1. Will a precipitate form if solutions of potassium sulfate and barium nitrate are combined? If so, write the net ionic equation for the reaction.
2. Will a precipitate form if solutions of potassium nitrate and magnesium sulfate are combined? If so, write the net ionic equation for the reaction.
3. Will a precipitate form if solutions of barium chloride and sodium sulfate are combined? If so, identify the spectator ions and write the net ionic equation.
4. Write the net ionic equation for the precipitation of nickel(II)sulfide.
My answer:
1. no rxn
2. no rxn
3. no rxn
4. Ni2+ (aq) + S2- (aq) ---->NiS (s)
I don't believe you know the solubility rules. Here is a simplified set.
http://www.files.chem.vt.edu/RVGS/ACT/notes/solubility_rules.html
So the answer to 1 is yes because BaSO4 is insoluble.
The answer to 2 is no because KNO3, MgSO4, K2SO4 and Mg(NO3)2 are soluble.
If the answer to 1 is yes then the answer to 3 must be yes, also.
Your answer for 4 is right.
You need to write the net ionic equations for the others and identify the spectator ions.
you got this wrong because all of them are except for number 2
1. To determine if a precipitate will form when solutions of potassium sulfate and barium nitrate are combined, we need to check if a potential insoluble compound is formed. By consulting a solubility chart, we can see that barium sulfate (BaSO4) is insoluble in water. Therefore, a precipitate will form.
To write the net ionic equation for the reaction, we can first write the balanced molecular equation:
K2SO4(aq) + Ba(NO3)2(aq) → BaSO4(s) + 2KNO3(aq)
Next, we can separate the soluble compounds into their ions:
2K+(aq) + SO4^2-(aq) + Ba^2+(aq) + 2NO3^-(aq) → BaSO4(s) + 2K+(aq) + 2NO3^-(aq)
Finally, we can cancel out the spectator ions that appear on both sides of the equation:
Ba^2+(aq) + SO4^2-(aq) → BaSO4(s)
2. In the case of combining potassium nitrate and magnesium sulfate solutions, no precipitate will form. Both potassium nitrate and magnesium sulfate are soluble in water, so the ions will remain in solution.
3. When barium chloride and sodium sulfate solutions are combined, a precipitate of barium sulfate (BaSO4) will form. Barium sulfate is insoluble in water.
The net ionic equation can be written as:
Ba^2+(aq) + SO4^2-(aq) → BaSO4(s)
The spectator ions in this reaction are chloride ions (Cl^-) and sodium ions (Na+), as they appear on both sides of the equation but do not participate in the precipitation reaction.
4. The net ionic equation for the precipitation of nickel(II) sulfide (NiS) can be written as:
Ni^2+(aq) + S^2-(aq) → NiS(s)
To determine if a precipitate will form in a chemical reaction, you need to consider the solubility rules and the balanced chemical equation.
1. For the reaction between potassium sulfate (K2SO4) and barium nitrate (Ba(NO3)2), we can use the solubility rules to determine if a precipitate will form.
The solubility rule states that sulfates (SO4 2-) are generally soluble, except for those of barium (Ba2+), strontium (Sr2+), and lead (Pb2+).
On the other hand, nitrate (NO3-) salts are generally soluble.
Since both the reactants are soluble compounds, no precipitate will form in this case. The net ionic equation is not applicable in this scenario.
2. For the reaction between potassium nitrate (KNO3) and magnesium sulfate (MgSO4), we can use the same approach.
Both potassium nitrate and magnesium sulfate are soluble compounds. Therefore, no precipitate will form in this reaction as well. The net ionic equation is not applicable.
3. For the reaction between barium chloride (BaCl2) and sodium sulfate (Na2SO4), we need to refer to the solubility rules again.
The solubility rule states that most chlorides (Cl-) are soluble, including barium chloride. Sulfates (SO4 2-) are also soluble, except when combined with barium, strontium, or lead.
Since barium sulfate (BaSO4) is insoluble, a precipitate will form in this reaction. The net ionic equation is:
Ba2+ (aq) + SO4 2- (aq) → BaSO4 (s)
In this equation, the spectator ions are sodium (Na+) and chloride (Cl-).
4. To write the net ionic equation for the precipitation of nickel (II) sulfide (NiS), we need the balanced chemical equation. Without the starting reactants provided, we cannot determine the net ionic equation.