What is the full net ionic equation for each reaction? do they form a precipitate or have a color change?
CuSO4+AgNO3
CuSO4+BaCl2
CuSO4+Cu(NO3)2
CuSO4+Pb(NO3)2
CuSO4+KI
CuSO4+Na2S2O3
AgNO3+BaCl2
AgNO3+Cu(NO3)2
AgNO3+Pb(NO3)2
AgNO3+KI
AgNO3+Na2S2O3
BaCl2+Cu(NO3)2
BaCl2+Pb(NO3)2
BaCl2+KI
BaCl2+Na2S2O3
Cu(NO3)2+Pb(NO3)2
Cu(NO3)2+KI
Cu(NO3)2+Na2S2O3
Pb(NO3)2+KI
Pb(NO3)2+Na2S2O3
KI+Na2S2O3
You need to know the solubility of compounds to work these problems. If a ppt (an insoluble material) is produced, then the reaction will proceed. Here is a simplified site that gives the solubility of the most common materials.
http://www.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
Na2S2O3 + AgNO3
hi i was just wondering what the solution would be to:
AgNO3 + Na2S2O3 + sunlight (light enegy)
?
To find the full net ionic equation for each reaction, we need to first write the balanced molecular equation. Then, we can determine the ions that participate in the reaction and write the full ionic equation by representing all species that are present as their separate ions. Finally, we can cancel out spectator ions to obtain the net ionic equation, which only includes the ions directly involved in the reaction.
Let's go through each reaction step-by-step:
1. CuSO4 + AgNO3
Molecular Equation: CuSO4(aq) + 2AgNO3(aq) → Cu(NO3)2(aq) + Ag2SO4(s)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + 2Ag+(aq) + 2NO3^-(aq) → Cu2+(aq) + 2NO3^-(aq) + 2Ag2SO4(s)
Net Ionic Equation: SO4^2-(aq) + 2Ag+(aq) → Ag2SO4(s)
Precipitate Formation: Yes, Ag2SO4(s) is a precipitate.
2. CuSO4 + BaCl2
Molecular Equation: CuSO4(aq) + BaCl2(aq) → BaSO4(s) + CuCl2(aq)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + Ba2+(aq) + 2Cl^-(aq) → BaSO4(s) + Cu2+(aq) + 2Cl^-(aq)
Net Ionic Equation: Ba2+(aq) + SO4^2-(aq) → BaSO4(s)
Precipitate Formation: Yes, BaSO4(s) is a precipitate.
3. CuSO4 + Cu(NO3)2
Molecular Equation: CuSO4(aq) + Cu(NO3)2(aq) → Cu2SO4(s) + 2Cu(NO3)2(aq)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + Cu2+(aq) + 2NO3^-(aq) → Cu2SO4(s) + 2Cu2+(aq) + 2NO3^-(aq)
Net Ionic Equation: Cu2+(aq) + SO4^2-(aq) → Cu2SO4(s)
Precipitate Formation: Yes, Cu2SO4(s) is a precipitate.
4. CuSO4 + Pb(NO3)2
Molecular Equation: CuSO4(aq) + Pb(NO3)2(aq) → PbSO4(s) + Cu(NO3)2(aq)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + Pb2+(aq) + 2NO3^-(aq) → PbSO4(s) + Cu2+(aq) + 2NO3^-(aq)
Net Ionic Equation: Cu2+(aq) + SO4^2-(aq) → CuSO4(s)
Precipitate Formation: No, there is no precipitate formed.
5. CuSO4 + KI
Molecular Equation: CuSO4(aq) + 2KI(aq) → CuI2(s) + K2SO4(aq)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + 2K+(aq) + 2I^-(aq) → CuI2(s) + 2K+(aq) + SO4^2-(aq)
Net Ionic Equation: 2I^-(aq) → I2(s)
Precipitate Formation: No, there is no precipitate formed.
6. CuSO4 + Na2S2O3
Molecular Equation: CuSO4(aq) + Na2S2O3(aq) → CuS2O3(s) + Na2SO4(aq)
Full Ionic Equation: Cu2+(aq) + SO4^2-(aq) + 2Na+(aq) + S2O3^2-(aq) → CuS2O3(s) + 2Na+(aq) + SO4^2-(aq)
Net Ionic Equation: No reaction occurs.
The same steps can be followed for the remaining reactions to determine the full net ionic equation and whether precipitates or color changes occur.