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)

C

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)

D

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

A

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

A

Which one of the following compounds is insoluble in water?
A) Na2CO3
B) K2SO4
C) Fe(NO3)3
D) ZnS
E) AgNO3

D

Which one of the following compounds is insoluble in water?
A) K2SO4
B) Ca(C2H3O2)2
C) MgC2O4
D) ZnCl2
E) Mn(NO3)2

C

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)

D

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)

E

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)

A

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

E

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) + SO42- (aq)
B) H+ (aq) + HSO4- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+ (aq) + SO42-(aq)
C) SO42- (aq) + 2Na+ (aq) → 2Na+ (aq) + SO42-(aq)
D) H+ (aq) + OH- (aq) → H2O( l)
E) 2H+ (aq) + SO42- (aq) + 2Na+ (aq) + 2OH- (aq) → 2H2O (l) + 2Na+ (aq) + SO42- (aq)

D

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)

C

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

D

Which one of the following is a diprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid

E

Which one of the following is a triprotic acid?
A) nitric acid
B) chloric acid
C) phosphoric acid
D) hydrofluoric acid
E) sulfuric acid

C

Which one of the following is a weak acid?
A) HNO3
B) HCl
C) HI
D) HF
E) HClO4

D

Which of the following are weak acids?
A) HF, HBr
B) HI, HNO3, HBr
C) HI, HF
D) HF
E) none of the above

D

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+

C

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)

B

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)

D

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)

E

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)

B

Which compound has the atom with the highest oxidation number?
A) CaS
B) Na3N
C) MgSO3
D) Al(NO2)3
E) NH4Cl

C

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

A

Which of these metals will be oxidized by the ions of cobalt?
A) nickel
B) tin
C) iron
D) copper
E) silver

C

Which of these metals will be oxidized by the ions of aluminum?
A) magnesium
B) zinc
C) chromium
D) iron
E) nickel

A

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

E

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)

A

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)

C

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.

B

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)

D

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+

B

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

C

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

C

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

C

Oxidation cannot occur without ________.
A) acid
B) oxygen
C) water
D) air
E) reduction

E

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)

A

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)

B

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

C

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+.

D

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

E

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

A

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

C

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

A

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

D

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

C

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

C

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

B

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

A

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

C

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

D

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

D

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

D

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 × 10^-3

C

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

D

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

D

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

A

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

B

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

E

________ 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

C

A strong electrolyte is one that ________ completely in solution.
A) reacts
B) associates
C) disappears
D) ionizes

D

A weak electrolyte exists predominantly as ________ in solution.
A) atoms
B) ions
C) molecules
D) electrons
E) an isotope

C

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

A

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

D

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

C

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

C

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

C

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-

B

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 SO42-
D) Na+ and I-
E) SO42- and I-

D

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-

A

The balanced net ionic equation for the precipitation of calcium carbonate when aqueous solutions of Na2CO3 and CaCl2 are mixed is ________.
A) 2Na+ (aq) + CO32- (aq) → Na2CO3 (aq)
B) 2Na+ (aq) + 2Cl- (aq) → 2NaCl (aq)
C) Na+ (aq) + Cl- (aq) → NaCl (aq)
D) Ca+(aq) + CO32- (aq) → CaCO3 (s)
E) Na2CO3 (aq) + Ca (aq) → 2NaCl (aq) + CaCO3 (s)

D

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)

A

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)

A

When H2SO4 is neutralized by NaOH in aqueous solution, the net ionic equation is ________.
A) SO42- (aq) + 2Na+ (aq) → Na2SO4 (aq)
B) SO42- (aq) + 2Na+ (aq) → Na2SO4 (s)
C) H+ (aq) + OH- (aq) → H2O (l)
D) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq)
E) 2H+ (aq) + 2NaOH (aq) → 2H2O (l) + 2Na+ (aq)

C

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+

E

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+

C

The spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium hydroxide are ________.
A) Br- and Na+
B) OH-, Br-, and Na+
C) OH- and Br-
D) Na+ only
E) H+, OH-, Br-, and Na+

A

The spectator ions in the reaction between aqueous hydrobromic acid and aqueous ammonia are ________.
A) H+ and NH3
B) H+, Br-, NH3, and NH4+
C) Br- only
D) Br- and NH4+
E) H+, Br-, and NH4+

C

Which of the following are strong acids?

HI
HNO3
HF
HBr
A) HF, HBr
B) HI, HNO3, HF, HBr
C) HI, HF, HBr
D) HNO3, HF, HBr
E) HI, HNO3, HBr

E

Which hydroxides are strong bases?

