Tavg ) ]
= [ Ccal + ms cs] ( To – Tavg )
equation (5)
Heat of reaction = q rxn =
equation (6)
Calculate moles of H+ reacted
Calculate molarity of unknown HCl solution
Write both your values here and then calculate average molarity and ssd
x! value
sx value ( the ssd )
Additional Calculation
The actual value of the )Hneut is - 55.9 kJ mol!1 . Calculate the molarity of your
unknown HCl using this value as follows. Show this calculation.
Your average molarity x
)Hneut (yours)
)Hneut (given)
Prelab Exercise
Name
This exercise reviews the important calculations associated with this experiment.
It must be completed before the laboratory period, and handed in before the
prelab lecture begins.
a. When 14.28 mL of 2.92 M HCl are added to 15 mL of 3.07 M NaOH, a
measurement shows that 2.35 kJ of heat are released. Calculate the heat of
neutralization in kJ mol21.
b. Similarly, when 13.98 mL of HCl of unknown concentration (but less than that of
the base) are reacted with 15 mL of 3.07 M NaOH, 2.08 kJ of heat are released.
From these experimental data, calculate the molarity of the HCl solution.
Student Name
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
Lab Partner
Demonstrator
Lab Section
DATA SHEET
Redox Titration, a Quantitative Analysis
Part 1 Standardization of the KMnO4 Solution
Preparation of Na2C2O4 solution
Mass of weighing funnel & Na2C2O4
Mass of clean, dry weighing funnel
Mass of Na2C2O4 in 100.00 mL solution
mol L21
Molarity of Na2C2O4 solution
Titration Results
run #
1
Final burette reading
Initial burette reading
Volume of KMnO4 solution
Average volume of KMnO4 used
Average molarity of KMnO4
Class average molarity of KMnO4
% deviation of my value from the class average value
2
3
DATA SHEET
Redox Titration, a Quantitative Analysis
Part 2 Determination of Fe2+ Content in an Iron Supplement Pill
Pill #1
#
Pill #2
Pill #3
Mass of powdered pill & boat
Mass of empty boat
Mass of pill
Average molarity of KMnO4 (your own, Part 1)
Final burette reading
Initial burette reading
Volume of KMnO4 solution
Moles of KMnO4
Moles of Fe2+
Fe2+ content in pill, mg
Moles of FeSO4.7H2O
Mass of FeSO4.7H2O
Mass % of FeSO4.7H2O
Average Mass % of FeSO4.7H2O in pill
(SF method)
Average Mass % of FeSO4.7H2O in pill
ssd
Additional calculation
Average Mass % of FeSO4.7H2O in pill
(SF method)
WORK SHEET
Part 1 Standardization of the KMnO4 Solution
Calculate the molarity of Na2C2O4 solution
Calculate the molarity of KMnO4 solution - a 25.00 mL volume of Na2C2O4 solution
was used for every run so the average value of the volume of KMnO4 can be used to
find your average [KMnO4]
Calculate % deviation of your average value from Part 1 from the class average value
Part 2 Determination of Fe2+ Content and Mass Percent FeSO4.7H2O in an Iron
Supplement Pill, Show calculations for one run only. Use your [KMnO4] value.
Calculate moles of permanganate used
Calculate moles of Fe2+
Calculate Fe2+ content in pill in mg
Calculate mass of FeSO4.7H2O in pill, in g
Calculate mass % of FeSO4.7H2O in pill
Write your three values here and then calculate average mass % and ssd of
FeSO4.7H2O in pill.
x! value
sx value ( the ssd )
Additional Calculation
Calculate the average mass percent of FeSO4.7H2O using the class average [KMnO4 ]
as follows. Show this calculation.
Average Mass % of FeSO4.7H2O x
[KMnO4 ] (class)
[KMnO4 ] (yours)
Prelab Exercise
Name
This exercise reviews the important calculations associated with this experiment.
It must be completed before the laboratory period, and handed in before the prelab
lecture begins.
a.
If 34.86 mL of KMnO4 solution are required to oxidize 25.00 mL of 0.02987 M
Na2C2O4 solution, what is the [KMnO4] ?
b.
A certain brand of iron supplement pill contains iron(II) sulphate heptahydrate,
FeSO4.7H2O, with miscellaneous binders and fillers. 26.84 mL of the KMnO4
solution used in part a) are needed to oxidize Fe2+ to Fe3+ in a 0.4835 g pill.
Calculate the mass % of FeSO4.7H2O (molar mass = 278.0 g mol--1) in the pill.
Lab Partner
Student Name
Demonstrator
QUALITATIVE ANALYSIS - DATA SHEET
Unknown # _____
ion(s)
tested
Colour of Unknown Solution _____________
reagent(s)
added
observations for known
observations for unknown
1. Ag+
HCl
2. NH4+
NaOH
flame
red litmus
what happens to red litmus?
<
what happens to red litmus?
<
3. Cu2+
1) NaOH
1)
2)
1)
2) NH3
1)
2)
2)
Al3+
1)
2)
Fe2+
1)
Fe3+
1)
Zn2+
interpretation
ion(s)
tested
reagent(s)
added
4. Na+
observations for known
observations for unknown
<
wire or
+
Li
wooden stick
<
flame
2+
<
Cu
5. SO422
<
1) BaCl2
1)
1)
2) HCl
2)
2)
6. NO32
FeSO4
H2SO4
<
<
7. CO322
in large t.t.,
what happens to limewater?
what happens to limewater?
