I would say that the best description of a reaction taking place is the net ionic equation.By definition, the net ionic equation keeps the spectator ions out. This means that all ions that don't actively take part in the reaction are not written down. Theoretically, they have no contribution to the reaction taking place, and so are not important to the description of the reaction.While the molecular will show us the geometries of the reactants, they will include the spectator ions in the structure, unless the net ionic equation was translated into molecular form, in which only the ions actively reacting are drawn. So, a molecular net ionic equation may be the best.
Write the balanced molecular equation, complete ionic equation, and net ionic equation.?
a. NH3(aq) + HNO3(aq) ---------> NH4NO3(aq) NH3(aq) + H3O+(aq) + NO3-(aq) --------> NH4+(aq) + NO3-(aq) + H2O(l) NH3(aq) + H3O+(aq) ---------> NH4+(aq) + H2O(l) b. Ba(OH)2(aq) + 2 HCl(aq) -------------> BaCl2(aq) + 2 H2O(l) Ba++(aq) + 2 OH-(aq) + 2 H3O+(aq) + 2Cl-(aq) ----> Ba++(aq) + 2Cl-(aq) + 4 H2O(l) OH-(aq) + H3O+(aq) ------------> 2 H2O(l) c. 3 HClO4(aq) + Fe(OH)3(s) -----------> Fe(ClO4)3 + 3 H2O(l) 3 H3O+(aq) + 3 ClO4-(aq) + Fe(OH)3(s) -----> Fe^+3(aq) + ClO4-(aq) + 6 H2O(l) 3 H3O+(aq) + Fe(OH)3(s) -----> Fe^+3(aq) + 6 H2O(l) d. AgOH(s) + HBr(aq) ------------> AgOH(s) + H2O(l) AgOH(s) + H3O+(aq) + Br-(aq) -----------> AgOH(s) + 2 H2O(l) AgOH(s) + H3O+(aq) + Br-(aq) -----------> AgOH(s) + 2 H2O(l)
Write the balanced molecular, complete ionic, and net ionic equations for each of the following acid-base reac?
a. HNO3(aq) + Al(OH)3(s) → molecular: 3HNO3 (aq) + Al(OH)3 (s) ---> Al(NO3)3 (s) + 3H2O (l) complete ionic: 3H+ (aq) + 3NO3- (aq) + Al(OH3) (s) ---> Al^3+ (aq) + 3NO3- (aq) + 3H2O (l) net ionic: 3H+(aq) + Al(OH)3 (s) ---> Al ^3+ (aq) + 3H2O (l) b. HC2H3O2(aq) + KOH(aq) → molecular : HC2H3O2 (aq) + KOH (aq) ---> KC2H3O2 (aq) + H2O (l) complete ionic: H+ (aq) + C2H3O2 - (aq) + K+ (aq) + OH- (aq) ---> K+ (aq) + C2H3O2- (aq) + H2O (l) net ionic: H+ (aq) + OH- (aq) ---> H2O (l) c. Ca(OH)2(aq) + HCl(aq) → molecular: Ca(OH)2 (aq) + 2HCL (aq)---> Ca(Cl)2 (aq) + 2H2O (l) complete ionic: Ca^2+ (aq) + 2OH - (aq) + 2H+ (aq) + 2Cl - (aq) ---> Ca^2+ (aq) + 2Cl - (aq) + 2H2O (l) net ionic: 2OH - (aq) + 2H+ (aq) ---> 2H2O (l)
Complete and balance the molecular, ionic, and net ionic equations for the following reactions?
