Write the complete ionic equation and the net ionic equation for the reaction below. The reaction does not need to be balanced. 1 point, for each compound, predicted and written correctly.1 point, one for each ion found in the complete ionic equation that is written correctly1 point for the correctly written net ionic equationPb(NO3)2(aq) + KI(aq) --->
Question
Write the complete ionic equation and the net ionic equation for the reaction below. The reaction does not need to be balanced. 1 point, for each compound, predicted and written correctly.1 point, one for each ion found in the complete ionic equation that is written correctly1 point for the correctly written net ionic equationPb(NO3)2(aq) + KI(aq) --->
Solution
The reaction between Pb(NO3)2 and KI can be written as follows:
Pb(NO3)2(aq) + 2KI(aq) --> PbI2(s) + 2KNO3(aq)
This is the molecular equation. Now, let's write the complete ionic equation. In this equation, all strong electrolytes (strong acids, strong bases, and soluble ionic salts) are dissociated into their ions.
Pb2+(aq) + 2NO3-(aq) + 2K+(aq) + 2I-(aq) --> PbI2(s) + 2K+(aq) + 2NO3-(aq)
This shows all of the particles as they exist in the solution. Now, we can cross out the spectator ions on both sides of the equation. Spectator ions are ions that do not participate in the reaction and remain in the solution. In this case, the spectator ions are K+ and NO3-.
After crossing out the spectator ions, we get the net ionic equation:
Pb2+(aq) + 2I-(aq) --> PbI2(s)
This equation only shows the ions that participate in the reaction.
Similar Questions
What is the net ionic equation for the reaction between Pb(NO3)2(aq) and KI(aq)? Pb+(aq) + I−(aq) → PbI(s) Pb2+(aq) + 2 I−(aq) → Pb(s) + I2(s) Pb2+(aq) + 2 I−(aq) → PbI2(s) K+(aq) + NO3−(aq) → KNO3(s) K+(aq) + NO3−(aq) → K(s) + NO(g) + O2(g)
Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.)Note: you are writing the molecular, and not the net ionic equation.→+NaClaqH2Ol
When a water solution of potassium hydroxide is added to a water solution of iron(III) nitrate, a precipitate of iron(III) hydroxide forms. What is the correctly balanced net ionic equation for the reaction?Group of answer choices3OH–(aq) + Fe3+(aq) → Fe(OH)3(s)K+(aq) + 3OH–(aq) + NO3–(aq) + Fe3+(aq) → K+(aq) + NO3–(aq) + Fe(OH)3(s)KOH(aq) + Fe(NO3)3(aq) → KNO3(aq) + Fe(OH)3(s)3K+(aq) + 3OH–(aq) + 3NO3–(aq) + Fe3+(aq) → 3K+(aq) + 3NO3–(aq) + Fe(OH)3(s)3KOH(aq) + Fe(NO3)3(aq) → 3KNO3(aq) + Fe(OH)3(s)
When a water solution of copper(II) sulfate is added to a water solution of sodium phosphate, a precipitate of copper(II) phosphate forms. What is the correctly balanced net ionic equation for the reaction?Group of answer choicesCuSO4(aq) + Na3PO4(aq) → Cu3(PO4)2(s) + Na2SO4(aq)3Cu2+(aq) + 2PO43–(aq) → Cu3(PO4)2(s)3Cu2+(aq) + 6Na+(aq) + 2PO43–(aq) + 3SO42–(aq) → Cu3(PO4)2(s) + 3SO42–(aq) + 6Na+(aq)3CuSO4(aq) + 2Na3PO4(aq) → Cu3(PO4)2(s) + 3Na2SO4(aq)Cu2+(aq) + PO42–(aq) → CuPO4(s)
Predict the reactants of this chemical reaction. That is, fill in the left side of the chemical equation. Be sure the equation you submit is balanced. (You can edit both sides of the equation to balance it, if you need to.)Note: you are writing the molecular, and not the net ionic equation.→+CaI2aqH2Ol
Upgrade your grade with Knowee
Get personalized homework help. Review tough concepts in more detail, or go deeper into your topic by exploring other relevant questions.