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

D

A neutralization reaction between an acid and a metal hydroxide produces ________.
A) water and a salt
B) hydrogen gas
C) oxygen gas
D) sodium hydroxide
E) ammonia

A

Of the metals below, which will dissolve in an aqueous solution containing nickel ion?

aluminum
chromium
barium
tin
potassium
A) aluminum and chromium
B) All will dissolve except for tin
C) barium and potassium
D) tin only
E) potassium only

B

Which of these metals is the least easily oxidized?

Na
Au
Fe
Ca
Ag
A) Na
B) Au
C) Fe
D) Ca
E) Ag

B

Which of these metals is the most easily oxidized?

Cu
Au
Pt
Li
Hg
A) Li
B) Cu
C) Au
D) Pt
E) Hg

A

Of the following elements, ________ is the most difficult to oxidize.

Cu
Hg
Au
Ag
Na
A) Cu, Hg, and Au
B) Hg and Ag
C) Au only
D) Ag only
E) Na only

C

Of the following elements, ________ is the most easily oxidized.

lithium
zinc
hydrogen
aluminum
gold
A) aluminum
B) zinc
C) hydrogen
D) lithium
E) gold

D

Of the following elements, ________ is the least easily oxidized.

sodium
calcium
hydrogen
gold
platinum
A) sodium
B) gold
C) calcium
D) hydrogen
E) platinum

B

Based on the equations below, which metal is the most active?

Pb(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Pb (s)
Pb(NO3)2 (aq) + Ag (s) → No reaction
Cu(NO3)2 (aq) + Ni (s) → Ni(NO3)2 (aq) + Cu (s)

A) Ni
B) Ag
C) Cu
D) Pb
E) N

A

Which species is oxidized in the reaction below?

Au(s) + 3NO3-(aq) + 6H+(aq) → Au3+(aq) + NO(g) + 3H2O (l)

H+
N+5
O2-
H2O
Au
A) H+
B) N+5
C) Au
D) O2-
E) H2O

C

What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
A) 18
B) 0.16
C) 0.45
D) 27
E) 2.7 × 10^-2

C

How many moles of Co2+ are present in 0.200 L of a 0.400 M solution of CoI2?
A) 2.00
B) 0.500
C) 0.160
D) 0.0800
E) 0.0400

D

How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?
A) 0.436
B) 0.871
C) 1.31
D) 3.70
E) 7.40

B

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?
A) 0.436
B) 1.31
C) 0.145
D) 3.70
E) 11.1

B

What are the respective concentrations (M) of Na+ and SO42- afforded by dissolving 0.500 mol Na2SO4 in water and diluting to 1.33 L?
A) 0.665 and 0.665
B) 0.665 and 1.33
C) 1.33 and 0.665
D) 0.376 and 0.752
E) 0.752 and 0.376

E

What are the respective concentrations (M) of K+ and CO32- afforded by dissolving 0.530 mol K2CO3 in water and diluting to 1.50 L?
A) 0.707 and 0.353
B) 0.118 and 0.353
C) 0.353 and 0.707
D) 0.353 and 0.353
E) 0.707 and 0.707

A

Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a 0.874 M solution of sodium sulfide to a total volume of 250.0 mL.
A) 0.175
B) 4.37
C) 0.525
D) 0.350
E) 0.874

D

An aqueous ethanol solution (400 mL) was diluted to 4.00 L, giving a concentration of 0.0400 M. The concentration of the original solution was ________ M.
A) 0.400
B) 0.200
C) 2.00
D) 1.60
E) 4.00

A

The concentration (M) of an aqueous methanol produced when 0.200 L of a 2.00 M solution was diluted to 0.800 L is ________.
A) 0.800
B) 0.200
C) 0.500
D) 0.400
E) 8.00

C

The molarity (M) of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution is ________.
A) 0.0657
B) 1.85 × 10^-3
C) 1.85
D) 2.33
E) 0.634

C

The molarity (M) of an aqueous solution containing 85.1 g of sucrose (C12H22O11) in 128 mL of solution is ________.
A) 0.665
B) 0.0019
C) 0.249
D) 665
E) 1.94

E

The molarity (M) of an aqueous solution containing 129 g of glucose (C6H12O6) in 200 mL of solution is ________.
A) 0.716
B) 0.0036
C) 3.58
D) 0.645
E) 645

C

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6) in 35.5 mL of solution is ________.
A) 14.8
B) 2.12
C) 481
D) 0.0118
E) 11.8