<
<
unknown + HCl
heat
in other
large t.t.,
limewater
inter
ion(s)
tested
reagent(s)
added
8. PO432
(NH4)6Mo7O2
observations for known
observations for unknown
interpretation
4
@4H2O
HNO3
heat (if necessary)
9. Cl2
AgNO3
10. Br2
I2
C2HCl3 +
chlorine water
colour in the lower layer for Br2
<
colour in the lower layer
<
colour in the lower layer for I2
<
Unknown # _____ contains ___________________________________________________________ .
Pre-Lab Exercise
Name
This exercise reviews the reactions associated with this experiment. It must be
completed before the laboratory period, and handed in before the pre-lab lecture.
JoAnn Student has an Unknown solution that contains iron (III) sulphate. For each
ion, state the test(s) that will show a positive result. Write the reaction(s) that will
occur for each, including states.
a.
iron (III) ion
test number ______
equation
b.
sulphate ion
equation
test number ______
Marking scheme
Prelab exercise
Lab performance
Sig figs, units
Calculations
Graphs
Orders
Student Name
Lab Partner
Demonstrator
Lab Section
Kinetics
SUMMARY DATA SHEET
Molarity of the stock potassium iodide solution
Molarity of the stock potassium bromate solution
Molarity of the stock hydrochloric acid solution
Integral order of the reaction in [BrO32] is
Integral order of the reaction in [H+] is
Integral order of the reaction in [I2] is
Overall order of the reaction is
Average value of the rate constant k,
ssd
(with units)
at an average room temperature of
Value of the Activation Energy, Ea is
ssd
K
Table 1: Experimental Data
run #
stock
°C
time t
s
relative rate
1000 / t
mol L!1 s!1
n/a
n/a
n/a
temperature
[BrO32]
in flask
mol L!1
1
1
avg of
run #1
2
3
4
5
6
7
8
t start _____
t finish _____
t avg
______
9
t start _____
t finish _____
t avg
______
10
grey boxes must be filled in before leaving the lab
[H+]
in flask
mol L!1
[I2]
in flask
mol L!1
WORK SHEETS
Preparation of 0.001000 M Na2S2O3 solution
Stock solution molarity
Calculate the volume of stock solution required to prepare 250.00 mL of 0.001000 M
Na2S2O3 solution.
Determination of the Values for ", $, p and k at room temperature
Determination of the value of "
run #
[BrO32]
run #
[BrO32]
relative rate
relative rate
Calculate the value of ", the order for [BrO32]
Integral value of "
Value of "
Determination of the value of $, the order for [H+]
[H+]
relative rate
run #
run #
[H+]
relative rate
Calculate the value of $
Value of $
Integral value of $
Determination of the value of p , the order of the reaction for [I2]
Table 2: [I !] and Relative Rates at Room Temperature
run #
[I2] in flask
mol L21
log [I2]
relative rate
mol L21 s21
log(rate)
Graph log(rate) vs log [I !] and calculate the slope. If graphing by hand show the slope
calculation and points used on your graph. Computer generated graphs must have the
equation of the line printed on the graph by the computer.
Value of p
Integral value of p
Determination of the average value of the rate constant, k
Use your integral values for ", $ and p to calculate k for each run, equation (1).
Table 3: Concentrations, Relative Rates and k at Room Temperature
run
#
[BrO32]
mol L21
[H+]
mol L21
[I2]
mol L21
relative
rate
temp.
K
k
Show one sample calculation of the value of k, and the derivation of the units of k
here.
List your values for k and then use your calculator to find the average and ssd.
Average value of k
ssd
units
List your values for the temperature and then use your calculator to find the average
and ssd.
at an average temperature
ssd
K
Determination of the Activation Energy, Ea
Use your integral values for ", $ and p to calculate k for each run, equation (1). It is
not necessary to show this calculation again (see above).
Table 4: k Values at Various Temperatures
run #
[BrO32]
mol L21
[H+]
mol L21
[I2]
mol L21
relative rate
mol L21 s21
k
temp
°C
Table 5: Arrhenius Data
approx
run #
temp,.°C
actual
1/T
temperature, K
K2
k
ln k
1
5
15
room
use
average
35
Graph ln k vs 1/T and calculate the slope. If graphing by hand show the slope
calculation and points used on your graph. Computer generated graphs must have the
equation of the line printed on the graph by the computer.
Slope of the line is
Calculate the value of Ea using the slope of your graph
Value of the Activation Energy Ea is
kJ mol21
Prelab Exercise
Name
This exercise reviews some important calculations associated with this experiment. It
must be completed before the laboratory period, and handed in before the prelab
lecture begins.
a)
Which two runs will you use to determine " ?
b)
Which two runs will you use to determine $ ?
c)
Which five runs will you use to determine p ?
d)
For the reaction
A ! Products
Calculate the value of k and the correct units.
[A]
rate
0.040 M
6.25 x 10 !6 mol L!1 s!1
0.080 M
2.50 x 10 !5 mol L!1 s!1