3: Chemical Reactions

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Balancing Combustion Reactions

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of propane C₃H₈.

a. \(\ce{C3H8 + O2 -> CO2 + H2O}\)

b. \(\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}\)

c. \(\ce{CO2 + H2O -> C3H8 + O2}\)

d. \(\ce{2C3H8 + 8O2 -> 6CO2 + 5H2O}\)

Answer: b. \(\ce{C3H8 + 5O2 -> 3CO2 + 4H2O}\)

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of butane C₄H₁₀

a. \(\ce{C4H10 + O2 -> 4CO2 + 5H2O}\)

b. \(\ce{C4H10 + 5O2 -> 4CO2 + 5H2O}\)

c. \(\ce{C4H10 + 7O2 -> 5CO2 + 8H2O}\)

d. \(\ce{2C4H10 + 13O2 -> 8CO2 + 10H2O}\)

Answer: d. \(\ce{2C4H10 + 13O2 -> 8CO2 + 10H2O}\)

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of hydrogen.

a. \(\ce{H2 + O2 -> H2O}\)

b. \(\ce{H2 + O -> H2O}\)

c. \(\ce{2H2 + O2 -> 2H2O}\)

d. There is no carbon so this does not combust.

Answer: c. \(\ce{2H2 + O2 -> 2H2O}\)

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of magnesium.

a. \(\ce{Mg + O -> MgO}\)

b. \(\ce{Mg + O2 -> MgO2}\)

c. \(\ce{2Mg + O2 -> 2MgO}\)

d. Magnesium will not combust.

Answer: c. \(\ce{2Mg + O2 -> 2MgO}\)

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of ethanol (CH₃CH₂OH - drinking alcohol).

a. \(\ce{CH3CH2OH + 3O2 -> 2CO2 + 3H2O}\)

b. \(\ce{2CH3CH2OH + 13O2 -> 4CO2 + 6H2O}\)

c. \(\ce{CH3CH2OH + O2 -> CO2 + H2O}\)

d. \(\ce{3CH3CH2OH + 9O2 -> 6CO2 + 12H2O}\)

Answer: c. \(\ce{CH3CH2OH + 3O2 -> 2CO2 + 3H2O}\)

Exercise \(\PageIndex{1}\)

Balance the equation for the combustion of isopropyl alcohol - (CH₃)₂CHOH - rubbing alcohol.

a. \(\ce{(CH3)2CHOH + O2 -> 2CO2 + 3H2O}\)

b. \(\ce{2(CH3)2CHOH + 9O2 -> 6CO2 + 8H2O}\)

c. \(\ce{CH3CH2OH + O2 -> 2CO2 + 3H2O}\)

d. \(\ce{3CH3CH2OH + 4O2 -> 3CO2 + 2H2O}\)

Answer: b. \(\ce{2(CH3)2CHOH + 9O2 -> 6CO2 + 8H2O}\)

Balancing Equations - Double Displacement Reactions

Exercise \(\PageIndex{1}\)

Potassium carbonate reacts with lead(II) nitrate to form lead(II) carbonate and potassium nitrate. What is the stoichiometric coefficient in front of the lead(II) nitrate for the balanced equation?

a. 1

b. 2

c. 3

d. 4

Answer: a. 1

Exercise \(\PageIndex{1}\)

Aluminum chloride reacts with silver sulfate to form aluminum sulfate and silver chloride. What is the stoichiometric coefficient in front of the silver chloride for the balanced equation?

a. 2

b. 3

c. 4

d. 6

Answer: d. 6

Exercise \(\PageIndex{1}\)

Manganese(II)sulfate reacts with sodium phosphate to produce manganese(II)phosphate and sodium sulfate. What is the stoichiometric coefficient in front of the sodium sulfate for the balanced equation?

a. 1

b. 2

c. 3

d. 4

Answer: c. 3

Exercise \(\PageIndex{1}\)

Sulfuric Acid reacts with Ammonium hydroxide to produce Ammonium sulfate and water. What is the stoichiometric coefficient in front of the water for the balanced equation?

a. 1

b. 2

c. 3

d. 4

Answer: b. 2

Exercise \(\PageIndex{1}\)

