Lab Report Experiment 3 4 And 5 3d1ib
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CHM 474: INORGANIC CHEMISTRY AS 202
NO. OF EXPERIMENT
3, 4 & 5
TITLE
Synthesis of potassium tris(oxalate)chromium(III) trihydrate, copper(II) oxalate complex and
NAME
potassium tris(oxalate)ferrate(III) MOHAMAD trihydrate. ZULFIKRI BIN MAT JUSOH
STUDENT NUMBER
2014910247
PARTNER’S NAME
AMIRUL IMRAN BIN IDOPI
GROUP
AS2022M1
LECTURER’S NAME
DR. LIM YING CHI N
LAB. INSTRUCTOR
MISS SARAH
DATE OF EXPERIMENT
15th &22nd. OCT. 2015
DATE OF SUBMITION
30th OCT. 2015
OBJECTIVE: 1. To synthesis potassium tris(oxalate)chromium(III) trihydrate. 2. To prepare a copper(II) oxalate complex. 3. To synthesis potassium tris(oxalate)ferrate(III) trihydrate.
INTRODUCTION: One of important aspects of any chemical research was the preparation of new compound. This process called as synthesis. In this experiment we will synthesised a special kind of compound called as a coordination compound. A coordination compound consisted of a central metal ion chemically bonded to one or more atoms or groups of atoms known as ligands by coordinate covalent bond. Transition metal readily formed these coordination compound, often resulting in bright colour. In this experiment we performed three experiment was about preparation of crystals. The crystal that we prepared were potassium tris(oxalate)chromium(III) trihydrate, copper(II) oxalate complex and potassium tris(oxalate)ferrate(III) trihydrate. The amount of coordination compound expected from given mass of reactants can be calculated and it was called theoretical yield. The actual mass of the coordination compound synthesised was called actual yield and it was usually less than the theoretical yield.
PROCEDURE: Experiment 3 1. 5.00 g of oxalate acid was dissolved in 10 ml distilled water in a conical flask. 1.8 g of potassium dichromate was added into the mixture in small portions and the funnel was placed on the mouth of conical flask. 2. After the reaction had subsided, 2.10 g of potassium oxalate monohydrate was added into the hot green-black liquid and it was heated until boiling for 5 minutes. 3. The flask was cooled down at room temperature and 10 ml 95% ethanol was added into the flask and it was cooled in ice bath with frequent stirring. 4. After cooling in ice for 15 minutes or when the precipitate completely formed, the precipitate was collected by suction filtration. 5. The crystals were washed with 5 ml portion 1:1 ethanol/distilled water and followed by 13 ml of 95% ethanol. 6. The crystals were placed on the watch glass and it was allowed to dry in the oven. 7. The mass of the synthesis crystals and percentage yield were determined. 8. The crystals were transferred into a plastic packet. It was kept for next experiment. Experiment 4 1. 2.00 g copper(II) sulphate was weighed and it was placed in conical flask. 30 ml of distilled water was added in the flask. The flask was heated slowly on a hot plate until the solid dissolves. 2. 6.20 g of potassium oxalate monohydrate was dissolved in 30 ml of distilled water in another flask. 3. The heated CuSO4 solution was added into the flask contained potassium oxalate monohydrate slowly. The flask was swirled slowly to mix. 4. The mixture was cooled in ice bath for 30 minutes. Blue crystals were formed. 5. The crystals were placed on the watch glass and it was allowed to dry in the oven. 6. The mass of the synthesis crystals and percentage yield were determined. 7. The crystals were transferred into a plastic packet. It was kept for next experiment.
