SmartBook Ch. 4 Pt. II

A precipitation reaction is a reaction in which two or more water-_____ ionic compounds react in aqueous solution to form one or more _____ precipitates.

soluble, ionic

A net ionic equation eliminates the _____ ions and shows the net chemical change taking place in a reaction.

spectator

Ions that are present in a reaction but not involved in the actual chemical change are called _____ ions. These ions will appear unchanged on both sides of a total ionic equation.

spectator

A(n) _____ ionic equation shows all soluble ionic substances dissociated into ions. Both the atoms and the electrical _____ must be balanced in this type of equation.

total, charge

Which of the following net ionic equations correctly predicts the formation of an insoluble product? Select all that apply. a) Ba2+ (aq) + CO32- (aq) → BaCO3 (s) b) Na+ (aq) + Cl- (aq) → NaCl (s) c) 2NH4+ (aq) + S2- (aq) → (NH4)2S (s) d) Ag+ (aq) + Br- (aq) → AgBr (s)

a) Ba2+ (aq) + CO32- (aq) → BaCO3 (s) d) Ag+ (aq) + Br- (aq) → AgBr (s)

Which of the following statements correctly describe a total ionic equation? Select all that apply. a) Charges must be included where appropriate in this type of equation. b) Charges and atoms must be balanced in this type of equation. c) This equation shows only the ions involved in a reaction. d) The total ionic equation includes all ions, including spectator ions. e) All species must show charges in this type of equation.

a) Charges must be included where appropriate in this type of equation. b) Charges and atoms must be balanced in this type of equation. d) The total ionic equation includes all ions, including spectator ions.

Which of the following compounds are soluble in water? Select all that apply. a) Pb(NO3)2 b) Na3PO4 c) BaSO4 d) NH4Cl e) CaCO3

a) Pb(NO3)2 b) Na3PO4 d) NH4Cl

Which of the following correctly defines spectator ions? a) Ions that appear in a net ionic equation b) Ions that do not participate in the reaction although they are present c) Ions that are dissociated in solution d) Ions that combine to form an insoluble precipitate

b) Ions that do not participate in the reaction although they are present

Select the correct net ionic equation if the total ionic equation is given by 2K+ (aq) + 2Cl- (aq) + Pb2+ (aq) + 2CH3COO- (aq) → 2K+ (aq) + PbCl2 (s) + 2CH3COO- (aq) a) Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s) b) K+ (aq) + CH3COO- (aq) → KCH3COO (s) c) K+ (aq) + Cl- (aq) → KCl (s) d) K+ (aq) + CH3COO- (aq) → K+ (aq) + CH3COO- (aq)

a) Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s)

Which of the following options correctly describe the steps required to decide whether or not a precipitate forms when two aqueous solutions are mixed? Select all that apply. a) The products of the reaction are identified from the possible cation-anion combinations. b) The first step is to identify the ions present in each solution. c) Each cation present could combine with any of the other ions present. d) If one product is a precipitate, the other will always be soluble. e) Any product that is insoluble in water will be a precipitate.

a) The products of the reaction are identified from the possible cation-anion combinations. b) The first step is to identify the ions present in each solution. e) Any product that is insoluble in water will be a precipitate.

Which of the following statements correctly describe a molecular equation? Select all that apply. a) This equation represents all reactants and products as if they were intact and undissociated. b) This equation gives the most accurate representation of the chemical changes taking place. c) A molecular equation will not include any charges on any of the species. d) This equation only shows molecular substances that participate in a reaction.

a) This equation represents all reactants and products as if they were intact and undissociated. c) A molecular equation will not include any charges on any of the species.

Place the steps required to determine whether or not a precipitate forms when two solutions are mixed in the correct order. Start with the first step at the top of the list. a) Note the ions present in the reactants. b) Use the solubility rules to determine whether or not either of the combinations gives an insoluble salt. c) Consider possible cation-anion combinations.

a, c, b

Select the correct net ionic equation if the total ionic equation is given by Ca (s) + 2H+ (aq) + 2Cl- (aq) → Ca2+ (aq) + H2 (g) + 2Cl- (aq) a) 2H+ (aq) → H2 (g) b) Ca (s) + 2H+ (aq) → Ca2+ (aq) + H2 (g) c) There is no net ionic equation. d) Ca (s) + 2Cl- (aq) → Ca2+ (aq) + 2Cl- (aq)

b) Ca (s) + 2H+ (aq) → Ca2+ (aq) + H2 (g)

Which of the following species should be included in the net ionic equation for the precipitation reaction given? (States of matter have not been included; use the solubility rules to determine which compound(s) form(s) precipitates, if any.) ZnSO4 + CaCl2 → CaSO4 + ZnCl2 a) Zn2+ b) CaSO4 c) ZnCl2 d) Ca2+ e) SO42-

b) CaSO4 d) Ca2+ e) SO42-

Identify the spectator ion in the following total ionic equation: 2Fe (s) + 3Ni2+ (aq) + 6Cl- (aq) → 2Fe3+ (aq) + 3Ni (s) + 6Cl- (aq) a) Ni2+ b) Cl- c) Fe3+

b) Cl-

Identify ALL the spectator ions in the following total ionic equation: 2Na+ (aq) + SO42- (aq) + Ba2+ (aq) + 2Cl- (aq) → BaSO4 (s) + 2Na+ (aq) + 2Cl- (aq) a) Ba2+ b) Cl- c) SO42- d) Na+

