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 wriye the net ionic equation?
There is no reaction between these two compounds. Each will dissociate in water.
To determine the precipitate and write the balanced, complete ionic, and net ionic equations for the reaction between FeSO4 (aq) and Csl (aq), we need to understand the solubility rules and reactions of the ions involved.
Solubility Rules:
1. Most sulfate (SO4^2-) salts are soluble, except those of calcium, strontium, barium, lead, and silver.
2. Most chloride (Cl-) salts are soluble, except those of lead, silver, and mercury (I).
3. Most Group IA (alkali metal) and ammonium (NH4+) salts are soluble.
Given that potassium sulfate (K2SO4) and iron(II) chloride (FeCl2) are soluble, we can predict the following reaction:
FeSO4 (aq) + 2KCl (aq) ⟶ FeCl2 (aq) + K2SO4 (aq)
Now, let's write the balanced equation:
FeSO4 (aq) + 2KCl (aq) ⟶ FeCl2 (aq) + K2SO4 (aq)
To write the complete ionic equation, we separate all the soluble compounds into their respective ions:
Fe^2+ (aq) + SO4^2- (aq) + 2K+ (aq) + 2Cl- (aq) ⟶ Fe^2+ (aq) + 2Cl- (aq) + 2K+ (aq) + SO4^2- (aq)
Simplifying the equation, we get:
SO4^2- (aq) + 2K+ (aq) + Fe^2+ (aq) + 2Cl- (aq) ⟶ 2Cl- (aq) + 2K+ (aq) + SO4^2- (aq) + Fe^2+ (aq)
Now, let's write the net ionic equation by eliminating the spectator ions (ions that appear on both sides and do not participate in the reaction):
Fe^2+ (aq) + 2Cl- (aq) ⟶ FeCl2 (s)
The net ionic equation shows that the formation of a precipitate occurs in this reaction, which is FeCl2 (s).