E

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?
A) 0.105
B) 6.11
C) 3.21
D) 6.11 × 10³
E) 12.2

B

How many grams of potassium bromide are there in 250.0 mL of a 2.50 M aqueous solution of potassium bromide?
A) 0.625
B) 298
C) 74.4
D) 1.19 × 10³
E) 119

C

The molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500. mL is ________.
A) 0.0879
B) 87.9
C) 0.0218
D) 0.0115
E) 0.870

A

The molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500. mL is ________.
A) 0.129
B) 0.109
C) 0.438
D) 0.0175
E) 0.870

C

What is the concentration of chloride ions in a 0.349 M solution of sodium chloride?
A) 0.349 M
B) 0.0349 M
C) 0.0060 M
D) 0.175 M
E) 0.698 M

A

What is the concentration of nitrate ions in a 0.343 M solution of lead (II) nitrate?
A) 0.686 M
B) 0.172 M
C) 1.03 M
D) 0.0343 M
E) 0.343 M

A

The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.
A) 0.193 M
B) 0.386 M
C) 0.0965 M
D) 0.579 M
E) 0.0643 M

B

The concentration of species in 100 mL of a 3.47 M solution of sodium iodide is ________ M sodium ion and ________ M iodide ion.
A) 0.0347, 0.0347
B) 0.347, 0.347
C) 0.347, 0.694
D) 0.694, 0.347
E) 3.47, 3.47

E

When 0.344 mol of HCl is combined with enough water to make a 450.0 mL solution, the concentration of HCl is ________ M.
A) 7.64 × 10-4
B) 0.155
C) 1.31
D) 0.764
E) 0.344

D

In a titration of 35.00 mL of 0.737 M H2SO4, ________ mL of a 0.827 M KOH solution is required for neutralization.
A) 35.0
B) 31.2
C) 25.8
D) 62.4
E) 39.3

D

Calculate the mass percent of sulfuric acid in a solid sample given that a 0.8390 g sample of that solid required 32.22 mL of 0.2012 M NaOH for neutralization.
A) 62.11
B) 2.64
C) 37.89
D) 75.78
E) 1.27

C

If an unknown sample contains 39.04% sulfuric acid by mass, then a 0.9368 g of that sample would require ________ mL of 0.2389 M NaOH for neutralization.
A) 31.22
B) 39.98
C) 7.80
D) 79.96
E) 15.61

A

A 17.5 mL sample of an acetic acid (CH3CO2H) solution required 29.6 mL of 0.250 M NaOH for neutralization. The concentration of acetic acid was ________ M.
A) 0.296
B) 0.423
C) 0.591
D) 0.105
E) 129.5

B

A 25.5 mL aliquot of HCl (aq) of unknown concentration was titrated with 0.113 M NaOH (aq). It took 51.2 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
A) 1.02
B) 0.114
C) 0.454
D) 0.113
E) 0.227

E

A 31.5 mL aliquot of HNO3 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
A) 0.0102
B) 0.0051
C) 0.0204
D) 0.227
E) 1.02

A

A 31.5 mL aliquot of H2SO4 (aq) of unknown concentration was titrated with 0.0134 M NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration (M) of the acid was ________.
A) 0.0102
B) 0.00508
C) 0.0204
D) 0.102
E) 0.227

B

Of the species below, only ________ is not an electrolyte.
A) HBr
B) LiCl
C) Ne
D) KOH
E) NaNO3

C

What is the formula for phosphoric acid?
A) H3PO4
B) H2PO4
C) H4PO4
D) H3PO3
E) none of the above

A

The total concentration of ions in a 0.250 M solution of HCl is ________.
A) 0
B) 0.125 M
C) 0.250 M
D) 0.500 M
E) 0.750 M

D

Which hydroxides are weak bases?
A) KOH
B) Ba(OH)2
C) RbOH
D) CsOH
E) None of these choices are weak bases.

E

Which of the following is soluble in water at 25 °C?
A) AgNO3
B) Hg2Cl2
C) PbCl2
D) Ag2S
E) AgCl

A

With which of the following will the Potassium ion form an insoluble salt?
A) Phosphate
B) Sulfate
C) Sulfide
D) Iodide
E) Potassium will form soluble salts with all choices.