Experiment 5 Procedure A 1. 5.00 g of ferrous ammonium sulphate was dissolved in 25 ml distilled water containing 1 ml of diluted sulphuric acid in the beaker. 2. 2.50 g of oxalate acid dihydrate was dissolved in 25 ml of distilled water in another beaker. Then it was added into the beaker containing ferrous ammonium sulphate. 3. The mixture was heated slowly until boiling and then it was allowed the yellow precipitate to settle. The supernatant was discarded. 15 ml hot water was added into the yellow precipitate. It was stirred and the supernatant was discarded. 4. 15 ml of hot water was added to precipitate. 3.5 g of solid potassium oxalate o
monohydrate. It was heated to approximately 40 C. Then immediately 10 ml of 6% H2O2 was added drop wisely and it was stirred continuously. 5. It was heated to boiling and the dissolved solution of 2.0 g of oxalic acid in 30 ml of distilled water was added into the mixture until the brown precipitate was dissolved. 6. It was boiled until the solution was clear. The solution was filtered through Buchner funnel. 30 ml of 95% ethanol was added slowly to the solution. Any crystals were formed was redissolved. Then, it was leaved in not direct light to crystallise for a week. Procedure B 1. The crystals were collected by suction filtration process. The beaker was rinsed with 10 ml of 1:1 ethanol/distillation water for two times. The crystals were washed with cold acetone. 2. The crystals were placed on the watch glass and it was allowed to dry on air. 3. The mass of the synthesis crystals and percentage yield were determined. 4. The crystals were transferred into a plastic packet. It was kept for next experiment.
RESULTS: Experiment 3: mass of K2[Cr(C2O4)3].3H2O Mass of watch glass and filter paper
35.1230 g
Mass of watch glass and filter paper + crystals
40.0201 g
Mass of crystals
4.8971 g
Theoretical yield
5.6046 g
Percent yield
87.38 %
Experiment 4: mass of K2[Cu(C2O4)2.(H2O)2 Mass of watch glass and filter paper
31.5282 g
Mass of watch glass and filter paper + crystals
34.1391 g
Mass of crystals
2.6109 g
Theoretical yield
2.8657 g
Percent yield
91.11 %
Experiment 5: mass of K3[Fe(C2O4)3].3H2O Mass of filter paper
0.3337 g
Mass of filter paper + crystals
4.7415 g
Mass of crystals
4.4078 g
Theoretical yield
6.2851 g
Percent yield
70.13 %
CALCULATION: Experiment 3: 7H2C2O4 + K2Cr2O7 + 2K2C2O4.H2O
2K3[Cr(C2O4)3]. 3H2O + 4CO2 + 3H2O
Theoretical mass of K2[Cr(C2O4)3].3H2O 5.0123 g H2C2O4
x
1 mol H2C2O4
x
2 mol K3[Cr(C2O4)3. 3H2O
90.02 g H2C2O4 =
7 mol H2C2O4
0.0159 mol K3[Cr(C2O4)3. H2O
1.8273 g K2Cr2O7
x
1 mol K2Cr2O7
x
2 mol K3[Cr(C2O4)3. 3H2O
294.2 g K2Cr2O7 =
1 mol K2Cr2O7
0.0124 mol K3[Cr(C2O4)3. H2O
2.1111 g K2C2O4.H2O
x
1 mol 2K2C2O4.H2O 184.22 g 2K2C2O4.H2O
=
x
2 mol K3[Cr(C2O4)3. 3H2O 2 mol 2K2C2O4.H2O
0.0115 mol K3[Cr(C2O4)3. H2O
