Deck 4: Aqueous Reactions and Solution Stoichiometry

Question 1

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

Answer 1

none of the above

Question 2

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

Answer 2

NiBr₂ and AgNO₃

Question 3

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

Answer 3

Mg₃(PO₄)₂

Question 4

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 5

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

A)HCl
B)Rb₂SO₄
C)Ar
D)KOH
E)NaCl

Question 6

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 H C₂H₃O₂ (aq)
E)NaOH (aq)and Fe(NO₃)₂ (aq)

Question 7

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 8

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

Question 9

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

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

Question 10

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 11

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)→ 3 H₂O (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)→ 3 H₂O (l)+ Al³⁺ (aq)
E)Al(OH)₃ (s)+ 3HNO₃ (aq)→ 3 H₂O (l)+ Al³⁺ (aq)+ NO₃^- (aq)

Question 12

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 13

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

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

Question 14

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)

Question 15

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

A)H⁺ (aq)+ HNO₃ (aq)+ 2OH^- (aq)→ 2 H₂O (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 16

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 17

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

A)Fe₃ (PO₄)₂
B)Fe(OH)₂
C)Fe(NO₃)₂
D)FeCO₃
E)FeS

Question 18

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 19

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

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

Question 20

Which one of the following compounds is insoluble in water?

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

Question 21

In which species does sulfur have the highest oxidation number?

A)S₈ (elemental form of sulfur)
B)H₂S
C)SO₂
D)H₂SO₃
E)K₂SO₄

Question 22

In which reaction does the oxidation number of hydrogen change?

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

Question 23

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 24

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

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

Question 25

In which species does nitrogen have the highest oxidation number?

A)N₂
B)NH₃
C)HNO₂
D)NO₂^-
E)NaNO₃

Question 26

In which reaction does the oxidation number of oxygen increase?

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

Question 27

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 28

Which compound has the atom with the highest oxidation number?

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

Question 29

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 30

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

A)KOH (aq)+ HC₂H₃O₂ (aq)→ OH^- (l)+ H C₂H₃O₂⁺ (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 31

Which one of the following solutions will have the greatest concentration of hydroxide ions?

A)0.300 M rubidium hydroxide
B)0.100 M magnesium hydroxide
C)0.100 M ammonia
D)0.100 M beryllium hydroxide
E)0.100 M hydrochloric acid

Question 32

Which one of the following is a weak acid?

A)HNO₃
B)HCl
C)HI
D)HF
E)HClO₄

Question 33

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 34

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 35

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 36

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)+ 3 H₂ (g)
E)Zn (s)+ 2HI (aq)→ ZnI₂ (aq)+ H₂ (g)

Question 37

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)→ 2 H₂O (l)+ Sr(NO₃)₂ (aq)
E)2HNO₃ (aq)+ Sr(OH)₂ (aq)→ Sr(NO₃)₂ (aq)+ 2 H₂ (g)

Question 38

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

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

Question 39

Which hydroxides are weak bases?

A)KOH, Ba(OH)₂
B)Sr(OH)₂, KOH, NaOH, Ba(OH)₂
C)KOH, NaOH
D)KOH, NaOH, Ba(OH)₂
E)None of these is a weak base.

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

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 42

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 43

What are the respective concentrations (M)of Cu⁺² and Cl^- afforded by dissolving 0.200 mol CuCl₂ in water and diluting to 345 mL?

A)0.200 and 0.200
B)0.580 and 1.16
C)0.200 and 0.400
D)1.16 and 2.32
E)0.580 and 0.290

Question 44

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 45

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 6.67 × 10^-2 mol of Ca²⁺.

Question 46

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

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

Question 47

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 48

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 49

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 50

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 51

Oxidation cannot occur without __________.

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

Question 52

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 53

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 54

Oxidation and __________ mean essentially the same thing.

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

Question 55

What are the respective concentrations (M)of Mg⁺² 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 56

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 57

Which solution has the same number of moles of NaOH as 50.00 mL of 0.100M solution of NaOH?

A)20.00 mL of 0.200M solution of NaOH
B)25.00 mL of 0.175M solution of NaOH
C)30.00 mL of 0.145M solution of NaOH
D)50.00 mL of 0.125M solution of NaOH
E)100.00 mL of 0.0500M solution of NaOH

Question 58

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 59

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 60

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 61

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 62

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 63

What volume (mL)of 0.135 M NaOH is required to neutralize 13.7 mL of 0.129 M HCl?

A)13.1
B)0.24
C)14.3
D)0.076
E)6.55

Question 64

What mass (g)of barium iodide is contained in 250 mL of a barium iodide solution that has an iodide ion concentration of 0.193 M?

A)9.44
B)18.9
C)0.024
D)0.048
E)37.7

Question 65

What mass (g)of AgBr is formed when 35.5 mL of 0.184 M AgNO₃ is treated with an excess of aqueous hydrobromic acid?

A)1.44
B)1.23
C)53.6
D)34.5
E)188

Question 66

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

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

Question 67

A 13.8 mL aliquot of 0.176 M H₃PO₄ (aq)is to be titrated with 0.110 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

A)7.29
B)22.1
C)199
D)66.2
E)20.9

Question 68

What mass (g)of CaF₂ is formed when 47.8 mL of 0.334 M NaF is treated with an excess of aqueous calcium nitrate?

A)1.25
B)0.472
C)2.49
D)0.943
E)0.623

Question 69

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 70

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 71

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 72

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

A)125
B)375
C)750
D)188
E)75.0

Question 73

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 74

__________ 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 75

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 76

What volume (ml)of a 3.45 M lead nitrate solution must be diluted to 450.0 ml to make a 0.990 M solution of lead nitrate?

A)129
B)109
C)101
D)56
E)45

Question 77

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

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

Question 78

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 79

A 36.3 mL aliquot of 0.0529 M H₂SO₄ (aq)is to be titrated with 0.0411 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

A)93.4
B)46.7
C)187
D)1.92
E)3.84

Question 80

What volume (mL)of a concentrated solution of sodium hydroxide (6.00 M)must be diluted to 200. mL to make a 1.50 M solution of sodium hydroxide?

A)0.0500
B)50.0
C)45.0
D)800.
E)0.800