Iron(III)chloride reacts with lead(IV)sulfate to produce Iron(III)sulfate and lead(IV)chloride. What is the stoichiometric coefficient in front of the Iron(III)chloride for the balanced equation?

a. 1

b. 2

c. 3

d. 4

Answer: d. 4

Acid Base Neutralization Reactions

Exercise \(\PageIndex{1}\)

Write the general (molecular) equation for the reaction between potassium hydroxide and perchloric acid.

a. \(\ce{KOH(aq) + HClO4(aq) -> KClO4(aq) + H2O(aq)}\)

b. \(\ce{KOH(aq) + HClO4(aq) -> KClO4(aq) + H2O(l)}\)

c. \(\ce{KOH(aq) + HClO4(aq) -> KClO3(aq) + H2O(l)}\)

d. NOTA

Answer: b. \(\ce{KOH(aq) + HClO4(aq) -> KClO4(aq) + H2O(l)}\)

Exercise \(\PageIndex{1}\)

Write the ionic equation for the reaction between potassium hydroxide and perchloric acid.

a. H+ + OH- \(\ce{->}\) H2O(l)

b. H+ + ClO4- + K+ + OH- --> K+ + ClO4- + H2O(l)

c. H+ + Cl- + K+ + OH- --> K+ + Cl- + H2O(l)

d. NOTA

Answer: b. H⁺ + ClO₄^- + K⁺ + OH^- --> K⁺ + ClO₄^- + H₂O(l)

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reaction between potassium hydroxide and perchloric acid.

a. H⁺ + OH^- --> H₂O(l)

b. H⁺ + ClO₄^- + K⁺ + OH^- --> K⁺ + ClO₄^- + H₂O(l)

c. H⁺ + Cl^- + K⁺ + OH^- --> K⁺ + Cl^- + H₂O(l)

d. NOTA

Answer: a. H⁺ + OH^- --> H₂O(l)

Exercise \(\PageIndex{1}\)

Write the general (molecular) equation for the reacton of ammonia with perchloric acid.

a. \(\ce{NH3(aq) + HClO4(aq) -> NH4ClO4(aq)}\)

b. \(\ce{NH3OH(aq) + HClO4(aq) -> NH4ClO4(aq) + H2O(l)}\)

c. \(\ce{NH3OH(aq) + HClO4(aq) -> NH4ClO4(aq) + H2O(aq)}\)

d. NOTA

Answer: a. \(\ce{NH3(aq) + HClO4(aq) -> NH4ClO4(aq)}\)

Exercise \(\PageIndex{1}\)

Write the ionic equation for the reacton of ammonia with perchloric acid.

a. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^- + H₂O(l)

b. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^- + H₂O(aq)

c. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^-

d. NOTA

Answer: c. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^-

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reacton of ammonia with perchloric acid.

a. NH₃(aq) + H⁺ --> NH₄⁺

b. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^-

c. NH₃(aq) + H⁺ + ClO₄^- --> NH₄⁺ + ClO₄^- + H₂O

d. NOTA

Answer: a. NH₃(aq) + H⁺ --> NH₄⁺

Exercise \(\PageIndex{1}\)

Write the general (molecular) equation for the reaction between potassium hydroxide and hypochlorous acid.

a. \(\ce{KOH(aq) + HClO(aq) -> KClO(s) + H2O(l)}\)

b. \(\ce{KOH(aq) + HClO(aq) -> KClO(aq) + H2O(aq)}\)

c. \(\ce{KOH(aq) + HClO(aq) -> KClO(aq) + H2O(l)}\)

d. NOTA

Answer: c. \(\ce{KOH(aq) + HClO(aq) -> KClO(aq) + H2O(l)}\)

Exercise \(\PageIndex{1}\)

Write the ionic equation for the reaction between potassium hydroxide and hypochlorous acid.

a. K⁺ + OH^- + HClO(aq) --> K⁺ + ClO^- + H₂O(l)

b. OH^- + HClO(aq) --> ClO^- + H₂O(l)

c. K⁺ + OH^- + HClO(aq) --> K⁺ + ClO^-

d. NOTA

Answer: a. K⁺ + OH^- + HClO(aq) --> K⁺ + ClO^- + H₂O(l)

