Question

In: Chemistry

Consider the following system composed of five 1 M aqueous solutions; iron (II) chloride, sodium sulfite,...

Consider the following system composed of five 1 M aqueous solutions; iron (II) chloride, sodium sulfite, sulfuric acid, silver nitrate, and sodium hydroxide.

Yoou will mix the solutions in a pair wise fashion so that all possible reactions between the solutions are tested. Use the solubility rules to predict when the precipitation reaction will occur. For each combination that produces a precipitation reaction write a balanced molecular equation and a net ionic equation. Indicate all phases in your equations.

The combination of sodium sulfite and sulfuric acid does not produce a precipitate but does produce a foul smelling gas, sulfur dioxide, and molecular water. Write a balanced molecular equation and a net ionic equation for the reaction. Indicate all phases in your equations.

One combination of chemical above does not produce a precipitate or a gas but you notice the test tube warms up significantly upon mixing. This is due to the high heat of neutralization. Identify the pair that produces a neutralization reaction and write a balanced molecular equation and a net ionic equation. Indicate all phases in your equations.

Solutions

Expert Solution

FeCl2(aq) + 2AgNO3(aq0 ----> Fe(NO3)2(aq0 +2 AgCl(s)

ionic equation
Fe+2(aq)+2Cl-(aq) + 2Ag+(aq)+2NO3-(aq) ----> Fe+2(aq)+2(NO3)-(aq)+2 AgCl(s)
removal of spectetor ions
net ionic equation
2Ag+(aq)+2Cl-(aq)----> 2AgCl(s)
FeCl2(aq) + 2NaOH(aq)----> Fe(OH)2(s) + 2NaCl(aq)
ionic equation
Fe+2(aq)+2Cl-(aq) + 2Na+(aq)+2OH-(aq)----> Fe(OH)2(s) + 2Na+(aq)+2Cl-(aq)
removal of spectetor ions
Fe+2(aq) + 2(OH)-(aq)----> Fe(OH)2(s) net ionic equation
2AgNO3(aq) + H2SO4(aq)---> Ag2SO4(s) + 2HNO3(aq)
ionic equation
2Ag+(aq)+2NO3-(aq) + 2H+(aq)+SO42-(aq)---> Ag2SO4(s) + 2H+(aq)+2NO3-(aq)
net ioni equation
2Ag+(aq) + So42-(aq) ----> Ag2SO4(s)
neutralisation reaction
H2SO4(aq) + 2NaOH(aq)---> Na2So4(aq)+ 2H2O(l)
Ionic equation
2H+(aq)+ SO42-(aq) + 2Na+(aq) + 2OH-(aq)----> 2Na+(aq) + SO42-(aq) + 2H2O(l)
removla of spectetor ions
2H+(aq) + 2OH-(aq)---> 2H2O(l)
FeCL2(aq) + Na2So3--->Fe(sO3)(s) + 2NaCl(aq)
ionic equation
Fe+2(aq)+2Cl-(aq) + 2Na+(aq)+So32-(aq)--->Fe(sO3)(s) + 2Na+(aq)+2Cl-(aq)
net ionic equation
Fe+2(aq) + SO32-(aq)--->FeSo3(s)
2AgNO3(aq) + Na2SO3(aq)--->Ag2SO3(s) + 2NaNO3(aq)
ionic equation
2Ag+(aq)+2NO3-(aq) + 2Na+(aq)+SO32-(aq)--->Ag2SO3(s) + 2Na+(aq)+2NO3-(aq)
net ionic equation
2Ag+(aq)+ So32-(aq)---->Ag2so3(s)

AgNO3(aq) + NaOH(aq)-----> AgOH(s)+ NaNO3(aq)

ionic equation

Ag+(aq)+NO3_(aq) + Na+(aq)+OH-(aq)-----> AgOH(s)+ Na+(aq)+NO3-(aq)

net ionic equation

Ag+(aq) + OH-(aq) -----> Ag(OH)(s)


