formal lab
Noah Stewart-Maddox
Chem 121
10/12/11
Synthesis of Potassium Ferric Oxalate Trihydrate and
The Determination of Oxalate Ion in Ferric Oxalate Trihydrate using Titrimetry
Abstract: In this two-part lab, we will learn about coordination compounds and their uses with stoiciometry. We will also find out about how theoretical yield is calculated from a reaction we will create. We will also synthesize Potassium Ferric Oxalate Trihydrate (K_3 [〖Fe(C_2 O_4)〗_3]•3H_2 O) using a two step reaction. In the second part of this lab we will calculate how much Oxalate Ion is present in the K_3 [〖Fe(C_2 O_4)〗_3]•3H_2 O using tirtimetry. This process is called quantitative chemical analysis and will be very helpful.
Introduction: To produce K_3 [〖Fe(C_2 O_4 )〗_3 ]•3H_2 O we will use a two step reaction:
Fe〖(NH_4)〗_2 〖(SO_4)〗_2•6H_2 O+H_2 C_2 O_4 □(→┴ ) FeC_2 O_4•2H_2 O+〖(NH_4)〗_2 SO_4+H_2 SO_4+4H_2 O
We will then use the Ferrous Oxalate Dihydrate (FeC_2 O_4•2H_2 O) in the second step of the reaction:
2FeC_2 O_4•2H_2 O+H_2 C_2 O_4+H_2 O_2+3K_2 C_2 O_4 □(→┴ ) 2K_3 [〖Fe〖(C〗_2 O_4)〗_3]•3H_2 O
This compound is called a coordination compound, which mean it contains a compound ion. In the second part of our lab, we calculated the amount of Oxalate Ion in our compound using titration. We will use the reaction: 5〖 C_2 O_4〗^(2-) + 2〖 MnO_4〗^- + 16 H^+ □(→┴ ) 10 CO_2+ 2 〖Mn〗^(2+) + 8 H_2 O
When stoichiometrically equivalent amounts of titrant is added to the reaction the color changed from clear to pink. This is beneficial, because it allows us to calculate the amount of the compound we were looking to calculate. This must be done with care, because the reaction is rather sudden and will change colors quickly. To do this we use a buret, which is a very precise instrument. In our reaction we have a formula that tells use the relation between the moles of the standard and the moles of〖 C_2 O_4〗^(2-):
#moles of 〖 C_2 O_4〗^(2-)=(5 moles 〖 C_2 O_4〗^(2-))/(2 moles 〖MnO_4〗^- )
Chem 121
10/12/11
Synthesis of Potassium Ferric Oxalate Trihydrate and
The Determination of Oxalate Ion in Ferric Oxalate Trihydrate using Titrimetry
Abstract: In this two-part lab, we will learn about coordination compounds and their uses with stoiciometry. We will also find out about how theoretical yield is calculated from a reaction we will create. We will also synthesize Potassium Ferric Oxalate Trihydrate (K_3 [〖Fe(C_2 O_4)〗_3]•3H_2 O) using a two step reaction. In the second part of this lab we will calculate how much Oxalate Ion is present in the K_3 [〖Fe(C_2 O_4)〗_3]•3H_2 O using tirtimetry. This process is called quantitative chemical analysis and will be very helpful.
Introduction: To produce K_3 [〖Fe(C_2 O_4 )〗_3 ]•3H_2 O we will use a two step reaction:
Fe〖(NH_4)〗_2 〖(SO_4)〗_2•6H_2 O+H_2 C_2 O_4 □(→┴ ) FeC_2 O_4•2H_2 O+〖(NH_4)〗_2 SO_4+H_2 SO_4+4H_2 O
We will then use the Ferrous Oxalate Dihydrate (FeC_2 O_4•2H_2 O) in the second step of the reaction:
2FeC_2 O_4•2H_2 O+H_2 C_2 O_4+H_2 O_2+3K_2 C_2 O_4 □(→┴ ) 2K_3 [〖Fe〖(C〗_2 O_4)〗_3]•3H_2 O
This compound is called a coordination compound, which mean it contains a compound ion. In the second part of our lab, we calculated the amount of Oxalate Ion in our compound using titration. We will use the reaction: 5〖 C_2 O_4〗^(2-) + 2〖 MnO_4〗^- + 16 H^+ □(→┴ ) 10 CO_2+ 2 〖Mn〗^(2+) + 8 H_2 O
When stoichiometrically equivalent amounts of titrant is added to the reaction the color changed from clear to pink. This is beneficial, because it allows us to calculate the amount of the compound we were looking to calculate. This must be done with care, because the reaction is rather sudden and will change colors quickly. To do this we use a buret, which is a very precise instrument. In our reaction we have a formula that tells use the relation between the moles of the standard and the moles of〖 C_2 O_4〗^(2-):
#moles of 〖 C_2 O_4〗^(2-)=(5 moles 〖 C_2 O_4〗^(2-))/(2 moles 〖MnO_4〗^- )