Deck 4: Aqueous Reactions and Solution Stoichiometry

Question 1

Of the species below, only ________ is not an electrolyte.

A)HCl
B)Rb₂SO₄
C)Ar
D)KOH
E)NaCl

Answer 1

Ar

Question 2

Which one of the following is a weak acid?

A)HNO₃
B)HCl
C)HI
D)HF
E)HClO₄

Answer 2

HF

Question 3

Which combination will produce a precipitate?

A)NH₄OH (aq)and HCl (aq)
B)AgNO₃ (aq)and Ca(C₂H₃O₂)₂ (aq)
C)NaOH (aq)and HCl (aq)
D)NaCl (aq)and HC₂H₃O₂ (aq)
E)NaOH (aq)and Fe(NO₃)₂ (aq)

Answer 3

NaOH (aq)and Fe(NO₃)₂ (aq)

Question 4

Which of the following is insoluble in water at 25 °C?

A)Mg₃(PO₄)₂
B)Na₂S
C)(NH₄)₂CO₃
D)Ca(OH)₂
E)Ba(C₂H₃O₂)₂

Question 5

When aqueous solutions of ________ are mixed, a precipitate forms.

A)NiBr₂ and AgNO₃
B)NaI and KBr
C)K₂SO₄ and CrCl₃
D)KOH and Ba(NO₃)₂
E)Li₂CO₃ and CsI

Question 6

Which combination will produce a precipitate?

A)NaC₂H₃O₂ (aq)and HCl (aq)
B)NaOH (aq)and HCl (aq)
C)AgNO₃(aq)and Ca(C₂H₃O₂)₂ (aq)
D)KOH (aq)and Mg(NO₃)₂ (aq)
E)NaF (aq)and HCl (aq)

Question 7

The net ionic equation for formation of an aqueous solution of Al(NO₃)₃ via mixing solid Al(OH)₃ and aqueous nitric acid is ________.

A)Al(OH)₃ (s) + 3HNO₃ (aq) → 3H₂O (l) + Al(NO₃)₃ (aq)
B)Al(OH)₃ (s) + 3NO₃^- (aq) → 3OH^- (aq) + Al(NO₃)₃ (aq)
C)Al(OH)₃ (s) + 3NO₃^- (aq) → 3OH^- (aq) + Al(NO₃)₃ (s)
D)Al(OH)₃ (s) + 3H⁺ (aq) → 3H₂O (l) + Al³⁺ (aq)
E)Al(OH)₃ (s) + 3HNO₃ (aq) → 3H₂O (l) + Al³⁺ (aq) + NO₃^- (aq)

Question 8

The net ionic equation for the reaction between aqueous sulfuric acid and aqueous sodium hydroxide is ________.

A)H⁺ (aq) + HSO₄^- (aq) + 2OH^- (aq) → 2H₂O (l) + SO₄^2- (aq)
B)H⁺ (aq) + HSO₄^- (aq) + 2Na⁺ (aq) + 2OH^- (aq) → 2H₂O (l) + 2Na⁺ (aq) + SO₄^2-(aq)
C)SO₄^2- (aq) + 2Na⁺ (aq) → 2Na⁺ (aq) + SO₄^2-(aq)
D)H⁺ (aq) + OH^- (aq) → H₂O( l)
E)2H⁺ (aq) + SO₄^2- (aq) + 2Na⁺ (aq) + 2OH^- (aq) → 2H₂O (l) + 2Na⁺ (aq) + SO₄^2- (aq)

Question 9

With which of the following will the ammonium ion form an insoluble salt?

A)chloride
B)sulfate
C)carbonate
D)sulfate and carbonate
E)none of the above

Question 10

The reaction between strontium hydroxide and chloric acid produces ________.

A)a molecular compound and a weak electrolyte
B)two weak electrolytes
C)two strong electrolytes
D)a molecular compound and a strong electrolyte
E)two molecular compounds

Question 11

Aqueous solutions of a compound did not form precipitates with Cl^-, Br^-, I^-, SO₄^2-, CO₃^2-, PO₄^3-, OH^-, or S^2-. This highly water-soluble compound produced the foul-smelling gas H₂S when the solution was acidified. This compound is ________.

