Aqueous soutions of magnesium chloride and silver nitrate are combined and a precipitate forms. A) Write the balanced molecular equation for this reaction. Be sure to include states on all chemical formulas. B) Write the balanced complete ionic equation for this reaction. Be sure to include states on all chemical formulas. C) Write the balanced net ionic equation for this reaction. Be sure to include states on all chemical formulas. D) Is this a redox reaction? Justify your answer.

Aqueous soutions of magnesium chloride and silver nitrate are combined and a precipitate forms. A) Write the balanced molecular equation for this reaction. Be sure to include states on all chemical formulas. B) Write the balanced complete ionic equation for this reaction. Be sure to include states on all chemical formulas. C) Write the balanced net ionic equation for this reaction. Be sure to include states on all chemical formulas. D) Is this a redox reaction? Justify your answer.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter5: Chemical Reactions

Section: Chapter Questions

Problem 5.32E

See similar textbooks

Similar questions

Classify the reactions represented by the following unbalanced equations by as many methods as possible. Balance the equations. msp;I4O9(s)I2O6(s)+I2(s)+O2(g) msp;Mg(s)+AgNO3(aq)Mg(NO3)2(aq)+Ag(s) msp;SiCl4(l)+Mg(s)MgCl2(s)+Si(s) msp;CuCl2(aq)+AgNO3(aq)Cu(NO3)2(aq)+AgCl(s) msp;Al(s)+Br2(l)AlBr3(s)
The element tin often occurs in nature as the oxide, SnO2 . To produce pure tin metal from this sort of tin ore, the ore usually is heated with coal (carbon). This produces pure molten tin, with the carbon being removed from the reaction system as the gaseous byproduct carbon monoxide. Write the unbalanced equation for this process.
The Solvay process is multistep industrial method for the manufacture of sodium carbonate, Na2CO3, which is also known as washing soda. Although most of the industrialized world utilizes the Solvay process for production of sodium carbonate, it is not manufactured in the United States because it can be obtained at lower cost from a large natural deposit in Wyoming. Questions 19 through 22 are based on reactions in that process. Sodium carbonate is used for many purposes, including glass manufacturing. How much NaCl is needed to react completely with 83.0g of ammonium hydrogen carbonate in NaCl+NH4HCO3NaHCO3+NH4Cl?
When hydrogen sulfide, H2S , gas is bubbled through a solution of lead(II) nitrate, Pb( NO3)2 , a black precipitate of lead(II) sulfide, PbS. forms, and nitric acid, HNO3 , is produced. Write the unbalanced chemical equation for this reaction.
Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acidbase, or oxidationreduction. msp;Fe(s)+H2SO4(aq)Fe3(SO4)2(aq)+H2(g) msp;HClO4(aq)+RbOH(aq)RbCIO4(aq)+H2O(l) msp;Ca(s)+O2(g)CaO(s) msp;H2SO4(aq)+NaOH(aq)Na2SO4(aq)+H2O(l) msp;Pb(NO3)2(aq)+Na2CO3(aq)PbCO3(s)+NaNO3(aq) msp;K2SO4(aq)+CaCl2(aq)KCl(aq)+CaSO4(s) msp;HNO3(aq)+KOH(aq)KNO3(aq)+H2O(l) msp;Ni(C2H3O2)2(aq)+Na2S(aq)NiS(s)+NaC2H3O2(aq) msp;Ni(s)+Cl2(g)NiCl2(s)
Apply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.
Using the general solubility rules given in Table 7.1, which of the following ions will form a precipitate with SO42? msp;Ba2+ msp;Na+ msp;NH4+ least two of the above ions will form a precipitate with SO42. l of the above ions will form a precipitate with SO42.