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reaction between potassium hydroxide and hypochlorous acid.

a. H⁺ + OH^- --> H₂O(l)

b. K⁺ + OH^- + HClO(aq) --> K⁺ + ClO^- + H₂O(l)

c. OH^- + HClO(aq) --> + ClO^- + H₂O(l)

d. NOTA

Answer: c. OH^- + HClO(aq) --> + ClO^- + H₂O(l)

Exercise \(\PageIndex{1}\)

Write the general (molecular) equation for the reaction between ammonia and hypochlorous acid

a. \(\ce{NH3(aq) + HClO(aq) -> NH4ClO(a)}\)

b. \(\ce{NH3(aq) + HClO(aq) -> NH4ClO(aq)}\)

c. \(\ce{NH3(aq) + HClO(aq) -> NH4ClO(aq) + H2O}\)

d. NOTA

Answer: b. \(\ce{NH3(aq) + HClO(aq) -> NH4ClO(aq)}\)

Exercise \(\PageIndex{1}\)

Write the ionic equation for the reaction between ammonia and hypochlorous acid

a. NH₃(aq) + HClO(aq) --> NH₄ClO(aq)

b. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^-

c. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^- + H₂O

d. NOTA

Answer: b. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^-

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reaction between ammonia and hypochlorous acid

a. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^-

b. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^- + H₂O

c. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^- + H₂O

d. NOTA

Answer: a. NH₃(aq) + HClO(aq) --> NH₄⁺ + ClO^-

Exercise \(\PageIndex{1}\)

Write the general (molecular) equation for the reaction of barium hydroxide with sulfuric acid

a. \(\ce{Ba(OH)2(aq) + H2SO4(aq) -> BaSO4(s) + H2O(l)}\)

b. \(\ce{Ba(OH)2(aq) + H2SO4(aq) -> BaSO4(s) + 2H2O(l)}\)

c. \(\ce{Ba(OH)2(aq) + H2SO4(aq) -> BaSO4(aq) + 2H2O(l)}\)

d. NOTA

Answer: b. \(\ce{Ba(OH)2(aq) + H2SO4(aq) -> BaSO4(s) + 2H2O(l)}\)

Exercise \(\PageIndex{1}\)

Write the ionic equation for the reaction of barium hydroxide with sulfuric acid

a. H⁺ + OH^- --> H₂O(l)

b. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> Ba + SO₄^-2 + 2H₂O(l)

c. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> BaSO₄(s) + 2H₂O(l)

d. NOTA

Answer: c. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> BaSO₄(s) + 2H₂O(l)

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reaction of barium hydroxide with sulfuric acid

a. H⁺ + OH^- --> H₂O(l)

b. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> Ba + SO₄^-2 + 2H₂O(l)

c. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> BaSO₄(s) + 2H₂O(l)

d. NOTA

Answer: c. Ba⁺² + 2OH^- + 2H⁺ +SO₄^-2 --> BaSO₄(s) + 2H₂O(l)

Solubility

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{Na2S(aq) + CuCl2(aq) -> }\)

a. \(\ce{Na2S(aq) + CuCl2(aq) -> CuS(s) + 2NaCl(aq)}\)

b. \(\ce{Na2S(aq) + CuCl2(aq) -> CuS(aq) + 2NaCl(s)}\)

c. \(\ce{Na2S(aq) + CuCl2(aq) -> CuS(s) + NaCl(aq)}\)

d. NOTA

Answer: a. \(\ce{Na2S(aq) + CuCl2(aq) -> CuS(s) + 2NaCl(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{(NH4)2CO3(aq) + Zn(NO3)2(aq) -> }\)

a. \(\ce{(NH4)2CO3(aq) + Zn(NO3)2(aq) -> NH4(NO3)2(aq) + 2ZnCO3 (s)}\)

b. \(\ce{(NH4)2CO3(aq) + Zn(NO3)2(aq) -> 2NH4NO3(aq) + ZnCO3 (s)}\)

c. \(\ce{(NH4)2CO3(aq) + Zn(NO3)2(aq) -> 2NH4NO3(s) + ZnCO3 (aq)}\)

