chapter 7 quiz questions, review questions, and textbook questions

An aqueous solution of sodium sulfate is allowed to react with an aqueous solution of barium nitrate.What is the coefficient of the solid in the balanced equation (in standard form)?

1

The common strong acids are HCl, HNO3, and H2SO4, whereas NaOH and KOH are the common strong bases. Write the neutralization reaction equations for each of these strong acids with each of these strong bases in aqueous solution.

1. HCl(aq)+NaOH(aq) --> NaCl(aq)+H2O(l) 2. HNO3(aq)+NaOH(aq)--> NaNO3(aq)+H2O(l) 3. H2SO4(aq)+2NaOH(aq)--> Na2SO4(aq)+2H2O(l) 4. HCl(aq)+KOH(aq)--> KCl(aq)+H2O(l) 5. HNO3(aq)+KOH(aq) --> KNO3(aq)+H2O(l) 6. H2SO4(aq)+2KOH(aq)--> K2SO4(aq)+2H2O(l)

classify each of the following reactions as many ways as possible 1. 2K(s) + Cl2(g)---> 2KCl(s) 2. Fe2O3(s) +2Al (s)---> Al2O3(s) + 2Fe(s) 3. 2Mg(s) + O2(g)---> 2MgO(s) 4. HNO3(aq) + NaOH(aq) ---> H2O(l) + NaNO3(aq) 5. kbR(AQ) + AgNo3(aq) ---> AgBr(s) + KNO3(aq) 6. PbO2(s) ---> Pb(s) + O2(g) 7. 4NH3(g) + 5O2(g)---> 4NO(g) + 6H2O(g) 8. S8(s) + 8O2(g)---> 8SO2(g) 9. 2Al(s) +3Cl2(g)---> 2AlCl3(s) 10. 2AlN(s)---> 2Al(s) + N2(g) 11. BaCl2(aq) + Na2SO4(aq) ---> BaSO4(s) + 2NaCl(aq) 12.2Cs(s) + Br2(l)---> 2CsBr(s) 13. KOH(aq) + HCl(aq)---> H2O(l) + KCl(aq) 14. 2C2H2(g) + 5O2(g)---> 4CO2(g) + 2H2O(l)

1. synthesis and oxidation-reduction reaction 2. oxidation-reduction reaction 3. synthesis and oxidation-reduction reaction 4. acid-base 5. precipitation reaction 6. decomposition reaction and oxidation-reduction reaction 7. oxidation-reduction reaction and combustion 8. synthesis reaction, oxidation-reduction reaction, and combustion 9. oxidation-reduction reaction and synthesis 10. oxidation-reduction reaction and decomposition 11. precipitation reaction 12. oxidation-reoxidation-reduction reaction duction reaction and synthesis 13. acid-base 14. oxidation-reduction reaction and combustion

When the following equation is balanced in standard form, what is the coefficient in front of the H2O? C8H18(g) + O2(g) CO2(g) + H2O(g)

18

How many electrons are transferred in the following oxidation-reduction reaction? Zn(s) + 2AgNO3(aq) → Zn(NO3)2(aq) + 2Ag(s)

2

An aqueous solution of sodium sulfate is allowed to react with an aqueous solution of lead(II) nitrate.The complete ionic equation contains which of the following species (when balanced in standard form)?.

2Na+(aq)

An aqueous solution of sodium sulfide is allowed to react with an aqueous solution of magnesium chloride.The complete ionic equation contains which of the following species (when balanced in standard form)?

2Na+(aq)

2Na(s)+ Br2(l)--->

2NaBr(s)

KOH(aq) + Fe(NO3)3(aq)

3KOH(aq)+Fe(NO3)3(aq)= Fe(OH)3(s)+3KNO3(aq) 1.balance equation bexause products said Fe would be 3+ 2. hydroxides are insoluble thus solid is formed

How many of the following are oxidation-reduction reactions?I. reaction of a metal with a nonmetalII. synthesisIII. combustionIV. precipitationV. decomposition

4

AgNO3(aq)+KCl(aq)=

AgCl(s)+KNO3(aq) 1. Chloride salts are soluble however Ag is exception making it insoluble and thus solid

Which of the following will not be spectator ions in the reaction in aqueous solution of barium nitrate and potassium phosphate?