So, K2C2O4.H2O is limiting reactant 0.0115 mol K3[Cr(C2O4)3. 3H2O
x
487.36 g K3[Cr(C2O4)3].3 H2O 1 mol K3[Cr(C2O4)3. 3H2O
=
5.6046 g K3[Cr(C2O4)3. 3H2O
Percent yield of K3[Cr(C2O4)3. 3H2O 4.8971g 5.6046 g = 87.38 %
X
100
Experiment 4: CuSO4.5H2O +
2K2C2O4.H2O
K2[Cu(C2O4)2(H2O)2]
+ K2SO4 + 5H2O
Theoretical mass of K2[Cu(C2O4)2.(H2O)2] 2.0236 g CuSO4.5H2O x
1 mol CuSO4.5H2O
x
1mol K2[Cu(C2O4)2(H2O)2]
249.62 g CuSO4.5H2O =
0.0081 mol K2[Cu(C2O4)2(H2O)2]
6.2260 g K2C2O4.H2O
x
1 mol K2C2O4.H2O 184.22 g K2C2O4.H2O
=
1 mol CuSO4.5H2O
x
1 mol K2[Cu(C2O4)2(H2O)2] 2 mol K2C2O4.H2O
0.0169 mol K2[Cu(C2O4)2(H2O)2]
So, CuSO4.5H2O is limiting reactant 0.0081 mol K2[Cu(C2O4)2(H2O)2]
x
353.79 g K2[Cu(C2O4)2(H2O)2] 1 K2[Cu(C2O4)2(H2O)2]
=
2.8657 g K2[Cu(C2O4)2(H2O)2]
Percent yield of K2[Cu(C2O4)2(H2O)2] 2.6109 g x 2.8657 g =
91.11 %
100
Experiment 5: 3K2C2O4 + 2Fe(OH)3 + 3H2C2O4
2K3[Fe(C2O4)3].3H2O
+
3H2O
Theoretical mass of K3[Fe(C2O4)3].3H2O 5.0064 g Fe(NH4)2(SO4). 6H2O
x
1 mol Fe(NH4)2(SO4). 6H2O 392.02 g Fe(NH4)2(SO4). 6H2O
2+
= 0.0128 mol FeC2O4 x 1 mol Fe
x
1 mol FeC2O4 = 0.0128 mol Fe(OH)3
x
3+
2 mol Fe
x
1 mol Fe(OH)3
2+
2 mol Fe
3+
1 mol Fe
2 mol K3[Fe(C2O4)3].3H2O 2 mol Fe(OH)3
=
0.0128 mol K3[Fe(C2O4)3].3H2O
3.5004 g K2C2O4
x
1 mol K2C2O4
x
166.22 g K2C2O4 =
3 mol K2C2O4
0.0140 mol K3[Fe(C2O4)3].3H2O
2.0024 g H2C2O4
x
1 mol H2C2O4
x
90.02 g H2C2O4 =
2 mol K3[Fe(C2O4)3].3H2O
2 mol K3[Fe(C2O4)3].3H2O 3 mol H2C2O4
0.0148 mol K3[Fe(C2O4)3].3H2O
So, K2C2O4 is limiting reactant. 0.0128 mol K3[Fe(C2O4)3].3H2O
x
491.21 g K3[Fe(C2O4)3].3H2O 1 mol K3[Fe(C2O4)3].3H2O
=
6.2851 g K3[Fe(C2O4)3].3H2O
Percent yield of K3[Fe(C2O4)3].3H2O Actual yield X Theoretical yield 4.4078 g X 6.2851 g = %
100
100
70.13
DISCUSSION: In
this
experiment,
tris(oxalate)chromium(III)
we
had
trihydrate,
prepared
copper(II)
crystals
oxalate
such
complex
as
potassium
and
potassium
tris(oxalate)ferrate(III) trihydrate. The process to synthesis the crystals were known as crystallisation. The results of the experiment that we obtained were 4.8971 g emerald green solid K3[Cr(C2O4)3. 3H2O, 2.6109 g blue solid K2[Cu(C2O4)2(H2O)2] and 4.4078 g green solid K3[Fe(C2O4)3].3H2O. The percent yield that we get after the calculation were 87.36 % of
K3[Cr(C2O4)3.
3H2O,
91.11
%
of
K2[Cu(C2O4)2(H2O)2]
and
70.13
%
of
K3[Fe(C2O4)3].3H2O. The error may be occurred when we run this experiment that will affect the result of experiment. The error was there may be had some product remained at the Buchner funnel when we collected the product after suction filtration to transferred it into watch glass. Besides that, the product may dissolve when we washed the product with ethanol and cold water. The precautions that we must take in the experiment, we must always were wearing gloves to protect our hand from exposed to acid. Then, we must be careful handling hot plate when we heated the mixture.