Related Solutions

Suppose 6.88 g of iron(II) chloride is dissolved in 150. mL of a 0.30 M aqueous...
Suppose 6.88 g of iron(II) chloride is dissolved in 150. mL of a 0.30 M aqueous solution of silver nitrate. Calculate the final molarity of chloride anion in the solution. You can assume the volume of the solution doesn't change when the iron(II) chloride is dissolved in it. Be sure your answer has the correct number of significant digits.
Aqueous solutions sodium sulfate and copper (II) chloride were mixed together. The precipitate obtained during this...
Aqueous solutions sodium sulfate and copper (II) chloride were mixed together. The precipitate obtained during this reaction was dried and weighed to be 0.5665 g. How much copper (II) chloride in grams was used up during this reaction?
1.Consider the reaction when aqueous solutions of Chromium(II) iodide and sodium acetate are combined. The net...
1.Consider the reaction when aqueous solutions of Chromium(II) iodide and sodium acetate are combined. The net ionic equation for this reaction is 2.Consider the reaction when aqueous solutions of lead(II) acetate and manganese(II) iodide are combined. The net ionic equation for this is 3. Consider the reaction when aqueous solutions of lead(II) nitrate and manganese (II) bromide are combined. The net ionic equation for this is 4. Write the balanced net ionic equation for this reaction. Pb(NO3)2(aq)+MnI2(aq)->PbI2(s)+Mn(NO3)2(aq) 5. Write a...
What precipitate forms when aqueous soulutions of Potassium Chloride, Sodium Sulfide, Iron(II) Nitrate are simultaneously mixed?...
What precipitate forms when aqueous soulutions of Potassium Chloride, Sodium Sulfide, Iron(II) Nitrate are simultaneously mixed? Show the molecular and net ionic equation for the reaction.
l 2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of...
l 2. Determine the mole fraction of zinc(II) sulfite in a 4.22 M aqueous solution of zinc(II) sulfite. The density of the solution is 1.01 g mL-1.  answer is not 0.0699
Consider mixing an excess of lead(II) nitrate (aq) with 200.0 mL of 0.400 M sodium chloride....
Consider mixing an excess of lead(II) nitrate (aq) with 200.0 mL of 0.400 M sodium chloride. Determine the mass of solid formed, assuming a complete reaction What volume (in mL) of 0.800 M lead(II) nitrate must you add to make sure you make the mass of product you calculated in problem 3? A 0.1044 g sample of the salt MCl was dissolved in water (making it in the aqueous phase). An excess of AgNO3 (aq) was added, precipitating 0.0889 g...
Which of the following aqueous solutions are good buffer systems? . a. 0.15 M sodium hydroxide...
Which of the following aqueous solutions are good buffer systems? . a. 0.15 M sodium hydroxide + 0.29 M sodium bromide . b. 0.31 M hydrofluoric acid + 0.20 M potassium fluoride . c. 0.27 M nitric acid + 0.24 M potassium nitrate . d. 0.16 M hydrocyanic acid + 0.18 M potassium cyanide . e. 0.31 M ammonium nitrate + 0.30 M ammonia . b.How many moles of sodium hydroxide would have to be added to 250 mL of...
Which of the following aqueous solutions are good buffer systems? . 0.36 M sodium perchlorate +...
Which of the following aqueous solutions are good buffer systems? . 0.36 M sodium perchlorate + 0.28 M sodium chloride 0.11 M hypochlorous acid + 0.13 M sodium hypochlorite 0.29 M hydrobromic acid + 0.19 M potassium bromide 0.34 M ammonia + 0.32 M ammonium bromide 0.15 M potassium hydroxide + 0.25 M potassium bromide
1) For the following reaction, 50.6 grams of iron(II) chloride are allowed to react with 127...
1) For the following reaction, 50.6 grams of iron(II) chloride are allowed to react with 127 grams of silver nitrate . iron(II) chloride(aq) + silver nitrate(aq)  iron(II) nitrate(aq) + silver chloride(s) What is the maximum amount of iron(II) nitrate that can be formed?______ grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? ____ grams 2) For the following reaction, 21.7 grams of iron are allowed to react with 33.9...
1) For the following reaction, 50.6 grams of iron(II) chloride are allowed to react with 127...
1) For the following reaction, 50.6 grams of iron(II) chloride are allowed to react with 127 grams of silver nitrate . iron(II) chloride(aq) + silver nitrate(aq) iron(II) nitrate(aq) + silver chloride(s) What is the maximum amount of iron(II) nitrate that can be formed?_____________ grams What is the FORMULA for the limiting reagent? What amount of the excess reagent remains after the reaction is complete? _______________grams 2) For the following reaction, 21.7 grams of iron are allowed to react with 33.9...
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT