Question 1

Which one of the following mixtures is not a solution?

Accepted Answer

A) white vinegar 
B) bottled spring water 
C) filtered dry air 
D) clear tea 
E) pulpy orange juice 
A) white vinegar 
B) bottled spring water 
C) filtered dry air 
D) clear tea 
E) pulpy orange juice

Question 2

Solutions of hydrochloric acid, sulfuric acid, and phosphoric acid with equal concentrations and volumes are neutralized by a solution of sodium hydroxide. If it takes 25.0 mL of the sodium hydroxide solution to neutralize the hydrochloric acid, what volume of the sodium hydroxide solution does it take to neutralize each of the other two solutions? Explain.

Accepted Answer

It takes 50.0 mL for sulfuric acid and 7

Question 3

Nitrogen-fixing bacteria and plants are capable of converting atmospheric nitrogen (N2) to ammonia (NH3). This process is an example of ________

Accepted Answer

A) an acid-base reaction. 
B) a precipitation reaction. 
C) an oxidation reaction. 
D) a reduction reaction. 
E) ion exchange. 
A) an acid-base reaction. 
B) a precipitation reaction. 
C) an oxidation reaction. 
D) a reduction reaction. 
E) ion exchange.

Question 4

Which picture best represents an atomic-level view of hydrochloric acid, which is a strong acid, in aqueous solution (water molecules not shown)?

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 5

Lead is the least toxic metal ion to fish compared to zinc, copper, and mercury ions. Fish can tolerate a lead concentration slightly above 0.850 mM. What is this concentration in ppm? Assume the density of the water is 1.00 g/mL.

Accepted Answer

A) 176 ppm 
B) 83 ppm 
C) 352 ppm 
D) 0.176 ppm 
E) 0.352 ppm 
A) 176 ppm 
B) 83 ppm 
C) 352 ppm 
D) 0.176 ppm 
E) 0.352 ppm

Question 6

A homogeneous mixture of two or more substances is called ________

Accepted Answer

A) a compound. 
B) an electrolyte. 
C) a solution. 
D) a solvent. 
E) a mess. 
A) a compound. 
B) an electrolyte. 
C) a solution. 
D) a solvent. 
E) a mess.

Question 7

What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL of solution containing 10.79 g of Ag+?

Accepted Answer

A) 10.8 g 
B) 21.6 g 
C) 28.6 g 
D) 7.2 g 
E) 14.3 g 
A) 10.8 g 
B) 21.6 g 
C) 28.6 g 
D) 7.2 g 
E) 14.3 g

Question 8

Chlorine gas easily gains two electrons to form two chloride ions. In this process, chlorine is ________

Accepted Answer

A) reduced. 
B) oxidized. 
C) ionized. 
D) complexed. 
E) both ionized and oxidized. 
A) reduced. 
B) oxidized. 
C) ionized. 
D) complexed. 
E) both ionized and oxidized.

Question 9

If the molar concentration of sodium sulfate (Na2SO4) is 0.10 M, what is the concentration of sodium ion?

Accepted Answer

A) 0.10 M 
B) 0.050 M 
C) 0.20 M 
D) 0.30 M 
E) 0.40 M 
A) 0.10 M 
B) 0.050 M 
C) 0.20 M 
D) 0.30 M 
E) 0.40 M

Question 10

Which picture best represents an atomic-level view of a weak electrolyte solution (water molecules not shown)?

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 11

Which one of the following statements is not correct?

Accepted Answer

A) Solubility of a substance is the maximum amount that dissolves in a specified amount of solvent at a given temperature. 
B) A saturated solution contains the maximum amount of solute dissolved in a solvent at equilibrium. 
C) A supersaturated solution contains more solute than predicted by the solubility of the substance. 
D) A supersaturated solution can be produced by slowly decreasing the temperature. 
E) A supersaturated solution can be produced by slowly adding the solvent. 
A) Solubility of a substance is the maximum amount that dissolves in a specified amount of solvent at a given temperature. 
B) A saturated solution contains the maximum amount of solute dissolved in a solvent at equilibrium. 
C) A supersaturated solution contains more solute than predicted by the solubility of the substance. 
D) A supersaturated solution can be produced by slowly decreasing the temperature. 
E) A supersaturated solution can be produced by slowly adding the solvent.

Question 12

What is the difference between a strong acid and a weak acid?

Accepted Answer

A strong acid ionize

Question 13

Identify which of the following compounds are insoluble in water.

Accepted Answer

A)  K2S 
B)  AgCl 
C)  Mg(OH)2 
D)  (NH4)2CO3 
E)  PbSO4 
A)  K2S 
B)  AgCl 
C)  Mg(OH)2 
D)  (NH4)2CO3 
E)  PbSO4

Question 14

Chalk contains calcium carbonate. What would be the best solution for cleaning a sidewalk that a preschool class covered with smiling suns, flowers, birds, rainbows, and houses using sidewalk chalk?

Accepted Answer

A) ammonia 
B) plain water 
C) vinegar 
D) paint thinner 
E) olive oil 
A) ammonia 
B) plain water 
C) vinegar 
D) paint thinner 
E) olive oil

Question 15

Determine the molar concentration of ethanol (C2H6O) in a wine that is 14% ethanol by mass. The density of this wine is 0.93 g/cm3.

Accepted Answer

A) 0.063 M 
B) 13.0 M 
C) 0.14 M 
D) 2.8 M 
E) 3.0 M 
A) 0.063 M 
B) 13.0 M 
C) 0.14 M 
D) 2.8 M 
E) 3.0 M

Question 16

Which of the following compounds is a strong electrolyte?

Accepted Answer

A) methane, CH4 
B) methanol, CH3OH 
C) ammonia, NH3 
D) hydrofluoric acid, HF 
E) potassium chloride, KCl 
A) methane, CH4 
B) methanol, CH3OH 
C) ammonia, NH3 
D) hydrofluoric acid, HF 
E) potassium chloride, KCl

Question 17

Lead sinkers used for saltwater fishing do not react with sodium ions in the water. From this we can infer that ________

Accepted Answer

A) lead can reduce sodium ions. 
B) sodium ions can reduce lead. 
C) lead can oxidize sodium ions. 
D) sodium ions cannot oxidize lead. 
E) sodium ions cannot reduce lead. 
A) lead can reduce sodium ions. 
B) sodium ions can reduce lead. 
C) lead can oxidize sodium ions. 
D) sodium ions cannot oxidize lead. 
E) sodium ions cannot reduce lead.

Question 18

Based on the activity series shown below, predict which metal or metal ions from the table could reduce Ba2+ ions.

Accepted Answer

If Ba²⁺ is reduced, we are lo

Question 19

If 120 g of NaOH were used to prepare 500 mL of solution, what would the concentration be?

Accepted Answer

A) 1 M 
B) 2 M 
C) 3 M 
D) 4 M 
E) 6 M 
A) 1 M 
B) 2 M 
C) 3 M 
D) 4 M 
E) 6 M

Question 20

Water-soluble toxic chromium compounds are waste products of electroplating operations, but the chromium can be precipitated as Cr(OH)3 to remediate the water. How much 1.0 M NaOH solution is needed to remove the chromium from 100 L of a solution that is 0.001 M in Cr3+?

Accepted Answer

A) 100 mL 
B) 300 mL 
C) 10 L 
D) 30 L 
E) 33 L 
A) 100 mL 
B) 300 mL 
C) 10 L 
D) 30 L 
E) 33 L

Exam 4: Solution Chemistry: The Hydrosphere

Which one of the following mixtures is not a solution?

Nitrogen-fixing bacteria and plants are capable of converting atmospheric nitrogen (N2) to ammonia (NH3). This process is an example of ________

Which picture best represents an atomic-level view of hydrochloric acid, which is a strong acid, in aqueous solution (water molecules not shown)?

Lead is the least toxic metal ion to fish compared to zinc, copper, and mercury ions. Fish can tolerate a lead concentration slightly above 0.850 mM. What is this concentration in ppm? Assume the density of the water is 1.00 g/mL.

A homogeneous mixture of two or more substances is called ________

What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL of solution containing 10.79 g of Ag+?

Chlorine gas easily gains two electrons to form two chloride ions. In this process, chlorine is ________

If the molar concentration of sodium sulfate (Na2SO4) is 0.10 M, what is the concentration of sodium ion?

Which picture best represents an atomic-level view of a weak electrolyte solution (water molecules not shown)?

Which one of the following statements is not correct?

What is the difference between a strong acid and a weak acid?

Identify which of the following compounds are insoluble in water.

Chalk contains calcium carbonate. What would be the best solution for cleaning a sidewalk that a preschool class covered with smiling suns, flowers, birds, rainbows, and houses using sidewalk chalk?

Determine the molar concentration of ethanol (C2H6O) in a wine that is 14% ethanol by mass. The density of this wine is 0.93 g/cm3.

Which of the following compounds is a strong electrolyte?

Lead sinkers used for saltwater fishing do not react with sodium ions in the water. From this we can infer that ________

Based on the activity series shown below, predict which metal or metal ions from the table could reduce Ba2+ ions.

If 120 g of NaOH were used to prepare 500 mL of solution, what would the concentration be?

Water-soluble toxic chromium compounds are waste products of electroplating operations, but the chromium can be precipitated as Cr(OH)3 to remediate the water. How much 1.0 M NaOH solution is needed to remove the chromium from 100 L of a solution that is 0.001 M in Cr3+?

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Nitrogen-fixing bacteria and plants are capable of converting atmospheric nitrogen (N₂) to ammonia (NH₃). This process is an example of ________

What mass of silver chloride will be recovered if excess sodium chloride is added to 500 mL of solution containing 10.79 g of Ag⁺?

If the molar concentration of sodium sulfate (Na₂SO₄) is 0.10 M, what is the concentration of sodium ion?

Determine the molar concentration of ethanol (C₂H₆O) in a wine that is 14% ethanol by mass. The density of this wine is 0.93 g/cm³.

Based on the activity series shown below, predict which metal or metal ions from the table could reduce Ba²⁺ ions.

Water-soluble toxic chromium compounds are waste products of electroplating operations, but the chromium can be precipitated as Cr(OH)₃ to remediate the water. How much 1.0 M NaOH solution is needed to remove the chromium from 100 L of a solution that is 0.001 M in Cr³⁺?