Question 1

Which homogeneous mixture is opaque and has particles large enough to be filtered?

Accepted Answer

A) colloid 
B) solution 
C) suspension 
D) both colloids and suspensions 
E) none of the above 
A) colloid 
B) solution 
C) suspension 
D) both colloids and suspensions 
E) none of the above

Question 2

What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

Accepted Answer

A) 1.2 M 
B) 1.5 M 
C) 6.0 M 
D) 24 M 
E) 30 M 
A) 1.2 M 
B) 1.5 M 
C) 6.0 M 
D) 24 M 
E) 30 M

Question 3

Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?

Accepted Answer

A) 4 mL of alcohol is mixed with enough water to make 250 mL of solution. 
B) 10 mL of alcohol is mixed with enough water to make 250 mL of solution. 
C) 4 mL of alcohol is mixed with 250 mL of water. 
D) 10 mL of alcohol is mixed with 250 mL of water. 
E) none of the above 
A) 4 mL of alcohol is mixed with enough water to make 250 mL of solution. 
B) 10 mL of alcohol is mixed with enough water to make 250 mL of solution. 
C) 4 mL of alcohol is mixed with 250 mL of water. 
D) 10 mL of alcohol is mixed with 250 mL of water. 
E) none of the above

Question 4

The number of components in a solution is ________.

Accepted Answer

A) at least 2 
B) 3 
C) 4 
D) 5 
E) 6 
A) at least 2 
B) 3 
C) 4 
D) 5 
E) 6

Question 5

All of the following statements describing solutions are true except

Accepted Answer

A) making a solution involves a physical change. 
B) solutions are homogeneous. 
C) the particles in a solution are atomic or molecular in size. 
D) solutions are colorless. 
E) solutions are transparent. 
A) making a solution involves a physical change. 
B) solutions are homogeneous. 
C) the particles in a solution are atomic or molecular in size. 
D) solutions are colorless. 
E) solutions are transparent.

Question 6

A supersaturated solution

Accepted Answer

A) contains as much solvent as it can hold 
B) contains no double bonds 
C) contains dissolved solute in equilibrium with undissolved solid 
D) will rapidly precipitate if a seed crystal is added. 
E) none of the above 
A) contains as much solvent as it can hold 
B) contains no double bonds 
C) contains dissolved solute in equilibrium with undissolved solid 
D) will rapidly precipitate if a seed crystal is added. 
E) none of the above

Question 7

How many grams of FeSO4 are present in a 20.0 mL sample of a 0.500 M solution?

Accepted Answer

A) 65.8 g 
B) 6.08 g 
C) 3.04 g 
D) 1.52 g 
E) 0.760 g 
A) 65.8 g 
B) 6.08 g 
C) 3.04 g 
D) 1.52 g 
E) 0.760 g

Question 8

What is the % (w/v)concentration of a solution containing 8.0 grams of alcohol in 50.0 mL of solution?

Accepted Answer

A) 2.0% 
B) 4.0% 
C) 8.0% 
D) 16% 
E) 50% 
A) 2.0% 
B) 4.0% 
C) 8.0% 
D) 16% 
E) 50%

Question 9

Adding solute to a solution increases each of the following except

Accepted Answer

A) molality. 
B) boiling point. 
C) osmotic pressure. 
D) freezing point. 
A) molality. 
B) boiling point. 
C) osmotic pressure. 
D) freezing point.

Question 10

Considering 0.10 M solutions of each substance,which contains the smallest concentration of ions?

Accepted Answer

A) (NH4)3PO4 
B) Ca(NO3)2 
C) FeSO4 
D) K2CO3 
E) Na2SO4 
A) (NH4)3PO4 
B) Ca(NO3)2 
C) FeSO4 
D) K2CO3 
E) Na2SO4

Question 11

Which of the following should be immiscible with carbon tetrachloride,CCl4?

Accepted Answer

A) C6H12 
B) CH3CH2OH 
C) Br2 
D) C3H8 
E) C4H10 
A) C6H12 
B) CH3CH2OH 
C) Br2 
D) C3H8 
E) C4H10

Question 12

How many g of Fe(NO3)3 are present in a 20.0 mL sample of a 0.500 M solution?

Accepted Answer

A) 2.14 g 
B) 9.68 g 
C) 4.84 g 
D) 2.42 g 
E) 1.21 g 
A) 2.14 g 
B) 9.68 g 
C) 4.84 g 
D) 2.42 g 
E) 1.21 g

Question 13

Considering 1.0 M solutions of each substance,which contains the largest concentration of ions?

Accepted Answer

A) K2SO4 
B) FeCl3 
C) NaOH 
D) NH3 
E) KCl 
A) K2SO4 
B) FeCl3 
C) NaOH 
D) NH3 
E) KCl

Question 14

How many grams of CaCl2 are needed to prepare 125 mL of a 1.50 M solution?

Accepted Answer

A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g 
A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g

Question 15

Which statement about solubility is not true?

Accepted Answer

A) No additional solute will dissolve in a saturated solution. 
B) A supersaturated solution is unstable. 
C) Solubility of ionic solids increases greatly with temperature. 
D) In a solution containing excess solute,an equilibrium exists between dissolved and undissolved solute. 
E) The solubility of substances is measured as g solute/100 mL solvent. 
A) No additional solute will dissolve in a saturated solution. 
B) A supersaturated solution is unstable. 
C) Solubility of ionic solids increases greatly with temperature. 
D) In a solution containing excess solute,an equilibrium exists between dissolved and undissolved solute. 
E) The solubility of substances is measured as g solute/100 mL solvent.

Question 16

What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make 1.50 L of solution?

Accepted Answer

A) 0.0313 M 
B) 0.556 M 
C) 0.800 M 
D) 1.28 M 
E) 32.0 M 
A) 0.0313 M 
B) 0.556 M 
C) 0.800 M 
D) 1.28 M 
E) 32.0 M

Question 17

The exothermic step in the dissolution of NaCl in water is

Accepted Answer

A) the separation of the ions in the salt. 
B) the separation of the water molecules. 
C) solvation (hydration)of the ions from the salt. 
D) separation of the ions in the salt and the separation of the water molecules. 
A) the separation of the ions in the salt. 
B) the separation of the water molecules. 
C) solvation (hydration)of the ions from the salt. 
D) separation of the ions in the salt and the separation of the water molecules.

Question 18

Which solution will have the highest boiling point?

Accepted Answer

A) 0.050 M KNO3 
B) 0.075 M CaCl2 
C) 0.025 M NH4NO3 
D) 0.020 M Na3PO4 
E) 0.10 M C6H12O6 
A) 0.050 M KNO3 
B) 0.075 M CaCl2 
C) 0.025 M NH4NO3 
D) 0.020 M Na3PO4 
E) 0.10 M C6H12O6

Question 19

How many g of CaCl2 are needed to prepare 500.mL of a 0.375 M solution?

Accepted Answer

A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g 
A) 0.188 g 
B) 1.69 g 
C) 3.00 g 
D) 20.8 g 
E) 37.0 g

Question 20

A 20.0 mL sample of CuSO4 was evaporated to dryness,leaving 0.967 g of residue.What was the molarity of the original solution?

Accepted Answer

A) 48.4 M 
B) 0.0207 M 
C) 0.0484 M 
D) 0.303 M 
E) 0.433 M 
A) 48.4 M 
B) 0.0207 M 
C) 0.0484 M 
D) 0.303 M 
E) 0.433 M

Exam 9: Solutions

Which homogeneous mixture is opaque and has particles large enough to be filtered?

What is the final concentration if 100 mL of water is added to 25.0 mL of 6.0 M NaCl?

Which procedure will produce 250 mL of a solution that is 4% by volume alcohol in water?

The number of components in a solution is ________.

All of the following statements describing solutions are true except

A supersaturated solution

How many grams of FeSO4 are present in a 20.0 mL sample of a 0.500 M solution?

What is the % (w/v)concentration of a solution containing 8.0 grams of alcohol in 50.0 mL of solution?

Adding solute to a solution increases each of the following except

Considering 0.10 M solutions of each substance,which contains the smallest concentration of ions?

Which of the following should be immiscible with carbon tetrachloride,CCl4?

How many g of Fe(NO3)3 are present in a 20.0 mL sample of a 0.500 M solution?

Considering 1.0 M solutions of each substance,which contains the largest concentration of ions?

How many grams of CaCl2 are needed to prepare 125 mL of a 1.50 M solution?

Which statement about solubility is not true?

What is the molarity of a solution prepared by dissolving 48.0 g of NaOH in enough water to make 1.50 L of solution?

The exothermic step in the dissolution of NaCl in water is

Which solution will have the highest boiling point?

How many g of CaCl2 are needed to prepare 500.mL of a 0.375 M solution?

A 20.0 mL sample of CuSO4 was evaporated to dryness,leaving 0.967 g of residue.What was the molarity of the original solution?

Matter and Measurements

Atoms and the Periodic Table

Ionic Compounds

Molecular Compounds

Classification and Balancing of Chemical Reactions

Chemical Reactions: Mole and Mass Relationships

Chemical Reactions: Energy, rates, and Equilibrium

Gases, liquids, and Solids

Acids and Bases

Nuclear Chemistry

Introduction to Organic Chemistry: Alkanes

Alkenes, alkynes, and Aromatic Compounds

Some Compounds With Oxygen, sulfur, or a Halogen

Amines

Aldehydes and Ketones

Carboxylic Acids and Their Derivatives

Amino Acids and Proteins

Enzymes and Vitamins

The Generation of Biochemical Energy

Carbohydrates

Carbohydrate Metabolism

Lipids

Lipid Metabolism

Nucleic Acids and Protein Synthesis

Genomics

Protein and Amino Acid Metabolism

Chemical Messengers: Hormones, neurotransmitters, and Drugs

Body Fluids

Filters

How many grams of FeSO₄ are present in a 20.0 mL sample of a 0.500 M solution?

Which of the following should be immiscible with carbon tetrachloride,CCl₄?

How many g of Fe(NO₃)₃ are present in a 20.0 mL sample of a 0.500 M solution?

How many grams of CaCl₂ are needed to prepare 125 mL of a 1.50 M solution?

How many g of CaCl₂ are needed to prepare 500.mL of a 0.375 M solution?

A 20.0 mL sample of CuSO₄ was evaporated to dryness,leaving 0.967 g of residue.What was the molarity of the original solution?