Rdr4 Chemical Equilibrium
bDATES PERFORMED: JANUARY 8, 2013
CHEMICAL EQUILIBRIUM
D.M. TAN1 AND P.B. ALEGRO2
1DEPARTMENT OF MINING, METALLURGICAL, AND MATERIALS ENGINEERING, COLLEGE OF ENGINEERING
2 INSTITUTE OF CHEMISTRY, COLLEGE OF SCIENCE
UNIVERSITY OF THE PHILIPPINES, DILIMAN QUEZON CITY, PHILIPPINES
RECEIVED JANUARY 15, 2013
RESULTS AND DISCUSSION
A. Iron- Silver Equilibrium
The first part of the experimentation focuses in the iron-silver system. Silver nitrate (AgNO3) was added to ferrous sulfate (FeSO4) shown in this equation: 2AgNO3(l) + FeSO4(l) Ag2SO4-(aq)+ Fe(NO3)2(aq) The additon of AgNO3 to FeSO4 equilibrium had an effect on the equlibria. Though no precipitate was formed after just mixing the solutions, a precipitate formed after centrifugation. This was done to achieve separation of silver precipitate to the supernate.
The silver precipitate is formed due to the unsolubility of AgNO3 which displaces the chemical equilibrium of FeSO4 towards the silver compound. This is an application of Le-Chatelier fundament which states that an equilibrium will attempt to shift in a direction that will counteract a stress that is placed on it.
The supernate was then tested for the presence of three ions namely, Fe2+, Fe3+, and Ag+. In the test for Fe2+, he supernate was added with K3Fe(CN)6 that resulted to net ionic equation: Fe2+(aq) + K3Fe(CN)6(aq) KFe[Fe(CN)6](s)
The precipitate which is KFe[Fe(CN)6](s) is a prussian blue precipitae which indicates the presence of Fe2+ ions. Next, for Fe3+, KCNS was added in the supernate shown in this net ionic equation: Fe3+(aq) + SCN-(aq) Fe(SCN)2+(aq)
A blood red solution was achieved which indicates the presence of Fe3+ ions. Lastly, for the Ag+ test, the HCl was added to the supernate shown in the ionic equation below: Ag+(aq) + Cl-(aq) AgCl(s)
A white precipitate formed which indicates the presence ogf Ag+ ions.
Since the reactants
CHEMICAL EQUILIBRIUM
D.M. TAN1 AND P.B. ALEGRO2
1DEPARTMENT OF MINING, METALLURGICAL, AND MATERIALS ENGINEERING, COLLEGE OF ENGINEERING
2 INSTITUTE OF CHEMISTRY, COLLEGE OF SCIENCE
UNIVERSITY OF THE PHILIPPINES, DILIMAN QUEZON CITY, PHILIPPINES
RECEIVED JANUARY 15, 2013
RESULTS AND DISCUSSION
A. Iron- Silver Equilibrium
The first part of the experimentation focuses in the iron-silver system. Silver nitrate (AgNO3) was added to ferrous sulfate (FeSO4) shown in this equation: 2AgNO3(l) + FeSO4(l) Ag2SO4-(aq)+ Fe(NO3)2(aq) The additon of AgNO3 to FeSO4 equilibrium had an effect on the equlibria. Though no precipitate was formed after just mixing the solutions, a precipitate formed after centrifugation. This was done to achieve separation of silver precipitate to the supernate.
The silver precipitate is formed due to the unsolubility of AgNO3 which displaces the chemical equilibrium of FeSO4 towards the silver compound. This is an application of Le-Chatelier fundament which states that an equilibrium will attempt to shift in a direction that will counteract a stress that is placed on it.
The supernate was then tested for the presence of three ions namely, Fe2+, Fe3+, and Ag+. In the test for Fe2+, he supernate was added with K3Fe(CN)6 that resulted to net ionic equation: Fe2+(aq) + K3Fe(CN)6(aq) KFe[Fe(CN)6](s)
The precipitate which is KFe[Fe(CN)6](s) is a prussian blue precipitae which indicates the presence of Fe2+ ions. Next, for Fe3+, KCNS was added in the supernate shown in this net ionic equation: Fe3+(aq) + SCN-(aq) Fe(SCN)2+(aq)
A blood red solution was achieved which indicates the presence of Fe3+ ions. Lastly, for the Ag+ test, the HCl was added to the supernate shown in the ionic equation below: Ag+(aq) + Cl-(aq) AgCl(s)
A white precipitate formed which indicates the presence ogf Ag+ ions.
Since the reactants