A)Pb(NO₃)₂
B)(NH₄)₂S
C)KBr
D)Li₂CO₃
E)AgNO₃

Question 12

Which combination will produce a precipitate?

A)Pb(NO₃)₂ (aq)and HCl (aq)
B)Cu(NO₃)₂ (aq)and KC₂H₃O₂ (aq)
C)KOH (aq)and HNO₃ (aq)
D)AgC₂H₃O₂ (aq)and HC₂H₃O₂ (aq)
E)NaOH (aq)and Sr(NO₃)₂ (aq)

Question 13

The net ionic equation for formation of an aqueous solution of NiI₂ accompanied by evolution of CO₂ gas via mixing solid NiCO₃ and aqueous hydriodic acid is ________.

A)2NiCO₃ (s) + HI (aq) → 2H₂O (l) + CO₂ (g) + 2Ni²⁺ (aq)
B)NiCO₃ (s) + I^- (aq) → 2H₂O (l) + CO₂ (g) + Ni²⁺ (aq) + HI (aq)
C)NiCO₃ (s) + 2H⁺ (aq) → H₂O (l) + CO₂ (g) + Ni²⁺ (aq)
D)NiCO₃ (s) + 2HI (aq) → 2H₂O (l) + CO₂ (g) + NiI₂ (aq)
E)NiCO₃ (s) + 2HI (aq) → H₂O (l) + CO₂ (g) + Ni²⁺ (aq) + 2I^- (aq)

Question 14

Which one of the following is a diprotic acid?

A)nitric acid
B)chloric acid
C)phosphoric acid
D)hydrofluoric acid
E)sulfuric acid

Question 15

Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)reaction?

A)calcium nitrate
B)sodium bromide
C)lead nitrate
D)barium nitrate
E)sodium chloride

Question 16

Which one of the following compounds is insoluble in water?

A)K₂SO₄
B)Ca(C₂H₃O₂)₂
C)MgC₂O₄
D)ZnCl₂
E)Mn(NO₃)₂

Question 17

The balanced molecular equation for complete neutralization of H₂SO₄ by KOH in aqueous solution is ________.

A)2H⁺ (aq) + 2OH^- (aq) → 2H₂O (l)
B)2H⁺ (aq) + 2KOH (aq) → 2H₂O (l) + 2K⁺ (aq)
C)H₂SO₄ (aq) + 2OH^- (aq) → 2H₂O (l) + SO₄^2- (aq)
D)H₂SO₄ (aq) + 2KOH (aq) → 2H₂O (l) + K₂SO₄ (s)
E)H₂SO₄ (aq) + 2KOH (aq) → 2H₂O (l) + K₂SO₄ (aq)

Question 18

The net ionic equation for the reaction between aqueous nitric acid and aqueous sodium hydroxide is ________.

A)H⁺ (aq) + HNO₃ (aq) + 2OH^- (aq) → 2H₂O (l) + NO₃^- (aq)
B)HNO₃ (aq) + NaOH (aq) → NaNO₃ (aq) + H₂O (l)
C)H⁺ (aq) + OH^- (aq) → H₂O (l)
D)HNO₃ (aq) + OH^- (aq) → NO₃^- (aq) + H₂O (l)
E)H⁺ (aq) + Na⁺ (aq)+ OH^- (aq) → H₂O (l) + Na⁺ (aq)

Question 19

Which one of the following compounds is insoluble in water?

A)Na₂CO₃
B)K₂SO4
C)Fe(NO₃)₃
D)ZnS
E)AgNO₃

Question 20

Which one of the following is a triprotic acid?

A)nitric acid
B)chloric acid
C)phosphoric acid
D)hydrofluoric acid
E)sulfuric acid

Question 21

Zinc is more active than cobalt and iron but less active than aluminum. Cobalt is more active than nickel but less active than iron. Which of the following correctly lists the elements in order of increasing activity?

A)Co < Ni < Fe < Zn < Al
B)Ni < Fe < Co < Zn < Al
C)Ni < Co < Fe < Zn < Al
D)Fe < Ni < Co < Al < Zn
E)Zn < Al < Co < Ni < Fe

Question 22

Oxidation is the ________ and reduction is the ________.