E

Which one of the following solutions will have the greatest concentration of hydroxide ions?
A) 1.10 M rubidium hydroxide
B) 0.368 M calcium hydroxide
C) 0.368 M ammonium hydroxide
D) 0.368 M potassium hydroxide
E) 0.368 M sulfuric acid

A

In which species does bromine have an oxidation number of zero?
A) HBrO4
B) NaBrO3
C) Br-
D) Br2
E) HBr

D

In which species does nitrogen have an oxidation number of zero?
A) N2
B) NaNO3
C) HNO2
D) NO2-
E) NH3

A

In which species does nitrogen have the highest oxidation number?
A) NaNO3
B) HNO2
C) NO2-
D) NH3
E) N2

A

What is the concentration (M) of potassium ions in 153 mL of a 1.25 M K3PO4 solution?

3.75

How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.250 M NaOH solution?
A) 0.00313
B) 0.00625
C) 20
D) 5.00
E) 0.125

D

How many grams of NaOH (MW = 40.0) are there in 200.0 mL of a 0.175 M NaOH solution?
A) .00219
B) 114
C) 1.40
D) 0.0350
E) 14.0

C

How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH?
A) 0.0096
B) 430
C) 2.4
D) 9.6
E) 4.3

D

How many moles of chloride ions are in 0.500 L of a 0.250 M solution of AlCl3?
A) 0.125
B) 0.0500
C) 0.375
D) 0.167
E) 0.750

C

What is the concentration (M) of KCl in a solution made by mixing 25.0 mL of 0.100 M KCl with 50.0 mL of 0.100 M KCl?
A) 0.100
B) 0.0500
C) 0.0333
D) 0.0250
E) 125

A

What is the concentration (M) of CH3OH in a solution prepared by dissolving 34.4 g of CH3OH in sufficient water to give exactly 230 mL of solution?
A) 11.9
B) 0.00159
C) 1.59
D) 4.67
E) 5.31

D

What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give exactly 330. mL of solution?
A) 11.9
B) 1.11
C) 0.00159
D) 1.59
E) 0.0841

B

How many grams of H3PO4 are in 145 mL of a 3.50 M solution of H3PO4?
A) 0.508
B) 49.7
C) 20.0
D) 4.90
E) 612

B

How many grams of H3PO4 are in 175 mL of a 4.00 M solution of H3PO4?
A) 0.700
B) 20.0
C) 68.6
D) 4.90
E) 612

C

A solution of CH3F is prepared by dissolving 17.2 g of CH3F in sufficient water to give exactly 300 mL of solution. What is the concentration (M) of the newly prepared CH3F solution?

1.68

325 mL of a 5.50 M phosphoric acid solution was prepared for laboratory. How many grams of phosphoric acid was in this solution.

175

A KCl solution was prepared by dissolving 9.3 g of KCl in sufficient water to give 350 mL of solution. What is the concentration (M) of the newly prepared KCl solution?

0.36

How many grams of an unknown substance with a molar mass of 40.0 are there in 500.0 mL of a 0.175 M solution of the unknown?

3.50

How many grams of hydrazine N2H4 must be added to a solvent to prepare 375 mL of a solution that is 5.5 M hydrazine?

66

How many moles of chloride ions are present in 0.300 L of a 0.150 M solution of AlCl3?

0.135

How many moles of Cu2+ ions are present in 0.100 L of a 0.100 M solution of CuCl2?

0.0100

What are the respective concentrations (M) of Cu2+ and Cl- afforded by dissolving 0.871 mol CuCl2 in water and diluting to 259 mL?
A) 3.36 and 6.73
B) 0.00336 and 3.36
C) 0.00336 and 0.00336
D) 3.36 and 3.36
E) 0.297 and 0.113

A

What mass (g) of barium iodide is contained in 188mL of a barium iodide solution that has an iodide ion concentration of 0.532 M?
A) 19.6
B) 39.1
C) 19,600
D) 39,100
E) 276

A

What is the concentration (M) of potassium ions in a solution made by diluting 40.0 mL of a 0.474 M solution of potassium sulfide to a total volume of 300 mL.

0.126

What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 185.6 mL to make a 3.23 M solution of sodium hydroxide?
A) 99.9
B) 3600
C) 287
D) 0.104
E) 0.0100

A

What volume (mL) of a 5.45 M lead nitrate solution must be diluted to 820.7 mL to make a 1.41 M solution of lead nitrate?
A) 212
B) 6310
C) 3170
D) 0.00936
E) 0.00471

A

How many milliliters of a 14.2 M HCl solution is needed to prepare 0.715 L solution of HCl with a concentration of 0.350 M?
A) 0.0568
B) 3.55
C) 56.8
D) 17.6
E) 0.0176