1. molecular: NaHSO3(aq) + HBr(aq) --> NaBr(aq) + H2O(l) + SO2(g) ionic equation: Na^+(aq) + HSO3^-(aq) + H^+(aq) + Br^-(aq) --> Na^+(aq) + Br^-(aq) + H2O(l) + SO2(g) net ionic equation: HSO3^-(aq) + H^+(aq) + --> H2O(l) + SO2(g) 2. molecular: (NH4)2CO3(aq) + NaOH(aq) --> Na2CO3(aq) + 2 H2O(l) + 2 NH3(aq) ionic equation: 2 NH4^2(aq) + CO3^2-(aq) + 2 Na^+(aq) + 2 OH^-(aq) --> 2 Na^+(aq) + CO3^2-(aq) + 2 H2O(l) + 2 NH3(g) net ionic equation: 2 NH4^2(aq) + 2 OH^-(aq) --> 2 H2O(l) + 2 NH3(g) 3. molecular: (NH4)2CO3(aq) + Ba(OH)2(aq) --> BaCO3(s) + 2 H2O(l) + 2 NH3(g) ionic equation: 2 NH4^+(aq) + CO3^2-(aq) + Ba^2+(aq) + 2 OH^-(aq) --> BaCO3(s) + 2 H2O(l) + 2 NH3(g) net ionic equation: 2 NH4^+(aq) + CO3^2-(aq) + Ba^2+(aq) + 2 OH^-(aq) --> BaCO3(s) + 2 H2O(l) + 2 NH3(g) Note the last two equations are the same. Everything has changed between reactants and products. 4. molecular: FeS(s) + 2 HCl(aq) --> FeCl2(aq) + H2S(g) ionic equation: FeS(s) + 2 H^+(aq) + 2 Cl^-(aq) --> Fe^2+(aq) + 2 Cl^-(aq) + H2S(g) net ionic equation: FeS(s) + 2 H^+(aq) --> Fe^2+(aq) + H2S(g) Hope this helps you.
2NaCl + Pb(NO3)2 --> PbCl2 + 2NaCl2Na+(aq) + 2Cl-(aq) + Pb2+(aq) +2 NO3(aq) --> Pb2+Cl-2(s) + 2Na+(aq) + 2NO3-(aq)Pb2+(aq) + 2Cl-(aq) --> PbCl2(s)
Balanced complete ionic and net ionic equations?
H+(aq) + OH-(aq) = H2O(lq) + KI (aq) What you have written above is somewhat obscure: The best that I can identify is that you have provided part of an ionic equation: Start with the molecular equation with states: HI(aq) + KOH(aq) → H2O(l) + KI(aq) Now separate into ions, those species that can dissociate H+ (aq) + I-(aq) + K+(aq) + OH-(aq) →H2O(l) + K+(aq) + I-(aq) Now write the net ionic equation: inspect the above ionic equation and delete anything that is identical on both sides of the → sign Net Ionic Equation: H+(aq) + OH-(aq) → H2O(l) Write the molecular equation with states: Na2SO4 (aq) +CaI2 (aq) = CaSO4 (s) + 2NaI Write the full ionic equation as before: 2Na+(aq) + SO4 2- (aq) + Ca2+(aq) + 2I- (aq) → CaSO4(s) + 2Na+(aq) + 2I-(aq) Net ionic equation after canceling out identical ions: Ca2+(aq) + SO4 2- (aq) → CaSO4 (s) 2HC2H3O2 (aq) + Na2CO3(aq) = H2O(l) + CO2 (g) + 2NaC2H3O2 (aq) Full ionic equation: 2H+ (aq) + 2(C2H3O2) - (aq) + 2Na+(aq) + CO3 2-(aq) → H2O(l) + CO2(g) + 2Na+(aq) + 2(C2H3O2)-(aq) Again cancel out all identical ions Write the net ionic equation: 2H+(aq) + CO3 2-(aq) → H2O(l) + CO2(g) NH4Cl (aq) + NaOH (aq) = H2o (l) + NH3 (g) + NaCl (aq) Full ionic equation: NH4+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) → NH3(g) + Na+(aq) + Cl-(aq) + H2O(l) Write net ionic equation by canceling identical ions: NH4+(aq) + OH-(aq) → NH3(g) + H2O(l) In this last equation, there is some justification to write NH4OH(aq) as the product. I have not done this because it is doubtful that this actually exists as a compound, and secondly the ammonia as a gas is released from the solution ( you can easily smell it) especially if the solution is warmed. That is why I stick with showing NH3(g) being produced.
