1. Na2CO3(aq) + Ni(NO3)2(aq) 2. NaCl(aq) + AgNO3(aq) 3. Na2CO3(aq) + HCl(aq) Select Select precipitate gas...
Write Balanced Ionic Equations and Balanced Net Ionic Equations for the following combinations (including states ex.(s) or (aq)): BaCl2 and AgNO3, KBr and AgNO3, K2CrO4 and AgNO3, NaOH and AgNO3, Na2CO3 and BaCl2, (NH4)2SO4 and BaCl2, Pb(NO3)2 and Na2CO3, Zn(NO3)2 and Na2CO3, FeCl3 and Na2CO3, Cu(NO3)2 and Na2CO3, K2CrO4 and Pb(NO3)2, NaOH and Pb(NO3)2, NaOH and FeCl3, NaCH3COO and FeCl3, MgCl2 and NaOH, Cu(NO3)2 and NaOH.
please help fill these out Al(s) + CuCl(aq) - Cu(s) + AgNO,(aq) + Double replacement reactions 9. Test tube number 1. NaCl(aq) +_ KNO3(aq) - NaCl(aq) + _ AgNO3(aq) - Na2CO3(aq) +_ _ HCl(aq) - NaOH(aq) + HCl(aq) - BaCl2(aq) + H2SO (aq) Pb(NO3)2(aq) + __KCrO (aq) + Fe(NO3)3(aq) +_ NaOH(aq) - 8. Cu(NO3)2(aq) +_ _NaOH(aq) --
5. Which combination will produce a precipitate? a) NH4OH(aq) and HCl(aq) b) AgNO3(aq) and CaCl2(aq) c) NaOH(aq) and HCl(aq) d) NaCl(aq) and H2SO4(aq)
Which of the following reactions will not form a precipitate? A) K2C2O4(aq)+Ba(OH)2(aq)→ B) Pb(NO3)2(aq)+H2SO4(aq)→ C) CaCO3(s)+H2SO4(aq)→ incorrect D) AgNO3(aq)+NaI(aq)→ E) Na2CO3(aq)+HCl(aq)→
Double Displacement -- Complete and balance the following reactions 1. AgNO3 (aq) + HCl (aq) ---------------> 2. Cu(NO3)2 (aq) + NaOH (aq) ---------> 3. Fe(NO3)3 (aq) + Cd(OH)2 (aq) -------> 4. Pb(NO3)2 (aq) + H2SO4 (aq) ----------> 5. Hg2(NO3)2 (aq) + Na2CO3 (aq) ------->
Unbalanced Equations AgNO3 + NaCl -- AgCl + NaNO3 Ca(NO3)2 + Na2CO3 -- Caco; +NaNO3 Pb(NO3)2 +K Cro, PbCrO, KNO, FeCl3 + NaOH -- Fe(OH)3 + NaCl FeCl2 + Nas -- Fes + NaCl Initial Mass of NaCl og 20 g 40 g 60g Add AgNO3 Add 1 g Add 10 8 Total Mass of AgNO3 added: 0g Reset Experiment AgNO; NaCl AgCl NaNO; 0.08 0.0 g 0.0 g 0.0 g Redo the experiment by clicking on Reset Experiment. Add...
For each combination of reagents, write a balanced molecular equation. Indicate whether a reaction occurred in each case. If no reaction occurred, indicate "NR" for 'no reaction.' For reactions that did occur, write the net ionic equation for each. Classify each reaction that occurred as acid/base, redox, or a precipitation reaction. CuSO4 and NaNO3 aq (NR) CuSO4 and NaCl aq (NR) Na3PO4 and Pb(OAc)2 aq (rxn) Na2CO3 and CaCl2 aq (rxn) Na2CO3 and HCl aq (NR) HCl and NaOH (aq)...
Need the total ionic equation and net ionic equation and the driving forces of these equations. UL TULI PILIPILULLS. ILS I When H2CO3 is formed it decomposes: H2CO3(aq) - H2O(1) 00 +SO21. Here, the arrow is used instead of (g): both mean that the substance 10 H2SO3(aq) + H2O(l) + S02f. Here, the an is a gas. Table 2. Equations for Double Replacement Reactions Equations Driving Force Tolal sonic Equahon 1. NaCl(aq) + AgNO3(aq) → TIE: NIE: Pet Sonic- Equation...
What are the identities of the precipitate in each of the following reactions: A) AgNO3 (aq) + KI (aq) ------> Ag (s) + KNO3 (aq) B) Pb(NO3)2 (aq) + 2KI (aq) ------> PbI2 (s) + 2KNO3 (aq) C) Na3PO4 (aq) + 3Ca(NO3)2 (aq) ------> Ca3(PO4)2 (s) + 6NaNO3 (g) D) MgSO4 (aq) + BaCl2 (aq) ------> BaSO4 (s) + MgCl2 (aq) E) COCl2 (aq) + Ca(OH)2 (aq) ------> CaCl2 (aq) + Co(OH)2 (s)
Part C. Solubility reactions Table 1 Precipitate Reactants Observation Net Ionic Equation AgNO3 + NaCl Ag+(aq) + Cl-(aq) → AgI N/A Solution KNOs +NaC remained clear No reactiorn Cu(NO3)2 +NaOH Ba(NO3)2+ NaOH Ba(NO3)2 + Na2SO4 color) Cas(PO4)2 Ca(NO3)2 +Na2CO3 CuCO3