D

A stock solution of HNO3 is prepared and found to contain 12.7 M of HNO3. If 25.0 mL of the stock solution is diluted to a final volume of 0.500 L, the concentration of the diluted solution is ________ M.
A) 0.254
B) 1.57
C) 0.635
D) 635
E) 254

C

Pure acetic acid (HC2H3O2) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 20.00 mL of glacial acetic acid at 25 °C in sufficient water to give 500.0 mL of solution. The density of glacial acetic acid at 25 °C is 1.05 g/mL.
A) 2.52 × 10³
B) 42.0
C) 0.0420
D) 0.699
E) 6.99 × 10-⁴

D

What is the molarity of iodide ion in a solution prepared by mixing 20.0 mL of 0.100 M HI and 5.00 mL of 0.200 M KI?
A) 0.180
B) 8.33
C) 0.120
D) 1.50
E) 0.0400

C

What mass (g) of AgBr is formed when 57.8 mL of 0.423 M AgNO3 is treated with an excess of aqueous hydrobromic acid?
A) 4.59
B) 2.30
C) 25.7
D) 0.130
E) 25,700

A

0.400 g of solid NaCl is added to 50 mL of a 0.100 M MgCl2 solution. Assuming the final volume does not change, what is the molarity of chloride ion in the final solution?
A) 0.237
B) 0.108
C) 0.208
D) 0.337
E) 0.137

D

Calculate the number of grams of unknown solute (MW = 56.105 g/mol) in 250.0 mL of a 0.169 M solution.
A) 2.37
B) 83.0
C) 0.753
D) 2.37 × 10³
E) 7.53 × 10^-4

A

How much CaF2 (g) is formed when 15.7 mL of 0.612 M KF reacts with an excess of aqueous calcium bicarbonate?
A) 0.750
B) 750
C) 0.123
D) 0.375
E) 2000

D

What is the molarity of a NaOH solution if 15.5 mL of a 0.220 M H2SO4 solution is required to neutralize a 25.0-mL sample of the NaOH solution?
A) 0.273
B) 0.355
C) 0.710
D) 42.6
E) 0.136

A

How many milliliters of 1.500 M aqueous KI solution must be added to an aqueous solution containing 0.100 mol of Pb(NO3)2 to completely precipitate the lead?
A) 7.50 × 10^-3
B) 66.7
C) 0.0667
D) 0.133
E) 133

E

Silver ions can be precipitated from aqueous solutions by the addition of aqueous chloride:

Ag+ (aq) + Cl- (aq) → AgCl (s)

Silver chloride is virtually insoluble in water so that the reaction appears to go to completion. How many grams of solid NaCl must be added to 25.0 mL of 0.149 M AgNO3 solution to completely precipitate the silver?
A) 9.81
B) 6.37 × 10^-5
C) 0.218
D) 0.102
E) 0.633

C

How many milliliters of 0.188 M HClO4 solution are needed to neutralize 50.00 mL of 0.0832 M NaOH?
A) 0.782
B) 8.85 × 10-3
C) 113
D) 0.0452
E) 22.1

E

What volume (mL) of 0.102 M NaOH is required to neutralize 17.1 mL of 0.443 M HCl?
A) 74.3
B) 3.94
C) 0.773
D) 0.0135
E) 0.000773

A

What volume (mL) of 0.201 M potassium hydroxide will it take to reach the equivalence point in a 16.3 mL aliquot of 0.226 M triprotic acid?
A) 2.22
B) 18.3
C) 55.0
D) 6.11
E) 120

C

What is the concentration (M) of 39.88 mL of an unknown NaOH solution if it required 46.08 mL of 0.6592 M HCl to neutralize?
A) 0.7617
B) 2788
C) 1211
D) 1.313
E) 1.211

A

A titration reached the equivalence point when 16.1 mL of 0.209 M H2SO4 (aq) was added to 12.0 mL of NaOH (aq) of unknown concentration. What is the concentration (M) of this unknown NaOH solution?
A) 0.561
B) 80.8
C) 0.280
D) 0.140
E) 3.21

A

The solvent in an aqueous solution is ________.`

water

If it took 49.33 mL of 0.2454 M KOH solution to neutralize 35.0 mL of arsenic acid (H3AsO4), what is the concentration (M) of the arsenic acid solution?

0.1153

How many moles of CaCl2 are formed in the neutralization of 138 mL of 0.352 M Ca(OH)2 with aqueous HCl?

0.0486

Ca(OH)2 is a strong base.

true

The compound HClO4 is a weak acid.

false

HNO2 is a strong acid.

false

The compound NH4Cl is a weak acid.

true

Ammonia is a strong base.

false