Ba2+ and PO43-

Ba(NO3)2(aq)+NaCl(aq)

BaCl2+ Na(NO3) 1. barium is 2+ so we have to multiply Cl's -1 times 2 2. both are soluble so none is present

Na2S(aq)+Cu(NO3)2(aq)

CuS(s)+2NaNO3(aq) 1. dont forget to balance out whole equation 2. copper sulfide is solide because sulfides are insoluble

NH4Cl(aq) + Pb(No3)2(aq)

PbCl2(s)+2NH4NO3(aq) 1.spread all out and put correct ions on each 2.because NO3 has a 2 on the outside , when doing ions put the 2 as if it where a coefficient 3.match each up and keep that coefficient

An aqueous solution of potassium chloride is mixed with an aqueous solution of sodium nitrate.

There is no solid formed when the two solutions are mixed.

Which of the following statements is not true?

When two nonmetals react, the compound formed is ionic.

A substance that, when dissolved in water, produces a solution that conducts electric current very efficiently is called

a strong electrolyte

aqueous Ammonium Chloride and aqueous lead(II) Nitrate react to form solid lead(II) chloride and aqueous ammonium nitrate a. molecular equation b. complete ionic equation c.net ionic equation

a. 2NH4Cl(aq) + Pb(NO3)2(aq)= PbCl2(s) + 2NH4NO3(aq) b. 2NH4+(aq) + 2Cl^-(aq) + Pb^2+(aq) + 2NO3^-(aq) = PbCl2(s) + 2NH4^+(aq) + 2NO3^-(aq) c. 2Cl^-(aq) + Pb^2+(aq) = PbCl2(s)

aqueous potassium hydroxide is mixed with aqueous iron(III) nitrate to form solid iron(III) hydroxide and aqueous potassium nitrate a. molecular equation b. complete ionic equation c.net ionic equation

a. 3KOH(aq) + Fe(NO3)3(aq)= Fe(OH)3(s) + 3KNO3(aq) b. 3K^+(aq) + 3OH^-(aq) + Fe^3+(aq) + 3NO3^-(aq) = Fe(OH)3(s) + 3K^+(aq) + 3NO3^-(aq) c. 3OH^-(aq) + Fe^3+(aq) = Fe(OH)3(s)

reaction between hydrochloric acid and aqueous sodium hydroxide a. molecular equation b. complete ionic equation c.net ionic equation

a. HCl(aq) + NaOH(aq) ---> H20(l) + NaCl(aq) b. H^+(aq) + Cl^-(aq) + Na^+(aq) + OH^-(aq) ---> H20(l) + Na^+(aq) + Cl^-(aq) c. H^+(aq) + OH^-(aq) ---> H20(l)

reaction of aqueous nitric acid and aqueous potassium hydroxide a. molecular equation b. complete ionic equation c.net ionic equation

a. HNO3(aq) + KOH(aq) ---> H20(l) + KNO3(aq) b. H^+(aq) + NO3^-(aq) + K^+(aq) + OH^-(aq) ---> H20(l) + K^+(aq) + NO3^-(aq) c. H^+(aq) + OH^-(aq) ---> H20(l)

aqueous sodium sulfide is mixed with aqueous copper(II) nitrate to produce solid copper (II) sulfide and aqueous sodium nitrate a. molecular equation b. complete ionic equation c.net ionic equation

a. Na2S(aq) + Cu(NO3)2(aq)= CuS(s) + 2NaNO3(aq) b. 2Na+(aq) + S^2-(aq) + Cu^2+(aq) + 2NO3^-(aq) = CuS(s) + 2Na^+(aq) + 2NO3^-(aq) c. S^2-(aq) + Cu^2+(aq) = CuS(s)

aqueous sodium chloride is added to aqueous silver nitrate to form solid silver chloride plus aqueous sodium nitrate a. molecular equation b. complete ionic equation c.net ionic equation

a. NaCl(aq)+AgNO3(aq)= AgCl(s)+NaNO3(aq) b. Na^+(aq) + Cl^-(aq) + Ag^+(aq) + NO3^-(aq) = AgCl(s) + Na^+(aq) + NO3^-(aq) c. Cl^-(aq) + Ag^+(aq) = AgCl(s)

Write the balanced net ionic equation for the reaction that takes place when aqueous solutions of the following are mixed. If no reaction is likely, explain why no reaction would be expected for that combination of solutes. a. potassium nitrate and sodium chloride b. calcium nitrate and sulfuric acid c. ammonium sulfide and lead(II) nitrate d.sodium carbonate and iron(III) chloride e. mercurous nitrate and calcium chloride f. silver acetate and potassium chloride h. sulfuric acid and nickel(II) sulfate

a. no reaction( all combinations are soluble) b. Ca2+(aq) + SO42-(aq) --> CaSO4(s) c. Pb2+(aq) + S2-(aq)--> PbS(s) d. 2Fe3+(aq) + 3CO32-(aq)--> Fe2(CO3)3(s) e. Hg22+(aq) + 2Cl-(aq)--> Hg2Cl2(s) f. Ag+(aq) + Cl-(aq)--> AgCl(s) h. no reaction (all combinations are soluble)