CONCLUSION: The
conclusion
in
tris(oxalate)chromium(III)
the
experiment
trihydrate,
was
copper(II)
the
oxalate
crystals complex
of
potassium
and
potassium
tris(oxalate)ferrate(III) trihydrate were synthesised by crystallisation process. The percent yield of the crystals obtained were 87.36 % of K 3[Cr(C2O4)3. 3H2O, 91.11 % of K2[Cu(C2O4)2(H2O)2] and 70.13 % of K3[Fe(C2O4)3].3H2O.
REFERENCES: 1. Hadariah Bahron, Kamariah Muda, Sharifah Rohaiza Syed Omar, Karimah Kassim/2015/Inorgani Chemistry: Experiment for Undergraduates/UiTM PRESS. 2.
th
Silberberg, Amateis/2015/Chemistry: The Molecular Nature of Matter and Change 7 edition/Mc Graw Hill Education.
ANSWERS THE QUESTIONS: 1.
Oxidation state of chromium in K2Cr2O7 and in the product.
K2Cr2O7 = 0 (+1)(2) + (X)(2) + (-2)(7) = 0 2X = +14 – 2 X = +6
K3[Cr(C2O4)3]. 3H2O = 0 (+1)(3) + (X) + (-2)(3) + 3(0) = 0 X = +6 – 3 X = +3
2. Half equation reaction involved in preparation 2-
of the complex. 5C2O4 2-
Cr2O7
5C2O4
2-
+
14H
+ 14H
+
+
+ 10e
10CO2 2Cr
+ Cr2O7
2-
2+
10CO2
+ 10e +
7H2O + 2Cr
2+
+ 7H2O
Figure 1: flow chat for Experiment 3
Figure 2: flow chat for Experiment 4
nm
Figure 3: flow chat for Experiment 5
NO. OF EXPERIMENT
3, 4 & 5
TITLE
Synthesis of potassium tris(oxalate)chromium(III) trihydrate, copper(II) oxalate complex and
NAME
potassium tris(oxalate)ferrate(III) MOHAMAD trihydrate. ZULFIKRI BIN MAT JUSOH
STUDENT NUMBER
2014910247
PARTNER’S NAME
AMIRUL IMRAN BIN IDOPI
GROUP
AS2022M1
LECTURER’S NAME
DR. LIM YING CHI N
LAB. INSTRUCTOR
MISS SARAH
DATE OF EXPERIMENT
15th &22nd. OCT. 2015
DATE OF SUBMITION
30th OCT. 2015
OBJECTIVE: 1. To synthesis potassium tris(oxalate)chromium(III) trihydrate. 2. To prepare a copper(II) oxalate complex. 3. To synthesis potassium tris(oxalate)ferrate(III) trihydrate.
INTRODUCTION: One of important aspects of any chemical research was the preparation of new compound. This process called as synthesis. In this experiment we will synthesised a special kind of compound called as a coordination compound. A coordination compound consisted of a central metal ion chemically bonded to one or more atoms or groups of atoms known as ligands by coordinate covalent bond. Transition metal readily formed these coordination compound, often resulting in bright colour. In this experiment we performed three experiment was about preparation of crystals. The crystal that we prepared were potassium tris(oxalate)chromium(III) trihydrate, copper(II) oxalate complex and potassium tris(oxalate)ferrate(III) trihydrate. The amount of coordination compound expected from given mass of reactants can be calculated and it was called theoretical yield. The actual mass of the coordination compound synthesised was called actual yield and it was usually less than the theoretical yield.
