When the following solutions are mixed together, FeSO4 (aq) + Csl (aq):
What precipitate if any will form,
Write the balanced equation, write the complete ionic equation and write the net ionic equation?
Answered below.
To determine if a precipitate will form when FeSO4(aq) is mixed with Csl(aq), we need to consider the solubility rules.
First, let's write the balanced equation for the reaction:
FeSO4(aq) + Csl(aq) → FeCl2(aq) + Cs2SO4(aq)
Next, let's write the complete ionic equation by separating all the soluble compounds into their individual ions:
Fe2+(aq) + SO42-(aq) + Cs+(aq) + Cl-(aq) → Fe2+(aq) + 2Cl-(aq) + Cs+(aq) + SO42-(aq)
Now, let's write the net ionic equation by removing the spectator ions (ions that appear on both sides of the equation and don't participate in the reaction):
SO42-(aq) + 2Cl-(aq) → no reaction
Since there is no reaction between sulfate ions (SO42-) and chloride ions (Cl-), no precipitate will form in this case.
To determine the net ionic equation, you need to be familiar with the solubility rules and the concept of spectator ions. By checking the solubility rules, you can determine if any of the possible reaction products are insoluble, leading to the formation of a precipitate.