Write a balanced chemical, ionic, and net equation for the following...?
1. Nitric Acid: HNO3 Barium Hydroxide: Ba(OH)2 Here's the chemical equation when we combine the two HNO3 (aq) + Ba(OH)2 (aq) --> Ba(NO3)2 (aq) + H2O (l) Barium Nitrate is soluble in water and does not form a precipitate. Now let's balance the chemical equation... 2 HNO3 (aq) + Ba(OH)2 (aq) --> Ba(NO3)2 (aq) + 2 H2O (l) And break it into an ionic equation... 2 H+ (aq) + 2 NO3- (aq) + Ba(2+) (aq) + 2 OH- (aq) --> Ba(2+) (aq) + 2 NO3- (aq) + 2 H2O (l) And then cancel out the spectator ions, which are NO3- and Ba(2+)... 2 H+ (aq) + 2 OH- (aq) --> 2 H2O (l) H+ (aq) + OH- (aq) --> H2O (l) And that's the net ionic equation. 2. Sulfuric Acid: H2SO4 Sodium Hydroxide: NaOH H2SO4 (aq) + NaOH (aq) --> Na2SO4 (aq) + H2O (l) Balancing the chemical equation we find... H2SO4 (aq) + 2 NaOH (aq) --> Na2SO4 (aq) + 2 H2O (l) The complete ionic equation is... 2 H+ (aq) + SO4(2-) (aq) + 2 Na+ (aq) + 2 OH- (aq) --> 2 Na+ (aq) + SO4(2-) (aq) + 2 H2O (l) And the net ionic is... 2 H+ (aq) + 2 OH- (aq) --> 2 H2O (l) H+ (aq) + OH- (aq) --> H2O (l) And there you have it.
Write the balanced molecular, complete ionic, and net ionic equations?
a. NH3(aq) + HNO3(aq) ---------> NH4NO3(aq) NH3(aq) + H3O+(aq) + NO3-(aq) --------> NH4+(aq) + NO3-(aq) + H2O(l) NH3(aq) + H3O+(aq) ---------> NH4+(aq) + H2O(l) b. Ba(OH)2(aq) + 2 HCl(aq) -------------> BaCl2(aq) + 2 H2O(l) Ba++(aq) + 2 OH-(aq) + 2 H3O+(aq) + 2Cl-(aq) ----> Ba++(aq) + 2Cl-(aq) + 4 H2O(l) OH-(aq) + H3O+(aq) ------------> 2 H2O(l) c. 3 HClO4(aq) + Fe(OH)3(s) -----------> Fe(ClO4)3 + 3 H2O(l) 3 H3O+(aq) + 3 ClO4-(aq) + Fe(OH)3(s) -----> Fe^+3(aq) + ClO4-(aq) + 6 H2O(l) 3 H3O+(aq) + Fe(OH)3(s) -----> Fe^+3(aq) + 6 H2O(l) d. AgOH(s) + HBr(aq) ------------> AgOH(s) + H2O(l) AgOH(s) + H3O+(aq) + Br-(aq) -----------> AgOH(s) + 2 H2O(l) AgOH(s) + H3O+(aq) + Br-(aq) -----------> AgOH(s) + 2 H2O(l)
Your complete ionic equation includes all ions in solution, including spectator ions. Your net ionic equation leaves out spectator ions and focuses on what changes in the reaction.For example:Full equation:NaOH(aq) + HCl(aq) →NaCl(aq) + H2O(l)Complete Ionic Equation:Na+(aq) + OH-(aq) + H+(aq) + Cl-(aq) →Na+(aq) + Cl-(aq) + H2O(l)**Remember: water is not ionic, it is a covalent compound so it is written like this**Net Ionic Equation:H+(aq) + OH-(aq) → H2O(l)I leave out sodium and chloride ions because they are irrelevant in the reaction and are called spectator ions.