A)gain of oxygen, loss of electrons
B)loss of oxygen, gain of electrons
C)loss of electrons, gain of electrons
D)gain of oxygen, loss of mass
E)gain of electrons, loss of electrons

Question 23

Based on the activity series, which one of the reactions below will occur?

A)Zn (s) + MnI₂ (aq) → ZnI₂ (aq) + Mn (s)
B)SnCl₂ (aq) + Cu (s) → Sn (s) + CuCl₂ (aq)
C)2AgNO₃ (aq) + Pb (s) → 2Ag (s) + Pb(NO₃)₂ (aq)
D)3Hg (l) + 2Cr(NO₃)₃ (aq) → 3Hg(NO₃)₂ + 2Cr (s)
E)3FeBr₂ (aq) + 2Au (s) → 3Fe (s) + 2AuBr₃ (aq)

Question 24

The balanced reaction between aqueous potassium hydroxide and aqueous acetic acid is ________.

A)KOH (aq) + HC₂H₃O₂ (aq) → OH^- (l) + HC₂H₃O₂⁺ (aq) + K (s)
B)KOH (aq) + HC₂H₃O₂ (aq) → H₂O (l) + KC₂H₃O₂ (aq)
C)KOH (aq) + HC₂H₃O₂ (aq) → H₂C₂H₃O₃ (aq) + K (s)
D)KOH (aq) + HC₂H₃O₂ (aq) → KC₂H₃O₃ (aq) + H₂ (g)
E)KOH (aq) + HC₂H₃O₂ (aq) → H₂KC₂H₃O (aq) + O₂ (g)

Question 25

In which reaction does the oxidation number of hydrogen change?

A)HCl (aq) + NaOH (aq) → NaCl (aq) + H₂O (l)
B)2Na (s) + 2H₂O (l) → 2NaOH (aq) + H₂ (g)
C)CaO (s) + H₂O (l) → Ca(OH)₂ (s)
D)2HClO₄ (aq) + CaCO₃ (s) → Ca(ClO₄)₂ (aq) + H₂O (l) + CO₂ (g)
E)SO₂ (g) + H₂O (l) → H₂SO₃ (aq)

Question 26

Of the reactions below, only ________ is not spontaneous.

A)Mg (s) + 2HCl (aq) → MgCl₂ (aq) + H₂(g)
B)2Ag (s) + 2HNO₃ (aq) → 2AgNO₃ (aq) + H₂ (g)
C)2Ni (s) + H₂SO₄ (aq) → Ni₂SO₄ (aq) + H₂ (g)
D)2Al (s) + 6HBr (aq) → 2AlBr₃ (aq) + 3H₂ (g)
E)Zn (s) + 2HI (aq) → ZnI₂(aq) + H₂ (g)

Question 27

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.

A)HNO₃ (aq) + Sr(OH)₂ (aq) → Sr(NO₃)₂ (aq) + H₂ (g)
B)HNO₃ (aq) + Sr(OH)₂ (aq) → H₂O (l) + Sr(NO₃)₂ (aq)
C)HNO₃ (aq) + SrOH (aq) → H₂O (l) + SrNO₃ (aq)
D)2HNO₃ (aq) + Sr(OH)₂ (aq) → 2H₂O (l) + Sr(NO₃)₂ (aq)
E)2HNO₃ (aq) + Sr(OH)₂ (aq) → Sr(NO₃)₂(aq) + 2H₂ (g)

Question 28

Sodium does not occur in nature as Na (s)because ________.

A)it is easily reduced to Na^-
B)it is easily oxidized to Na⁺
C)it reacts with water with great difficulty
D)it is easily replaced by silver in its ores
E)it undergoes a disproportionation reaction to Na^- and Na⁺

Question 29

Which of these metals will be oxidized by the ions of cobalt?

A)nickel
B)tin
C)iron
D)copper
E)silver

Question 30

Which of these metals will be oxidized by the ions of aluminum?

A)magnesium
B)zinc
C)chromium
D)iron
E)nickel

Question 31

Which of the following are weak acids?

