Deck 4: Reactions in Aqueous Solution

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 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 2

NaOH (aq)and Fe(NO₃)₂ (aq)

Question 3

Which one of the following compounds is insoluble in water?

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

Answer 3

MgC₂O₄

Question 4

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 5

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 6

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 7

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 8

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 9

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 10

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 11

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 12

Which one of the following compounds is insoluble in water?

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

Question 13

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 14

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 15

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 16

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 17

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 18

Which one of the following is a weak acid?

A)HNO₃
B)HCl
C)HI
D)HF
E)HClO₄

Question 19

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 20

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 21

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 22

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

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

Question 23

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 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

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 26

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 27

The process by which metal in the presence of air and water is converted into rust is known as ________.

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

Question 28

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 29

Which compound has the atom with the highest oxidation number?

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

Question 30

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 31

Oxidation cannot occur without ________.

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

Question 32

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 33

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 34

Which of the following reactions is not spontaneous?

A)Cu (s)+ 2HCl (aq)→ CuCl₂ (aq)+ H₂ (g)
B)Mg (s)+ 2HCl (aq)→ MgCl₂ (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 35

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 36

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 37

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 38

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 39

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

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

Question 40

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 41

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)0.0264
B)176
C)26.4
D)29.3
E)33.3

Question 42

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)14.1
B)1.15
C)127
D)107
E)38.8

Question 43

Which of the following 0.300 M solutions would contain the highest concentration of potassium ions?

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

Question 44

Which solution has the same number of moles of HCl as 25.0 mL of 0.200 M solution of HCl?

A)12.5 mL of 0.400 M solution of HCl
B)25.0 mL of 0.185 M solution of HCl
C)45.0 mL of 0.155 M solution of HCl
D)50.0 mL of 0.150 M solution of HCl
E)100.0 mL of 0.500 M solution of HCl

Question 45

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 46

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 47

A 0.355 M K₂SO₄ solution can be prepared by ________.

A)dilution of 500.0 mL of 1.00 M K₂SO₄ to 1.00 L
B)dissolving 46.7 g of K₂SO₄ in water and diluting to a total volume of 250.0 mL
C)dissolving 46.7 g of K₂SO₄ in water and diluting to 500.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL
D)dilution of 1.00 mL of 0.355 M K₂SO₄ to 1.00 L
E)diluting 46.7 mL of 1.90 M K₂SO₄ solution to 250.0 mL

Question 48

What are the respective concentrations (M)of Mg²⁺ and Cl^- afforded by dissolving 0.325 mol MgCl₂ in water and diluting to 250 mL?

A)0.0013 and 0.0013
B)0.0013 and 0.0026
C)1.30 and.1.30
D)1.30 and 2.60
E)2.60 and 2.60

Question 49

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)0.129
B)0.190
C)0.173
D)0.207
E)0.215

Question 50

A 650 mL sodium bromide solution has a bromide ion concentration of 0.245 M.What is the mass (g)of sodium bromide in solution?

A)103
B)0.00155
C)16400
D)16.4
E)0.159

Question 51

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 52

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 53

Mixing 1.00 mL of an aqueous solution with 9.00 mL of water represents a ________.

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

Question 54

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 55

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)1.25
B)0.11
C)1.75
D)0.070
E)1.75 ×

Question 56

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

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

Question 57

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)129.3 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 58

All of the following are true concerning 2.00 L of 0.100 M solution of Ca₃(PO₄)₂ except for ________.

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

Question 59

A one-hundredfold dilution of an enzymatic buffer solution can be obtained by using ________.

A)1 part sample and 100 parts diluent
B)99 parts sample and 1 part diluent
C)1 part sample and 99 parts diluent
D)100 parts sample and 1 part diluent
E)9 parts sample and 1 part diluent

Question 60

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 61

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 62

________ 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 63

A weak electrolyte exists predominantly as ________ in solution.

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

Question 64

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 65

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 66

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 67

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 68

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 69

When aqueous solutions of AgNO₃ and KI are mixed,silver iodide 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 70

The spectator ions in the reaction between aqueous hydrochloric acid and aqueous calcium hydroxide are ________.

A)OH^- and Cl^-
B)H⁺, OH^-, Cl^-, and Ca²⁺
C)Cl^{- and Ca2+}
D)H⁺ and OH^-
E)H⁺ and Ca²⁺

Question 71

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 NO}₃^-
D)H⁺ and NO₃^-
E)OH^- only

Question 72

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 73

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 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

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 76

When aqueous solutions of Pb(NO₃)₂ and NaCl are mixed,lead(II)chloride 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 77

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

A)Mg²⁺ and H⁺
B)H⁺ and OH^-
C)Mg²⁺ and Cl^-
D)H⁺ and Cl^-
E)OH^- only

Question 78

A strong electrolyte is one that ________ completely in solution.

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

Question 79

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 80

The balanced net ionic equation for the precipitation of calcium carbonate 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)