PROCEDURE: Experiment 3 1. 5.00 g of oxalate acid was dissolved in 10 ml distilled water in a conical flask. 1.8 g of potassium dichromate was added into the mixture in small portions and the funnel was placed on the mouth of conical flask. 2. After the reaction had subsided, 2.10 g of potassium oxalate monohydrate was added into the hot green-black liquid and it was heated until boiling for 5 minutes. 3. The flask was cooled down at room temperature and 10 ml 95% ethanol was added into the flask and it was cooled in ice bath with frequent stirring. 4. After cooling in ice for 15 minutes or when the precipitate completely formed, the precipitate was collected by suction filtration. 5. The crystals were washed with 5 ml portion 1:1 ethanol/distilled water and followed by 13 ml of 95% ethanol. 6. The crystals were placed on the watch glass and it was allowed to dry in the oven. 7. The mass of the synthesis crystals and percentage yield were determined. 8. The crystals were transferred into a plastic packet. It was kept for next experiment. Experiment 4 1. 2.00 g copper(II) sulphate was weighed and it was placed in conical flask. 30 ml of distilled water was added in the flask. The flask was heated slowly on a hot plate until the solid dissolves. 2. 6.20 g of potassium oxalate monohydrate was dissolved in 30 ml of distilled water in another flask. 3. The heated CuSO4 solution was added into the flask contained potassium oxalate monohydrate slowly. The flask was swirled slowly to mix. 4. The mixture was cooled in ice bath for 30 minutes. Blue crystals were formed. 5. The crystals were placed on the watch glass and it was allowed to dry in the oven. 6. The mass of the synthesis crystals and percentage yield were determined. 7. The crystals were transferred into a plastic packet. It was kept for next experiment.
Experiment 5 Procedure A 1. 5.00 g of ferrous ammonium sulphate was dissolved in 25 ml distilled water containing 1 ml of diluted sulphuric acid in the beaker. 2. 2.50 g of oxalate acid dihydrate was dissolved in 25 ml of distilled water in another beaker. Then it was added into the beaker containing ferrous ammonium sulphate. 3. The mixture was heated slowly until boiling and then it was allowed the yellow precipitate to settle. The supernatant was discarded. 15 ml hot water was added into the yellow precipitate. It was stirred and the supernatant was discarded. 4. 15 ml of hot water was added to precipitate. 3.5 g of solid potassium oxalate o
monohydrate. It was heated to approximately 40 C. Then immediately 10 ml of 6% H2O2 was added drop wisely and it was stirred continuously. 5. It was heated to boiling and the dissolved solution of 2.0 g of oxalic acid in 30 ml of distilled water was added into the mixture until the brown precipitate was dissolved. 6. It was boiled until the solution was clear. The solution was filtered through Buchner funnel. 30 ml of 95% ethanol was added slowly to the solution. Any crystals were formed was redissolved. Then, it was leaved in not direct light to crystallise for a week. Procedure B 1. The crystals were collected by suction filtration process. The beaker was rinsed with 10 ml of 1:1 ethanol/distillation water for two times. The crystals were washed with cold acetone. 2. The crystals were placed on the watch glass and it was allowed to dry on air. 3. The mass of the synthesis crystals and percentage yield were determined. 4. The crystals were transferred into a plastic packet. It was kept for next experiment.