A)HF, HBr
B)HI, HNO₃, HBr
C)HI, HF
D)HF
E)none of the above

Question 32

Oxidation and ________ mean essentially the same thing.

A)activity
B)reduction
C)metathesis
D)decomposition
E)corrosion

Question 33

A compound was found to be soluble in water. It was also found that addition of acid to an aqueous solution of this compound resulted in the formation of carbon dioxide. Which one of the following cations would form a precipitate when added to an aqueous solution of this compound?

A)NH₄⁺
B)K⁺
C)Cr³⁺
D)Rb⁺
E)Na⁺

Question 34

Oxidation cannot occur without ________.

A)acid
B)oxygen
C)water
D)air
E)reduction

Question 35

Which compound has the atom with the highest oxidation number?

A)CaS
B)Na₃N
C)MgSO₃
D)Al(NO₂)₃
E)NH₄Cl

Question 36

One method for removal of metal ions from a solution is to convert the metal to its elemental form so it can be filtered out as a solid. Which metal can be used to remove aluminum ions from solution?

A)zinc
B)cobalt
C)lead
D)copper
E)none of these

Question 37

Of the choices below, which would be the best for the lining of a tank intended for use in storage of hydrochloric acid?

A)copper
B)zinc
C)nickel
D)iron
E)tin

Question 38

The net ionic equation for the dissolution of zinc metal in aqueous hydrobromic acid is ________.

A)Zn (s) + 2Br^- (aq) → ZnBr₂ (aq)
B)Zn (s) + 2HBr (aq) → ZnBr₂ (aq) + 2H⁺ (aq)
C)Zn (s) + 2HBr (aq) → ZnBr₂ (s) + 2H⁺ (aq)
D)Zn (s) + 2H⁺ (aq) → Zn²⁺ (aq) + H₂ (g)
E)2Zn (s) + H⁺ (aq) → 2Zn²⁺ (aq) + H₂ (g)

Question 39

In which reaction does the oxidation number of oxygen increase?

A)Ba(NO₃)₂ (aq) + K₂SO₄ (aq) → BaSO₄ (s) + 2KNO₃ (aq)
B)HCl (aq) + NaOH (aq) → NaCl (aq) + H₂O (l)
C)MgO (s) + H₂O (l) → Mg(OH)₂ (s)
D)2SO₂ (g) + O₂ (g) → 2SO₃ (g)
E)2H₂O (l) → 2H₂ (g) + O₂ (g)

Question 40

Based on the activity series, which one of the reactions below will occur?

A)Fe (s) + ZnCl₂ (aq) → FeCl₂ (aq) + Zn (s)
B)Mn (s) + NiCl₂ (aq) → MnCl₂ (aq) + Ni (s)
C)Pb (s) + NiI₂ (aq) → PbI₂ (aq) + Ni (s)
D)SnBr₂ (aq) + Cu (s) → CuBr₂ (aq) + Sn (s)
E)None of the reactions will occur.

Question 41

What volume (mL)of a concentrated solution of magnesium chloride (9.00 M)must be diluted to 350. mL to make a 2.75 M solution of magnesium chloride?

A)2.75
B)50.0
C)45.0
D)107
E)350

Question 42

Which of the following reactions will not occur as written?

A)Zn (s) + Pb(NO₃)₂ (aq) → Pb (s) + Zn(NO₃)₂ (aq)
B)Mg (s) + Ca(OH)₂ (aq) → Ca (s) + Mg(OH)₂ (aq)
C)Sn (s) + 2AgNO₃ (aq) → 2Ag (s) + Sn(NO₃)₂ (aq)
D)Co (s) + 2AgCl (aq) → 2Ag (s) + CoCl₂ (aq)
E)Co (s) + 2HI (aq) → H₂ (g) + CoI₂ (aq)

Question 43

Which of the following is an oxidation-reduction reaction?

A)Cu (s) + 2AgNO₃ (aq) → 2Ag (s) + Cu(NO₃)₂ (aq)
B)HCl (aq) + NaOH (aq) → H₂O (l) + NaCl (aq)
C)AgNO₃ (aq) + HCl (aq) → AgCl (s) + HNO₃ (aq)
D)Ba(C₂H₃O₂)₂ (aq) + Na₂SO₄ (aq) → BaSO₄ (s) + 2NaC₂H₃O₂(aq)
E)H₂CO₃ (aq) + Ca(NO₃)₂ (aq) → 2HNO₃ (aq) + CaCO₃ (s)

Question 44

Mixing 10.00 mL of an aqueous solution with 10.00 mL of water represents a ________.

