Aqueous solutions of iron (III) sulphate and barium hydroxide are combined. Does a precipitate form? If yes write a net ionic equation for the precipitation reaction. You first identify the formula of the aqueous
compounds (note that iron is said to be iron(III)), and use it to write the
balanced equation; then list the four ionic species (each compound
dissociates into two type of ions) and use them as reagent for your
ionic equation.
Yes, a precipitate will form. The net ionic equation for the precipitation reaction is:
Fe3+ + OH- → Fe(OH)3(s)
To determine whether a precipitate forms when aqueous solutions of iron (III) sulphate (Fe2(SO4)3) and barium hydroxide (Ba(OH)2) are combined, we need to consider the solubility rules for these compounds.
The solubility rules state that most sulphates are soluble, while hydroxides are generally insoluble except when they are with Group 1 (alkali metals) and a few Group 2 (alkaline earth metals) elements, such as barium (Ba).
First, let's write the balanced equation for the reaction:
Fe2(SO4)3 (aq) + 3Ba(OH)2 (aq) → 2Fe(OH)3 (s) + 3BaSO4 (aq)
This equation shows that iron (III) sulphate reacts with barium hydroxide to form a precipitate of iron (III) hydroxide and soluble barium sulphate.
To write the net ionic equation, we need to ignore the spectator ions, which are the ions that do not participate in the reaction and remain in solution. In this case, the spectator ions are Ba2+ and SO42-. The net ionic equation can be written as follows:
Fe3+ (aq) + 3OH- (aq) → Fe(OH)3 (s)
This net ionic equation shows the essential chemical reaction between the iron (III) ion and hydroxide ion to form iron (III) hydroxide as the precipitate.
To determine if a precipitate forms when aqueous solutions of iron (III) sulfate and barium hydroxide are combined, we need to consider the solubility rules for these compounds.
Iron (III) sulfate, Fe2(SO4)3, is soluble in water as it is a group 1 sulfate or ammonium salt and does not contain a group 2 cation. This means it will dissociate into its ions: Fe3+ and 3 SO42-.
Barium hydroxide, Ba(OH)2, is also soluble in water as it is a group 1 hydroxide or alkali metal hydroxide. This means it will dissociate into its ions: Ba2+ and 2 OH-.
Now let's write the balanced equation for the reaction:
Fe2(SO4)3 (aq) + 3 Ba(OH)2 (aq) -> 2 Fe(OH)3 (s) + 3 BaSO4 (s)
Balancing the equation, we see that two moles of Fe2(SO4)3 react with six moles of Ba(OH)2 to yield two moles of Fe(OH)3 and six moles of BaSO4.
From the balanced equation, we can see that a precipitate does form in this reaction. The net ionic equation for the precipitation reaction can be written by cancelling out the spectator ions (ions that are present on both sides of the equation and do not participate in the reaction). The net ionic equation is as follows:
Fe3+ (aq) + 3 OH- (aq) -> Fe(OH)3 (s)
So, the net ionic equation for the precipitation reaction in this case is Fe3+ (aq) + 3 OH- (aq) -> Fe(OH)3 (s).