d. NOTA

Answer: b. \(\ce{(NH4)2CO3(aq) + Zn(NO3)2(aq) -> 2NH4NO3(aq) + ZnCO3 (s)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{LiPO4(aq) + AgNO3(aq) -> }\)

a. \(\ce{LiPO4(aq) + 3AgNO3(aq) -> Ag3PO4(aq) +3LiNO3(s)}\)

b. \(\ce{LiPO4(aq) + AgNO3(aq) -> Ag3PO4(aq) +LiNO3(s)}\)

c. \(\ce{LiPO4(aq) + 3AgNO3(aq) -> Ag3PO4(s) +3LiNO3(aq)}\)

d. NOTA

Answer: c. \(\ce{LiPO4(aq) + 3AgNO3(aq) -> Ag3PO4(s) +3LiNO3(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{(NH4)2SO4(aq) + NaI(aq) -> }\)

a. \(\ce{(NH4)2SO4(aq) + NaI(aq) -> Na2SO4(s) + 2NH4I(aq)}\)

b. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(aq) + 2NH4I(aq)}\)

c. \(\ce{(NH4)2SO4(aq) + NaI(aq) -> Na2SO4(aq) + 2NH4I(s)}\)

d. NOTA

Answer: b. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(aq) + 2NH4I(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{H2SO4(aq) + BaBr2(aq) -> }\)

a. \(\ce{H2SO4(aq) + BaBr2(aq) -> 2HBr(s) + BaSO4(aq)}\)

b. \(\ce{H2SO4(aq) + BaBr2(aq) -> 2HBr(aq) + BaSO4(aq)}\)

c. \(\ce{H2SO4(aq) + BaBr2(aq) -> 2HBr(aq) + BaSO4(s)}\)

d. NOTA

Answer: c. \(\ce{H2SO4(aq) + BaBr2(aq) -> 2HBr(aq) + BaSO4(s)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{BiCl3(aq) + NaOH(aq) -> }\)

a. \(\ce{BiCl3(aq) + 3NaOH(aq) -> Bi(OH)3(s) + 3NaCl(aq)}\)

b. \(\ce{BiCl3(aq) + 3NaOH(aq) -> Bi(OH)3(aq) + 3NaCl(aq)}\)

c. \(\ce{BiCl3(aq) + 3NaOH(aq) -> Bi(OH)3(aq) + 3NaCl(s)}\)

d. NOTA

Answer: a. \(\ce{BiCl3(aq) + 3NaOH(aq) -> Bi(OH)3(s) + 3NaCl(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{K2S(aq) + CaCl2(aq) -> }\)

a. \(\ce{K2S(aq) + CaCl2(aq) -> CaS(aq) + 2KCl(s)}\)

b. \(\ce{K2S(aq) + CaCl2(aq) -> CaS(s) + 2KCl(aq)}\)

c. \(\ce{K2S(aq) + CaCl2(aq) -> CaS(aq) + 2KCl(aq)}\)

d. NOTA

Answer: b. \(\ce{K2S(aq) + CaCl2(aq) -> CaS(s) + 2KCl(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{NaOH(aq) + H2C2O4(aq) -> }\)

a. \(\ce{2NaOH(aq) + H2C2O4(aq) -> Na2C2O4(aq) + 2H2O}\)

b. \(\ce{2NaOH(aq) + H2C2O4(aq) -> Na2C2O4(s) + 2H2O}\)

c. \(\ce{2NaOH(aq) + H2C2O4(aq) -> 2Na2C2O4(aq) + 2H2O}\)

d. NOTA

Answer: a. \(\ce{2NaOH(aq) + H2C2O4(aq) -> Na2C2O4(aq) + 2H2O}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{HCl(aq) + KC2H3O2(aq) -> }\)

a. \(\ce{HCl(aq) + KC2H3O2(aq) -> KCl(s) + HC2H3O2(aq)}\)

b. \(\ce{HCl(aq) + KC2H3O2(aq) -> KCl(aq) + HC2H3O2(s)}\)