A)crystallization
B)neutralization
C)twofold dilution
D)tenfold dilution
E)titration

Question 45

Which solution contains the largest number of moles of chloride ions?

A)10.0 mL of 0.500 M BaCl₂
B)4.00 mL of 1.000 M NaCl
C)7.50 mL of 0.500 M FeCl₃
D)25.00 mL of 0.400 M KCl
E)30.00 mL of 0.100 M CaCl₂

Question 46

A 0.100 M solution of ________ will contain the highest concentration of potassium ions.

A)potassium phosphate
B)potassium hydrogen carbonate
C)potassium hypochlorite
D)potassium iodide
E)potassium oxide

Question 47

The point in a titration at which the indicator changes is called the ________.

A)setpoint
B)indicator point
C)standard point
D)end point
E)volumetric point

Question 48

What volume (L)of 0.250 M HNO₃ is required to neutralize a solution prepared by dissolving 17.5 g of NaOH in 350 mL of water?

A)50.0
B)0.44
C)1.75
D)0.070
E)1.75 ×

Question 49

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca₃(PO₄)₂?

A)This solution contains 0.200 mol of Ca₃(PO₄)₂.
B)This solution contains 0.800 mol of oxygen atoms.
C)1.00 L of this solution is required to furnish 0.300 mol of Ca²⁺ ions.
D)There are 6.02 × 10²² phosphorus atoms in 500.0 mL of this solution.
E)This solution contains 0.600 mol of Ca²⁺.

Question 50

A 0.200 M K₂SO₄ solution is produced by ________.

A)dilution of 250.0 mL of 1.00 M K₂SO₄ to 1.00 L
B)dissolving 43.6 g of K₂SO₄ in water and diluting to a total volume of 250.0 mL
C)diluting 20.0 mL of 5.00 M K₂SO₄ solution to 500.0 mL
D)dissolving 20.2 g of K₂SO₄ in water and diluting to 250.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL
E)dilution of 1.00 mL of 250 M K₂SO₃ to 1.00 L

Question 51

What are the respective concentrations (M)of Fe³⁺ and I^- afforded by dissolving 0.200 mol FeI₃ in water and diluting to 725 mL?

A)0.276 and 0.828
B)0.828 and 0.276
C)0.276 and 0.276
D)0.145 and 0.435
E)0.145 and 0.0483

Question 52

Which one of the following is a correct expression for molarity?

A)mol solute/L solvent
B)mol solute/mL solvent
C)mmol solute/mL solution
D)mol solute/kg solvent
E)μmol solute/L solution

Question 53

An aliquot (28.7 mL)of a KOH solution required 31.3 mL of 0.118 M HCl for neutralization. What mass (g)of KOH was in the original sample?

A)1.64
B)7.28
C)0.173
D)0.207
E)0.414

Question 54

What mass (g)of potassium chloride is contained in 430.0 mL of a potassium chloride solution that has a chloride ion concentration of 0.193 M?

A)0.0643
B)0.0830
C)12.37
D)0.386
E)6.19

Question 55

A tenfold dilution of a sample solution can be obtained by taking ________.

A)1 part sample and 9 parts solvent
B)1 part sample and 10 parts solvent
C)9 parts sample and 1 part solvent
D)10 parts sample and 1 part solvent
E)99 parts sample and 1 part solvent

Question 56

You are given two clear solutions of the same unknown monoprotic acid, but with different concentrations. Which statement is true?

A)There is no chemical method designed to tell the two solutions apart.
B)It would take more base solution (per milliliter of the unknown solution)to neutralize the more concentrated solution.
C)A smaller volume of the less concentrated solution contains the same number of moles of the acid compared to the more concentrated solution.
D)If the same volume of each sample was taken, then more base solution would be required to neutralize the one with lower concentration.
E)The product of concentration and volume of the less concentrated solution equals the product of concentration and volume of the more concentrated solution.