The reagent shelf in a general chemistry lab contains aqueous solutions of the following substances: silver nitrate, sodium chloride, acetic acid, nitric acid, sulfuric acid, potassium chromate, barium nitrate, phosphoric acid, hydrochloric acid, lead nitrate, sodium hydroxide, and sodium carbonate. Suggest how you might prepare the following pure substances using these reagents and any normal laboratory equipment. If it is not possible to prepare a substance using these reagents, indicate why. a. BaCrO4(s) b. NaC2H3O2(s) c. AgCl(s) d. PbSO4(s) e. Na2SO4(s) f. chromium(III) sulfide g.BaCO3(s)

a.Ba(NO3)2(aq) + K2CrO4(aq) solution)-->BaCrO4(s) + 2KNO3(aq) b. NaOH(aq) + CH3COOH(aq)--> H2O(l) + NaCH3COO(aq) (then evaporate the water from the solution) c. AgNO3(aq) + NaCl(aq)--> AgCl(s) + NaNO3(aq) d. Pb(NO3)2(aq) + H2SO4(aq) -->PbSO4(s) + 2HNO3(aq) e. 2NaOH(aq) + H2SO4(aq) -->Na2SO4(aq) + 2H2O(l) (then evaporate the water from the solution) f. Ba(NO3)2(aq) + Na2CO3(aq) --> BaCO3(s) + 2NaNO3(a

Balance each equation. Which equations can be classified as oxidation-reduction reaction? a.FeO(s) + HNO3(aq)--> Fe(NO3)2(aq) + H2O(l) b.Mg(s) + CO2(g) + O2(g)-->MgCO3(s) c. NaOH(s) + CuSO4(aq)-->Cu(OH)2(s) + Na2SO4(aq) d. HI(aq) + KOH(aq)-->KI(aq) + H2O(l) e. C3H8(g) + O2(g)--> CO2(g) + H2O(g) f. Co(NH3)6Cl2(s)--> CoCl2(s) + NH3(g) g. HCl(aq) + Pb(C2H3O2)2(aq)--> HC2H3O2(aq) + PbCl2(s) h. C12H22O11(s)--> C(s) + H2O(g) i. Al(s) + 6HNO3(aq) --> Al(NO3)3(aq) + H2(g) j. B(s) + O2(g) --> B2O3(s)

a.FeO(s) + 2HNO3(aq) ® Fe(NO3)2(aq) + H2O(l) acid-base, double-displacement b. 2Mg(s) + 2CO2(g) + O2(g) --> 2MgCO3(s) synthesis; oxidation-reduction c. 2NaOH(s) + CuSO4(aq)--> Cu(OH)2(s) + Na2SO4(aq) precipitation, double-displacement d. HI(aq) + KOH(aq) --> KI(aq) + H2O(l) acid-base, double-displacement e. C3H8(g) + 5O2(g)--> 3CO2(g) + 4H2O(g) combustion; oxidation-reduction f. Co(NH3)6Cl2(s)--> CoCl2(s) + 6NH3(g) decomposition g. 2HCl(aq) + Pb(C2H3O2)2(aq)--> 2HC2H3O2(aq) + PbCl2(s) precipitation, double-displacement h. C12H22O11(s) --> 12C(s) + 11H2O(g) decomposition; oxidation-reduction i. 2Al(s) + 6HNO3(aq)--> 2Al(NO3)3(aq) + 3H2(g) single-displacement; oxidation-reduction j. 4B(s) + 3O2(g) --> 2B2O3(s) synthesis; oxidation-reduction

The reaction HNO3(aq) + KOH(aq) H2O(l) + KNO3(aq) is a(n) ________ reaction.

acid base

Classify the following reaction: HNO3(aq) + KOH(aq) → KNO3(aq) +H2O(l)

acid-base

True or false? The complete ionic equation contains only those substances directly involved in reactions in aqueous solutions.

false

What is the name of the acid formed when HBr gas is dissolved in water?

hydrobromic acid

KNO3(aq)+ Pb(NO3)2(aq)

no reaction takes place because both are soluble in water. No chemical change.

The reaction 2K(s) + Br2(l) → 2KBr(s) is a(n) ______________ reaction.

oxidation-reduction

The reaction AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq) is a(n) ______________ reaction.

precipitation

True or false? Oxidation and reduction must occur simultaneously.

true