c. \(\ce{HCl(aq) + KC2H3O2(aq) -> KCl(aq) + HC2H3O2(aq)}\)

d. NOTA

Answer: c. \(\ce{HCl(aq) + KC2H3O2(aq) -> KCl(aq) + HC2H3O2(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{KOH(aq) + FeBr3(aq) -> }\)

a. \(\ce{3KOH(aq) + FeBr3(aq) -> 3KBr(aq) + Fe(OH)3(aq)}\)

b. \(\ce{3KOH(aq) + FeBr3(aq) -> 3KBr(aq) + Fe(OH)3(s)}\)

c. \(\ce{3KOH(aq) + FeBr3(aq) -> 3KBr(s) + Fe(OH)3(aq)}\)

d. NOTA

Answer: b. \(\ce{3KOH(aq) + FeBr3(aq) -> 3KBr(aq) + Fe(OH)3(s)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{(NH4)2SO4(aq) + NaI(aq) -> }\)

a. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(s) + 2NH4I(aq)}\)

b. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(aq) + 2NH4I(s)}\)

c. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(aq) + 2NH4I(aq)}\)

d. NOTA

Answer: c. \(\ce{(NH4)2SO4(aq) + 2NaI(aq) -> Na2SO4(aq) + 2NH4I(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{Be(NO3)2(aq) + KOH(aq) -> }\)

a. \(\ce{Be(NO3)2(aq) + 2KOH(aq) -> 2KNO3(s) + Be(OH)2(aq)}\)

b. \(\ce{Be(NO3)2(aq) + 2KOH(aq) -> 2KNO3(aq) + Be(OH)2(s)}\)

c. \(\ce{Be(NO3)2(aq) + 2KOH(aq) -> 2KNO3(aq) + Be(OH)2(aq)}\)

d. NOTA

Answer: b. \(\ce{Be(NO3)2(aq) + 2KOH(aq) -> 2KNO3(aq) + Be(OH)2(s)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{Zn(C2H3O2)2(aq) + KNO3(aq) -> }\)

a. \(\ce{Zn(C2H3O2)2(aq) + 2KNO3(aq) -> Zn(NO3)2(aq) + 2KC2H3O2(aq)}\)

b. \(\ce{Zn(C2H3O2)2(aq) + 2KNO3(aq) -> Zn(NO3)2(s) + 2KC2H3O2(aq)}\)

c. \(\ce{Zn(C2H3O2)2(aq) + 2KNO3(aq) -> Zn(NO3)2(aq) + 2KC2H3O2(s)}\)

d. NOTA

Answer: a. \(\ce{Zn(C2H3O2)2(aq) + 2KNO3(aq) -> Zn(NO3)2(aq) + 2KC2H3O2(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{Na2SO4(aq) + HNO3(aq) -> }\)

a. \(\ce{Na2SO4(aq) + 2HNO3(aq) -> 2NaNO3(s) + H2SO4(aq)}\)

b. \(\ce{Na2SO4(aq) + 2HNO3(aq) -> 2NaNO3(aq) + H2SO4(s)}\)

c. \(\ce{Na2SO4(aq) + 2HNO3(aq) -> 2NaNO3(aq) + H2SO4(aq)}\)

d. NOTA

Answer: c. \(\ce{Na2SO4(aq) + 2HNO3(aq) -> 2NaNO3(aq) + H2SO4(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{CoSO4(aq) + Pb(NO3)2(aq) -> }\)

a. \(\ce{CoSO4(aq) + Pb(NO3)2(aq) -> PbSO4(aq) + Co(NO3)2(aq)}\)

b. \(\ce{CoSO4(aq) + Pb(NO3)2(aq) -> PbSO4(s) + Co(NO3)2(aq)}\)

c. \(\ce{CoSO4(aq) + Pb(NO3)2(aq) -> PbSO4(aq) + Co(NO3)2(s)}\)

d. NOTA

Answer: b. \(\ce{CoSO4(aq) + Pb(NO3)2(aq) -> PbSO4(s) + Co(NO3)2(aq)}\)

Exercise \(\PageIndex{1}\)

Predict the products and balance the following reaction. Indicate if the products are in the aqueous or solid phases.