Question 57

Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH?

A)20.0 mL of 0.200 M solution of NaOH
B)25.0 mL of 0.175 M solution of NaOH
C)30.0 mL of 0.145 M solution of NaOH
D)50.0 mL of 0.125 M solution of NaOH
E)100.0 mL of 0.0500 M solution of NaOH

Question 58

Which solution has the same number of moles of KCl as 75.00 mL of 0.250 M solution of KCl?

A)20.0 mL of 0.200 M solution of KCl
B)25.0 mL of 0.175 M solution of KCl
C)129 mL of 0.145 M solution of KCl
D)50.0 mL of 0.125 M solution of KCl
E)100 mL of 0.0500 M solution of KCl

Question 59

What are the respective concentrations (M)of Mg²⁺ and C₂H₃O₂^- afforded by dissolving 0.600 mol Mg(C₂H₃O₂)₂ in water and diluting to 135 mL?

A)0.444 and 0.889
B)0.0444 and 0.0889
C)0..889 and 0.444
D)0.444 and 0.444
E)4.44 and 8.89

Question 60

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to 200.0 mL to make a 0.880 M solution of sodium hydroxide?

A)2.64
B)176
C)26.4
D)29.3
E)50.0

Question 61

The spectator ions in the reaction between aqueous perchloric acid and aqueous barium hydroxide are ________.

A)OH^- and ClO₄^-
B)H⁺, OH^- , ClO₄^-, and Ba²⁺
C)H⁺ and OH^-
D)H⁺ and Ba²⁺
E)ClO₄^- and Ba²⁺

Question 62

The net ionic equation for the reaction between aqueous solutions of HF and KOH is ________.

A)HF + KOH → H₂O + K⁺ + F^-
B)HF + OH^{- →} H₂O + F^-
C)HF + K⁺ + OH^- → H₂O + KF
D)H⁺ + OH^- → H₂O
E)H⁺ + F^- + K⁺ + OH^- → H₂O + K⁺ + F^-

Question 63

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

A)H₂
B)H₂O
C)CO₂
D)NaOH
E)O₂

Question 64

A strong electrolyte is one that ________ completely in solution.

A)reacts
B)associates
C)disappears
D)ionizes

Question 65

When aqueous solutions of AgNO₃ and KI are mixed, AgI precipitates. The balanced net ionic equation is ________.

A)Ag⁺ (aq) + (aq) → AgI (s)
B)Ag⁺ (aq) + NO₃^- (aq) → AgNO₃ (s)
C)Ag⁺ (aq) + NO₃^- (aq) → AgNO₃ (aq)
D)AgNO₃ (aq) + KI (aq) → AgI (s) + KNO₃ (aq)
E)AgNO₃ (aq) + KI (aq) → AgI (aq) + KNO₃ (s)

Question 66

Which of the following are weak electrolytes? HNO₃
HF
NH₃
LiBr

A)HNO₃, LiBr
B)HNO₃, HF, NH₃, LiBr
C)HF, LiBr
D)HF, NH₃
E)HNO₃, NH₃, LiBr

Question 67

What are the spectator ions in the reaction between KOH (aq)and HNO₃ (aq)?

A)K⁺ and H⁺
B)H⁺ and OH^-
C)K⁺ and NO₃^-
D)H⁺ and NO₃^-
E)OH^- only

Question 68

What are the spectator ions in the reaction between Mg(OH)₂ (aq)and HCl (aq)?

A)Mg⁺² and H⁺
B)H⁺ and OH^-
C)Mg⁺² and Cl^-
D)H⁺ and Cl^-
E)OH^- only

Question 69

Which of the following would require the largest volume of 0.100 M sodium hydroxide solution for neutralization?

A)10.0 mL of 0.0500 M phosphoric acid
B)20.0 mL of 0.0500 M nitric acid
C)5.0 mL of 0.0100 M sulfuric acid
D)15.0 mL of 0.0500 M hydrobromic acid
E)10.0 mL of 0.0500 M perchloric acid

Question 70

What volume (mL)of 7.48 × 10^-2 M perchloric acid can be neutralized with 115 mL of 0.244 M sodium hydroxide?