RESULTS: Experiment 3: mass of K2[Cr(C2O4)3].3H2O Mass of watch glass and filter paper
35.1230 g
Mass of watch glass and filter paper + crystals
40.0201 g
Mass of crystals
4.8971 g
Theoretical yield
5.6046 g
Percent yield
87.38 %
Experiment 4: mass of K2[Cu(C2O4)2.(H2O)2 Mass of watch glass and filter paper
31.5282 g
Mass of watch glass and filter paper + crystals
34.1391 g
Mass of crystals
2.6109 g
Theoretical yield
2.8657 g
Percent yield
91.11 %
Experiment 5: mass of K3[Fe(C2O4)3].3H2O Mass of filter paper
0.3337 g
Mass of filter paper + crystals
4.7415 g
Mass of crystals
4.4078 g
Theoretical yield
6.2851 g
Percent yield
70.13 %
CALCULATION: Experiment 3: 7H2C2O4 + K2Cr2O7 + 2K2C2O4.H2O
2K3[Cr(C2O4)3]. 3H2O + 4CO2 + 3H2O
Theoretical mass of K2[Cr(C2O4)3].3H2O 5.0123 g H2C2O4
x
1 mol H2C2O4
x
2 mol K3[Cr(C2O4)3. 3H2O
90.02 g H2C2O4 =
7 mol H2C2O4
0.0159 mol K3[Cr(C2O4)3. H2O
1.8273 g K2Cr2O7
x
1 mol K2Cr2O7
x
2 mol K3[Cr(C2O4)3. 3H2O
294.2 g K2Cr2O7 =
1 mol K2Cr2O7
0.0124 mol K3[Cr(C2O4)3. H2O
2.1111 g K2C2O4.H2O
x
1 mol 2K2C2O4.H2O 184.22 g 2K2C2O4.H2O
=
x
2 mol K3[Cr(C2O4)3. 3H2O 2 mol 2K2C2O4.H2O
0.0115 mol K3[Cr(C2O4)3. H2O
So, K2C2O4.H2O is limiting reactant 0.0115 mol K3[Cr(C2O4)3. 3H2O
x
487.36 g K3[Cr(C2O4)3].3 H2O 1 mol K3[Cr(C2O4)3. 3H2O
=
5.6046 g K3[Cr(C2O4)3. 3H2O
Percent yield of K3[Cr(C2O4)3. 3H2O 4.8971g 5.6046 g = 87.38 %
X
100
Experiment 4: CuSO4.5H2O +
2K2C2O4.H2O
K2[Cu(C2O4)2(H2O)2]
+ K2SO4 + 5H2O
Theoretical mass of K2[Cu(C2O4)2.(H2O)2] 2.0236 g CuSO4.5H2O x
1 mol CuSO4.5H2O
x
1mol K2[Cu(C2O4)2(H2O)2]
249.62 g CuSO4.5H2O =
0.0081 mol K2[Cu(C2O4)2(H2O)2]
6.2260 g K2C2O4.H2O
x
1 mol K2C2O4.H2O 184.22 g K2C2O4.H2O
=
1 mol CuSO4.5H2O
x
1 mol K2[Cu(C2O4)2(H2O)2] 2 mol K2C2O4.H2O
0.0169 mol K2[Cu(C2O4)2(H2O)2]
So, CuSO4.5H2O is limiting reactant 0.0081 mol K2[Cu(C2O4)2(H2O)2]
x
353.79 g K2[Cu(C2O4)2(H2O)2] 1 K2[Cu(C2O4)2(H2O)2]
=
2.8657 g K2[Cu(C2O4)2(H2O)2]
Percent yield of K2[Cu(C2O4)2(H2O)2] 2.6109 g x 2.8657 g =
91.11 %
100
Experiment 5: 3K2C2O4 + 2Fe(OH)3 + 3H2C2O4
2K3[Fe(C2O4)3].3H2O
+
3H2O
Theoretical mass of K3[Fe(C2O4)3].3H2O 5.0064 g Fe(NH4)2(SO4). 6H2O
x
1 mol Fe(NH4)2(SO4). 6H2O 392.02 g Fe(NH4)2(SO4). 6H2O
2+
= 0.0128 mol FeC2O4 x 1 mol Fe
x
1 mol FeC2O4 = 0.0128 mol Fe(OH)3
x
3+
2 mol Fe
x
1 mol Fe(OH)3
2+
2 mol Fe
3+
1 mol Fe
2 mol K3[Fe(C2O4)3].3H2O 2 mol Fe(OH)3
=
0.0128 mol K3[Fe(C2O4)3].3H2O
3.5004 g K2C2O4
x
1 mol K2C2O4
x
166.22 g K2C2O4 =
3 mol K2C2O4
0.0140 mol K3[Fe(C2O4)3].3H2O
2.0024 g H2C2O4
x
1 mol H2C2O4
x
90.02 g H2C2O4 =
2 mol K3[Fe(C2O4)3].3H2O
2 mol K3[Fe(C2O4)3].3H2O 3 mol H2C2O4
0.0148 mol K3[Fe(C2O4)3].3H2O