\(\ce{Na2CO3(aq) + CaCl2(aq) -> }\)

a. \(\ce{Na2CO3(aq) + CaCl2(aq) -> CaCO3(s) + 2NaCl(aq)}\)

b. \(\ce{Na2CO3(aq) + CaCl2(aq) -> CaCO3(aq) + 2NaCl(aq)}\)

c. \(\ce{Na2CO3(aq) + CaCl2(aq) -> CaCO3(aq) + 2NaCl(s)}\)

d. NOTA

Answer: a. \(\ce{Na2CO3(aq) + CaCl2(aq) -> CaCO3(s) + 2NaCl(aq)}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of Na₂CO₃, NaI, and Na₂SO₄?

a. \(\ce{Na2SO4}\)

b. \(\ce{Na2CO3}\)

c. \(\ce{NaI}\)

d. NOTA

Answer: d. NOTA

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of AgNO₃, (NH₄)₂CO₃, and K₂SO₄?

a. \(\ce{Ag2SO4}\)

b. \(\ce{KNO3}\)

c. \(\ce{Ag2CO3}\)

d. NOTA

Answer: c. \(\ce{Ag2CO3}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of AgClO₄, BaI₂, and Pb(NO₃)₂?

a. \(\ce{AgI}\) and \(\ce{Ba(CLO4)2}\)

b. \(\ce{PbI}\) and \(\ce{AgI}\)

c. \(\ce{PbI}\) and \(\ce{BaNO3}\)

d. NOTA

Answer: b. \(\ce{PbI}\) and \(\ce{AgI}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of CoSO₄, Na₂S, and K₂CO₃?

a. \(\ce{Na2CO3}\), \(\ce{Na2SO4}\) and \(\ce{K2SO4}\)

b. \(\ce{CoS}\), \(\ce{Na2SO4}\) and \(\ce{K2S}\)

c. \(\ce{CoS}\) and \(\ce{CoCO3}\)

d. NOTA

Answer: c. \(\ce{CoS}\) and \(\ce{CoCO3}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of H₃PO₄, NaOH, and CaCO₃?

a. \(\ce{Ca3(PO4)2}\)

b. \(\ce{CaOH}\)

c. \(\ce{Na3PO4}\)

d. NOTA

Answer: a. \(\ce{Ca3(PO4)2}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of Na₂S, (NH₄)₂CO₃, and AgNO₃?

a. \(\ce{NaCO3}\) and \(\ce{Ag2CO3}\)

b. \(\ce{Ag2S}\) and \(\ce{Ag2CO3}\)

c. \(\ce{Ag2S}\) and \(\ce{(NH4)2S}\)

d. NOTA

Answer: b. \(\ce{Ag2S}\) and \(\ce{Ag2CO3}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of KC₂H₃O₂, H₂SO₄, and Mg(OH)₂?

a. \(\ce{K2SO4}\)

b. \(\ce{MgC2H3O2}\)

c. \(\ce{MgSO4}\)

d. NOTA

Answer: d. NOTA

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of H₃PO₄, CaBr₂, and Mg(NO₃)₂?

a. \(\ce{Ca(PO4)2}\) and \(\ce{Ca(NO3)2}\)

b. \(\ce{Mg3(PO4)2}\) and \(\ce{MgBr2}\)

c. \(\ce{Mg3(PO4)2}\) and \(\ce{Ca3(PO4)2}\)

d. NOTA

Answer: c. \(\ce{Mg3(PO4)2}\) and \(\ce{Ca3(PO4)2}\)

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of LiClO₄, Ba₂S, and NaOH?

a. \(\ce{BaOH}\)

b. \(\ce{Li2S}\)

c. \(\ce{NaClO4}\)

d. NOTA

Answer: d. NOTA

Exercise \(\PageIndex{1}\)

What solids if any would precipitate from a mixture of H₂S, MgSO₄, and CaCl₂?

a. \(\ce{MgS}\)

b. \(\ce{CaS}\)

c. \(\ce{MgCl2}\)

d. NOTA

Answer: a. \(\ce{MgS}\)

Solutions

All the questions in this section deal with the following solutions:

Solution A: 40.0 mL of 0.500 M AlCl₃
Solution B: 60.0 mL of 1.000 M Ag₂SO₄

Treat the solubilities of these solutions as would be determined from the solubility rules in the text. In reality, things are more complicated, as silver forms a AgCl₂^- ion in high chloride concentrations, which causes the precipitate to redissolve, giving lower yields than predicted. Also, in reality, Silver sulfate is a weak electrolyte and will not form a 1M solution, but we will treat it as a strong electrolyte, in accordance with our solubility rules. This is an important concept to understand, that is, these solubility rules are a simplification of things. During the second semester of this course we will introduce the more advanced concept of Solubility Constants, which will allow us to deal rigorously with the actual concentrations of ionic compounds in aqueous solutions.

Exercise \(\PageIndex{1}\)

What are the respective aluminum and chloride concentrations in solution A?

a. 1.0 M, 1.5M

b. 0.5M, 0.5M

c. 0.5M, 1.5M

d. Not enough information

Answer: c. 0.5M, 1.5M

Exercise \(\PageIndex{1}\)

What are the respective silver and sulfate ion concentrations in solution B?

a. 1.000M, 1.000M

b. 2.000M, 4.000M

c. 2.000M, 1.000M

d. Not enough information

Answer: c. 2.000M, 1.000M

Exercise \(\PageIndex{1}\)

Identify any precipitates which would form if the two solutions were mixed.

a. aluminum sulfate

b. silver chloride

c. aluminum sulfate and silver chloride

d. Not enough information

Answer: b. silver chloride

Exercise \(\PageIndex{1}\)

Identify any spectator ions which would result if the two solutions were mixed.

a. aluminum and chloride

b. silver and sulfate

c. aluminum and sulfate

d. silver and chloride

Answer: c. aluminum and sulfate

Exercise \(\PageIndex{1}\)

Write the balanced general (molecular equation) for the reaction which would occur if the two solutions were mixed.

a. Al⁺³ + Cl^- + Ag⁺ + SO₄^-2 --> Al⁺³ + SO₄^-2 + AgCl(s)

b. 2Al⁺³ + 2Cl^- + 3Ag⁺ + 3SO₄^-2 --> Al⁺³ + SO₄^-2 + 6AgCl(s)

c. 2Al⁺³ + 6Cl^- + 6Ag⁺ + 3SO₄^-2 --> 2 Al⁺³ + 3SO₄^-2 + 6AgCl(s)

d. none of these

Answer: c. 2Al⁺³ + 6Cl^- + 6Ag⁺ + 3SO₄^-2 --> 2 Al⁺³ + 3SO₄^-2 + 6AgCl(s)

Exercise \(\PageIndex{1}\)

Write the net ionic equation for the reaction which would occur if the two solutions were mixed.

a. 6Ag⁺ + 6Cl^---> 6AgCl(s)

b. Ag⁺ + Cl^- --> AgCl(s)

c. 2Al⁺³ + 3SO₄^-2 --> 2 Al₂3SO₄)₃(s)

d. none of these

Answer: c. 2Al⁺³ + 6Cl^- + 6Ag⁺ + 3SO₄^-2 --> 2 Al⁺³ + 3SO₄^-2 + 6AgCl(s)

Exercise \(\PageIndex{1}\)

Calculate the number of moles of all ions in solution A.

a. Al⁺³ = 0.5 mol, Cl^- = 1.5

b. Al⁺³ = 0.2 mol, Cl^- = 0.6

c. Al⁺³ = 0.02mol, Cl^- = 0.06

d. none of these

Answer: c. Al⁺³ = 0.02mol, Cl^- = 0.06

Exercise \(\PageIndex{1}\)

Calculate the number of moles of all ions in solution B.

a. 1 mol sulfate, 2 mol silver

b. 0.12 mol sulfate, 0.060 mol silver

c. 0.06 mol sulfate, 0.12 mole silver

d. none of these

Answer: c. 0.06 mol sulfate, 0.12 mole silver

Exercise \(\PageIndex{1}\)

What mass of precipitate is formed after the two solutions are mixed. Assume complete reaction.