A)125
B)8.60
C)188
D)750
E)375

Question 71

The spectator ions in the reaction between aqueous chloric acid and aqueous barium hydroxide are ________.

A)OH^- and ClO₃^-
B)H⁺, OH^-, ClO₃^-, and Ba²⁺
C)H⁺ and OH^-
D)H⁺ and Ba²⁺
E)ClO₃^- and Ba²⁺

Question 72

________ is an oxidation reaction.

A)Ice melting in a soft drink
B)Table salt dissolving in water for cooking vegetables
C)Rusting of iron
D)The reaction of sodium chloride with lead nitrate to form lead chloride and sodium nitrate
E)Neutralization of HCl by NaOH

Question 73

When aqueous solutions of Pb(NO₃)₂ and NaCl are mixed, PbCl₂ precipitates. The balanced net ionic equation is ________.

A)Pb²⁺ (aq) + 2Cl^- (aq) → PbCl₂ (s)
B)Pb²⁺ (aq) + 2NO₃^- (aq) → Pb(NO₃)₂ (s)
C)Pb²⁺ (aq) + 2NO₃^- (aq) → Pb(NO₃)₂ (aq)
D)Pb(NO₃)₂ (aq) + 2NaCl (aq) → PbCl₂ (s) + 2NaNO₃ (aq)
E)Pb(NO₃)₂ (aq) + 2NaCl (aq) → PbCl₂ (aq) + 2NaNO₃ (s)

Question 74

What are the spectator ions in the reaction between KCl (aq)and AgNO₃ (aq)?

A)K⁺ and Ag⁺
B)Ag⁺ and Cl^-
C)K⁺ and NO₃^-
D)Ag⁺ and NO₃^-
E)K⁺ only

Question 75

The balanced net ionic equation for precipitation of CaCO₃ when aqueous solutions of Na₂CO₃ and CaCl₂ are mixed is ________.

A)2Na⁺ (aq) + CO₃^2- (aq) → Na₂CO₃ (aq)
B)2Na⁺ (aq) + 2Cl^- (aq) → 2NaCl (aq)
C)Na⁺ (aq) + Cl^- (aq) → NaCl (aq)
D)Ca⁺(aq) + CO₃^2- (aq) → CaCO₃ (s)
E)Na₂CO₃ (aq) + Ca (aq) → 2NaCl (aq) + CaCO₃ (s)

Question 76

When H₂SO₄ is neutralized by NaOH in aqueous solution, the net ionic equation is ________.

A)SO₄^2- (aq) + 2Na⁺ (aq) → Na₂SO₄ (aq)
B)SO₄^2- (aq) + 2Na⁺ (aq) → Na₂SO₄ (s)
C)H⁺ (aq) + OH^- (aq) → H₂O (l)
D)H₂SO₄ (aq) + 2OH^- (aq) → 2H₂O (l) + SO₄^2- (aq)
E)2H⁺ (aq) + 2NaOH (aq) → 2H₂O (l) + 2Na⁺ (aq)

Question 77

Which of the following are strong electrolytes? HCl
HC₂H₃O₂
NH₃
KCl

A)HCl, KCl
B)HCl, NH₃, KCl
C)HCl, HC₂H₃O₂, NH₃, KCl
D)HCl, HC₂H₃O₂, KCl
E)HC₂H₃O₂, KCl

Question 78

Combining aqueous solutions of BaI₂ and Na₂SO₄ affords a precipitate of BaSO₄. Which ions are spectator ions in the reaction?

A)Ba²⁺ only
B)Na⁺ only
C)Ba²⁺ and SO₄^2-
D)Na^{+ and I-}
E)SO₄^2- and I^-

Question 79

Which ions are spectator ions in the formation of a precipitate of AgCl via combining aqueous solutions of CoCl₂ and AgNO₃?

A)Co²⁺ and NO₃^-
B)NO₃^- and Cl^-
C)Co²⁺ and Ag⁺
D)Cl^-
E)NO₃^-

Question 80

A weak electrolyte exists predominantly as ________ in solution.

A)atoms
B)ions
C)molecules
D)electrons
E)an isotope