So, K2C2O4 is limiting reactant. 0.0128 mol K3[Fe(C2O4)3].3H2O
x
491.21 g K3[Fe(C2O4)3].3H2O 1 mol K3[Fe(C2O4)3].3H2O
=
6.2851 g K3[Fe(C2O4)3].3H2O
Percent yield of K3[Fe(C2O4)3].3H2O Actual yield X Theoretical yield 4.4078 g X 6.2851 g = %
100
100
70.13
DISCUSSION: In
this
experiment,
tris(oxalate)chromium(III)
we
had
trihydrate,
prepared
copper(II)
crystals
oxalate
such
complex
as
potassium
and
potassium
tris(oxalate)ferrate(III) trihydrate. The process to synthesis the crystals were known as crystallisation. The results of the experiment that we obtained were 4.8971 g emerald green solid K3[Cr(C2O4)3. 3H2O, 2.6109 g blue solid K2[Cu(C2O4)2(H2O)2] and 4.4078 g green solid K3[Fe(C2O4)3].3H2O. The percent yield that we get after the calculation were 87.36 % of
K3[Cr(C2O4)3.
3H2O,
91.11
%
of
K2[Cu(C2O4)2(H2O)2]
and
70.13
%
of
K3[Fe(C2O4)3].3H2O. The error may be occurred when we run this experiment that will affect the result of experiment. The error was there may be had some product remained at the Buchner funnel when we collected the product after suction filtration to transferred it into watch glass. Besides that, the product may dissolve when we washed the product with ethanol and cold water. The precautions that we must take in the experiment, we must always were wearing gloves to protect our hand from exposed to acid. Then, we must be careful handling hot plate when we heated the mixture.
CONCLUSION: The
conclusion
in
tris(oxalate)chromium(III)
the
experiment
trihydrate,
was
copper(II)
the
oxalate
crystals complex
of
potassium
and
potassium
tris(oxalate)ferrate(III) trihydrate were synthesised by crystallisation process. The percent yield of the crystals obtained were 87.36 % of K 3[Cr(C2O4)3. 3H2O, 91.11 % of K2[Cu(C2O4)2(H2O)2] and 70.13 % of K3[Fe(C2O4)3].3H2O.
REFERENCES: 1. Hadariah Bahron, Kamariah Muda, Sharifah Rohaiza Syed Omar, Karimah Kassim/2015/Inorgani Chemistry: Experiment for Undergraduates/UiTM PRESS. 2.
th
Silberberg, Amateis/2015/Chemistry: The Molecular Nature of Matter and Change 7 edition/Mc Graw Hill Education.
ANSWERS THE QUESTIONS: 1.
Oxidation state of chromium in K2Cr2O7 and in the product.
K2Cr2O7 = 0 (+1)(2) + (X)(2) + (-2)(7) = 0 2X = +14 – 2 X = +6
K3[Cr(C2O4)3]. 3H2O = 0 (+1)(3) + (X) + (-2)(3) + 3(0) = 0 X = +6 – 3 X = +3
2. Half equation reaction involved in preparation 2-
of the complex. 5C2O4 2-
Cr2O7
5C2O4
2-
+
14H
+ 14H
+
+
+ 10e
10CO2 2Cr
+ Cr2O7
2-
2+
10CO2
+ 10e +
7H2O + 2Cr
2+
+ 7H2O
Figure 1: flow chat for Experiment 3
Figure 2: flow chat for Experiment 4
nm
Figure 3: flow chat for Experiment 5
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