a. 17g

b. 0.06g

c. 8.6g

d. none of these

Answer: c. 8.6g

Exercise \(\PageIndex{1}\)

What is the final concentration of the excess reagent after the two solutions are mixed?

a. 0.06M

b. 0.60M

c. 0.12M

d. none of these

Answer: b. 0.60M

Exercise \(\PageIndex{1}\)

What is the final concentration of the spectator ions after the two solutions are mixed?

a. aluminum is 0.20M, sulfate is 0.60 M

b. aluminum is 0.60M, sulfate is 0.60 M

c. aluminum is 0.20M, sulfate is 0.20 M

d. none of these

Answer: a. aluminum is 0.20M, sulfate is 0.60 M

Precipitation Reactions

Exercise \(\PageIndex{1}\)

Predict any products formed if ammonium fluoride is mixed with magnesium nitrate.

a. ammonium nitrate

b. magnesium fluoride

c. ammonium nitrate and magnesium fluroide

d. no reaction

Answer: b. magnesium fluoride

Exercise \(\PageIndex{1}\)

Predict any products that would result if solutions of mercury(I)perchlorate were mixed with Iron(III)chloride.

a. \(\ce{HgCl}\)

b. \(\ce{Hg2Cl2}\)

c. \(\ce{Fe(CLO4)2}\) and \(\ce{HgCl}\)

d. no reaction

Answer: b. \(\ce{Hg2Cl2}\)

Exercise \(\PageIndex{1}\)

Predict any products that would form if solutions of sodium sulfide, potassium oxolate and ammonium carbonate were mixed.

a. sodium carbonate

b. ammonium oxolate

c. ammonium sulfide and ammonium oxolate

d. no reaction

Answer: d. no reaction

Exercise \(\PageIndex{1}\)

Predict any products which would occur if solutions of Barium nitrate, lead(II)nitrate, sodium sulfate and sodium oxolate are mixed.

a. barium sulfate

b. Barium oxolate & lead(II)oxolate

c. Barium sulfate, barium oxolate & lead(II)oxolate

d. no reaction

Answer: c. Barium sulfate, barium oxolate & lead(II)oxolate

Exercise \(\PageIndex{1}\)

Predict any products which would form if solutions of ammonium carbonate, sodium phosphate and barium chloride are mixed.

a. ammonium phosphate

b. barium carbonate

c. barium carbonate & barium phosphate

d. no reaction

Answer: c. barium carbonate & barium phosphate

Oxidation Numbers

Exercise \(\PageIndex{1}\)

What is the oxidtion state of Chlorine in HClO?

a. 1

b. 3

c. 5

d. 7

Answer: a. 1

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in HClO₂?

a. 1

b. 3

c. 5

d. 7

Answer: b. 3

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in HClO₃?

a. 1

b. 3

c. 5

d. 7

Answer: c. 5

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in HClO₄?

a. 1

b. 3

c. 5

d. 7

Answer: d. 7

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in ClO^-?

a. 1

b. 3

c. 5

d. 7

Answer: a. 1

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in ClO₂^-?

a. 1

b. 3

c. 5

d. 7

Answer: b. 3

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in ClO₃^-?

a. 1

b. 3

c. 5

d. 7

Answer: c. 5

Exercise \(\PageIndex{1}\)

What is the oxidation state of chlorine in ClO₄^-?

a. 1

b. 3

c. 5

d. 7

Answer: d. 7

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in H₂SO₄?

a. 2

b. 4

c. 6

d. 8

Answer: c. 6

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in H₂SO₃?

a. 2

b. 4

c. 6

d. 8

Answer: b. 4

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in SO₃?

a. 2

b. 4

c. 6

d. 8

Answer: c. 6

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in SO₃^-2?

a. 2

b. 4

c. 6

d. 8

Answer: b. 4

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in SO₄^-2?

a. 2

b. 4

c. 6

d. 8

Answer: c. 6

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in S₂O₃^-2?

a. 2

b. 4

c. 6

d. 8

Answer: a. 2

Exercise \(\PageIndex{1}\)

What is the oxidation state of sulfur in Na₂S₂O₃?

a. 2

b. 4

c. 6

d. 8

Answer: a. 2

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