WRITE THE BALANCED CHEMICAL EQUATION,WRITE THE OVERALL IONIC EQUATION,IDENTIFY THE SPECTOR IONS AND POSSIBLE PRECIPITATES,WRITE THE NET IONIC EQUATION FOR mercury(II)chloride(aq)+potassium sulfide(aq)
You add the (aq) and (s)
HgCl2(aq) + K2S(aq) ==> HgS(s) + 2KCl(aq)
Now separate into ions but leave HgS(s) as the molecular form
Finally, cancel any ions that are common to both sides of the equation.
What is the balanced chemical equation for the reaction hcl(aq) + ca(oh)2(aq) cacl2(aq) + h2o(l)
To write the balanced chemical equation for the reaction between mercury(II) chloride (HgCl2, aq) and potassium sulfide (K2S, aq), we can use the following steps:
Step 1: Write the chemical formulas of the reactants and products.
HgCl2 (aq) + K2S (aq) → ?
Step 2: Identify the ions present in the reactants and products.
HgCl2 dissociates into the ions Hg2+ (aq) and 2Cl- (aq).
K2S dissociates into the ions 2K+ (aq) and S2- (aq).
Step 3: Write the balanced chemical equation by combining the ions to form products.
The balanced chemical equation for the reaction is:
HgCl2 (aq) + K2S (aq) → HgS (s) + 2KCl (aq)
To write the overall ionic equation, we need to write the equation with the dissociated ions:
Overall Ionic Equation:
Hg^2+ (aq) + 2Cl- (aq) + 2K+ (aq) + S^2- (aq) → HgS (s) + 2K+ (aq) + 2Cl- (aq)
To identify the spectator ions and possible precipitates, we compare the compounds on both sides of the equation:
Spectator ions: K+ and Cl- (These ions appear on both sides of the equation and do not participate in the formation of the precipitate.)
Possible Precipitate: HgS (s) is the precipitate formed as it appears only on the product side and not on the reactant side.
Net Ionic Equation:
Hg^2+ (aq) + S^2- (aq) → HgS (s)
Therefore, the net ionic equation for the reaction is:
Hg^2+ (aq) + S^2- (aq) → HgS (s)
To write the balanced chemical equation, the overall ionic equation, identify the spectator ions and possible precipitates, and write the net ionic equation for the reaction between mercury(II) chloride (HgCl2) and potassium sulfide (K2S), you should follow these steps:
Step 1: Write the balanced chemical equation:
HgCl2(aq) + K2S(aq) → HgS(s) + 2KCl(aq)
The balanced chemical equation is obtained by combining the ions of the two reactants based on their charges. The reactants and products should have the same number and type of atoms.
Step 2: Write the overall ionic equation:
In the overall ionic equation, we separate all the reactants and products into their constituent ions:
Hg2+(aq) + 2Cl-(aq) + 2K+(aq) + S2-(aq) → HgS(s) + 2K+(aq) + 2Cl-(aq)
Step 3: Identify the spectator ions:
Spectator ions are the ions that are present on both sides of the equation and do not undergo any change during the reaction. In this case, the K+ and Cl- ions are spectator ions. They are present on both sides of the equation, and their charges do not change. Therefore, they are not involved in the formation of the precipitate.
Step 4: Identify possible precipitates:
To determine if a precipitate is formed, we need to check the solubility rules. According to the solubility rules, mercury (II) sulfide (HgS) is insoluble, so it will precipitate.
Step 5: Write the net ionic equation:
The net ionic equation shows only the reactants and products that directly participate in the formation of the precipitate. To write the net ionic equation, we eliminate the spectator ions from the overall ionic equation:
Hg2+(aq) + S2-(aq) → HgS(s)
In this net ionic equation, the 2+ charge on mercury (Hg) is balanced by the 2- charge on sulfide (S), resulting in the formation of solid mercury sulfide (HgS) precipitate.
So, the final balanced chemical equation is:
HgCl2(aq) + K2S(aq) → HgS(s) + 2KCl(aq)
The overall ionic equation is:
Hg2+(aq) + 2Cl-(aq) + 2K+(aq) + S2-(aq) → HgS(s) + 2K+(aq) + 2Cl-(aq)
The spectator ions are K+ and Cl-.
The net ionic equation is:
Hg2+(aq) + S2-(aq) → HgS(s)