Question 1

A weak electrolyte exists predominantly as ________ in solution.

Accepted Answer

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

Question 2

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

Accepted Answer

A) 48.89 
B) 97.78 
C) 28.59 
D) 1.086 
E) 22.83 
A) 48.89 
B) 97.78 
C) 28.59 
D) 1.086 
E) 22.83

Question 3

The solvent in an aqueous solution is ________.

Accepted Answer

The answer of The solvent in an aqueous solution is...

Question 4

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

Accepted Answer

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) 
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 5

How many moles of Co2+ are present in 0.300 L of a 0.500 M solution of CoI2?

Accepted Answer

Question 6

Which one of the following compounds is insoluble in water?

Accepted Answer

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

Question 7

Sodium does not occur in nature as Na (s)because ________.

Accepted Answer

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+ 
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 8

The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are ________.

Accepted Answer

A) OH-, F-, and Ba2+ 
B) F- and Ba2+ 
C) OH- and F- 
D) Ba2+ only 
E) H+, OH-, F-, and Ba2+ 
A) OH-, F-, and Ba2+ 
B) F- and Ba2+ 
C) OH- and F- 
D) Ba2+ only 
E) H+, OH-, F-, and Ba2+

Question 9

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

Accepted Answer

A) Phosphate 
B) Sulfate 
C) Sulfide 
D) Iodide 
E) Potassium will form soluble salts with all choices. 
A) Phosphate 
B) Sulfate 
C) Sulfide 
D) Iodide 
E) Potassium will form soluble salts with all choices.

Question 10

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?

Accepted Answer

A) 18 
B) 0.16 
C) 0.45 
D) 27 
E) 2.7 × 10-2 
A) 18 
B) 0.16 
C) 0.45 
D) 27 
E) 2.7 × 10-2

Question 11

The compound HClO4 is a weak acid.

Accepted Answer

A) True 
 B)False

Question 12

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.

Accepted Answer

A) 0.175 
B) 4.37 
C) 0.525 
D) 0.350 
E) 0.874 
A) 0.175 
B) 4.37 
C) 0.525 
D) 0.350 
E) 0.874

Question 13

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

Accepted Answer

A) H2 
B) H2O 
C) CO2 
D) NaOH 
E) O2 
A) H2 
B) H2O 
C) CO2 
D) NaOH 
E) O2

Question 14

What is the formula for phosphoric acid?

Accepted Answer

A) H3PO4 
B) H2PO4 
C) H4PO4 
D) H3PO3 
E) none of the above 
A) H3PO4 
B) H2PO4 
C) H4PO4 
D) H3PO3 
E) none of the above

Question 15

How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?

Accepted Answer

Question 16

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

Accepted Answer

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

Question 17

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?

Accepted Answer

A) 0.561 
B) 80.8 
C) 0.280 
D) 0.140 
E) 3.21 
A) 0.561 
B) 80.8 
C) 0.280 
D) 0.140 
E) 3.21

Question 18

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

Accepted Answer

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

Question 19

With which ion will the mercury ion form an insoluble salt?

Accepted Answer

A) phosphate 
B) nitrate 
C) sulfate 
D) chloride 
E) acetate 
A) phosphate 
B) nitrate 
C) sulfate 
D) chloride 
E) acetate

Question 20

The molarity (M)of an aqueous solution containing 22.5 g of sucrose (C12H22O11)in 35.5 mL of solution is ________.

Accepted Answer

A) 0.0657 
B) 1.85 ×   
C) 1.85 
D) 3.52 
E) 0.104 
A) 0.0657 
B) 1.85 ×   
C) 1.85 
D) 3.52 
E) 0.104

Exam 4: Aqueous Reactions and Solution Stoichiometry

A weak electrolyte exists predominantly as ________ in solution.

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H2C2O4)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

The solvent in an aqueous solution is ________.

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

How many moles of Co2+ are present in 0.300 L of a 0.500 M solution of CoI2?

Which one of the following compounds is insoluble in water?

Sodium does not occur in nature as Na (s)because ________.

The spectator ions in the reaction between aqueous hydrofluoric acid and aqueous barium hydroxide are ________.

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

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?

The compound HClO4 is a weak acid.

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.

Which one of the following substances is produced during the reaction of an acid with a metal hydroxide?

What is the formula for phosphoric acid?

How many moles of BaCl2 are formed in the neutralization of 393 mL of 0.171 M Ba(OH)2 with aqueous HCl?

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

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?

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

With which ion will the mercury ion form an insoluble salt?

The molarity (M)of an aqueous solution containing 22.5 g of sucrose (C12H22O11)in 35.5 mL of solution is ________.

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

The Chemistry of Life: Organic and Biological Chemistry

Filters

Oxalic acid is a diprotic acid. Calculate the percent of oxalic acid (H₂C₂O₄)in a solid given that a 0.7984-g sample of that solid required 37.98 mL of 0.2283 M NaOH for neutralization.

How many moles of Co²⁺ are present in 0.300 L of a 0.500 M solution of CoI₂?

The compound HClO₄ is a weak acid.

How many moles of BaCl₂ are formed in the neutralization of 393 mL of 0.171 M Ba(OH)₂ with aqueous HCl?

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?

The molarity (M)of an aqueous solution containing 22.5 g of sucrose (C₁₂H₂₂O₁₁)in 35.5 mL of solution is ________.