b) Cl- d) Na+

Which of the following is the correct formula for the precipitate that forms when aqueous solutions of Pb(NO3)2 and KCl are mixed? a) KNO3 b) PbCl2 c) PbK d) PbCl

b) PbCl2

Given the balanced equation CaCO3 (s) + 2HCl (aq) → CaCl2 (aq) + H2O (l) + CO2 (g), select all the statements that correctly describe how to calculate the mass of CaCO3 that will react with 72.5 mL of a 0.250 M solution of HCl. (The molar mass of CaCO3 is 100.09 g/mol.) a) 3.62 × 10-2 moles of CaCO3 will react. b) The conversion factor 0.250mol HCl1L HCl0.250mol HCl1L HCl will be used as written in the calculation. c) 0.907 g of CaCO3 will react. d) 0.290 mol of HCl are used in this reaction.

b) The conversion factor 0.250mol HCl1L HCl0.250mol HCl1L HCl will be used as written in the calculation. c) 0.907 g of CaCO3 will react.

Which of the following options correctly describe a precipitation reaction? Select all that apply. a) The reaction involves a transfer of electrons between reactants. b) This type of reaction usually involves ionic compounds. c) This type of reaction forms one or more insoluble products. d) This type of reaction often occurs in aqueous solution. e) The reactants are insoluble precipitates.

b) This type of reaction usually involves ionic compounds. c) This type of reaction forms one or more insoluble products. d) This type of reaction often occurs in aqueous solution.

Match each ion to the correct description of its solubility when combined with an ion of opposite charge. Na+ SO42- CO32- Cl- a) Soluble except with Ca2+, Sr2+, Ba2+, Ag+, and Pb2+ b) Soluble in all combinations c) Soluble except with Ag+, Pb2+, Cu+, and Hg22+ d) Insoluble except with Group 1A cations or NH4+

b, a, d, c

Match each type of equation with the correct description. Molecular equation Total ionic equation Net ionic equation a) Omits spectator ions and shows the actual chemical change taking place b) Shows all the reactants and products as intact, undissociated compounds c) Shows soluble ionic substances dissociated into ions

b, c, a

Which of the following statements correctly describe a net ionic equation? Select all that apply. a) All species are represented as ions in this type of equation. b) A net ionic equation consists of the formulas for the spectator ions. c) A net ionic equation shows only the chemical change that is taking place in a reaction. d) A net ionic equation shows only the ionic species that are involved in the reaction and the products that form. e) A net ionic equation shows only the species that have undergone a change in the reaction, and any products that form.

c) A net ionic equation shows only the chemical change that is taking place in a reaction. e) A net ionic equation shows only the species that have undergone a change in the reaction, and any products that form.

Which of the following gives the correct net ionic equation for the process represented below? AgNO3 (aq) + KCl (aq) → AgCl (s) + KNO3 (aq) a) Ag+ (aq) + NO3- (aq) + K+ (aq) + Cl- (aq) → AgCl (s) + K+ (aq) + Cl- (aq) b) Ag+ (aq) + NO3- (aq) → AgNO3 (aq) c) Ag+ (aq) + Cl- (aq) → AgCl (s) d) K+ (aq) + NO3- (aq) → KNO3 (aq)

c) Ag+ (aq) + Cl- (aq) → AgCl (s)

Which combinations of solutions will produce one or more precipitates? Select all that apply. a) MgCl2 (aq) + Na2SO4 (aq)MgCl2 (aq) + Na2SO4 (aq) b) Ba(NO3)2 (aq) +KI (aq)Ba(NO3)2 (aq) + KI (aq) c) CaBr2 (aq) + K3PO4 (aq)CaBr2 (aq) + K3PO4 (aq) d) AgNO3 (aq) + NH4Br (aq)

c) CaBr2 (aq) + K3PO4 (aq)CaBr2 (aq) + K3PO4 (aq) d) AgNO3 (aq) + NH4Br (aq)

Which of the following ions always form soluble ionic compounds? Select all that apply. a) PO43- b) SO42- c) NH4+ d) Group 1A cations e) NO3-

c) NH4+ d) Group 1A cations e) NO3-

Three equations representing a chemical reaction are shown. Classify each equation according to type. 1) Molecular equation 2) Total ionic equation 3) Net ionic equation a) Pb2+ (aq) + 2NO3- (aq) + 2Na+ (aq) + 2Cl- (aq) → PbCl2 (s) + 2Na+ (aq) + 2NO3- (aq) b) Pb2+ (aq) + 2Cl- (aq) → PbCl2 (s) c) Pb(NO3)2 (aq) + 2NaCl (aq) → PbCl2 (s) + 2NaNO3 (aq)

c, a, b

Given the balanced equation Mg (s) + 2HNO3 (aq) → Mg(NO3)2 (aq) + H2 (g), calculate the volume of 0.624 M HNO3 required to react completely with 5.62 g of Mg. a) 5.62 L b) 0.370 L c) 2.89 L d) 0.741 L

d) 0.741 L

Which of the following correctly defines a precipitate? a) A liquid that forms in a reaction b) A soluble ionic compound c) An aqueous solution that forms from a solid d) A solid product that separates from a solution

d) A solid product that separates from a solution

A chemical equation that shows all reactants and products as intact, undissociated compounds is called a(n) _____ equation. The name is misleading because not all compounds in the equation consist of _____.

molecular, molecules

An insoluble product (i.e., a solid) that forms from a reaction in solution is called a(n) _____.

precipitate