Question 1

How many grams of H3PO4 are in 145 mL of a 3.50 M solution of H3PO4?

Accepted Answer

A) 0.508 
B) 49.7 
C) 20.0 
D) 4.90 
E) 612 
A) 0.508 
B) 49.7 
C) 20.0 
D) 4.90 
E) 612

Question 2

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

Accepted Answer

A) 1.85 
B) 2.12 
C) 0.197 
D) 3.52 
E) 11.8 
A) 1.85 
B) 2.12 
C) 0.197 
D) 3.52 
E) 11.8

Question 3

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?

Accepted Answer

A) 0.105 
B) 6.11 
C) 3.21 
D) 6.11 × 103 
E) 12.2 
A) 0.105 
B) 6.11 
C) 3.21 
D) 6.11 × 103 
E) 12.2

Question 4

How many grams of H3PO4 are in 415 mL of a 4.00 M solution of H3PO4?

Accepted Answer

Question 5

Which of the following are weak acids?

Accepted Answer

A) HF, HBr 
B) HI, HNO3, HBr 
C) HI, HF 
D) HF 
E) none of the above 
A) HF, HBr 
B) HI, HNO3, HBr 
C) HI, HF 
D) HF 
E) none of the above

Question 6

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium ion and ________ M sulfate ion.

Accepted Answer

A) 2.104, 1.052 
B) 2.104, 2.104 
C) 2.104, 4.208 
D) 1.052, 1.052 
E) 4.208, 2.104 
A) 2.104, 1.052 
B) 2.104, 2.104 
C) 2.104, 4.208 
D) 1.052, 1.052 
E) 4.208, 2.104

Question 7

Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)reaction?

Accepted Answer

A) calcium nitrate 
B) sodium bromide 
C) lead nitrate 
D) barium nitrate 
E) sodium chloride 
A) calcium nitrate 
B) sodium bromide 
C) lead nitrate 
D) barium nitrate 
E) sodium chloride

Question 8

How many grams of NaOH (MW = 40.0)are there in 500.0 mL of a 0.250 M NaOH solution?

Accepted Answer

A) 0.00219 
B) 114 
C) 14.0 
D) 5.00 
E) 0.125 
A) 0.00219 
B) 114 
C) 14.0 
D) 5.00 
E) 0.125

Question 9

Ammonia is a strong base.

Accepted Answer

A) True 
 B)False

Question 10

When aqueous solutions of Pb(NO3)2 and NaCl are mixed, PbCl2 precipitates. The balanced net ionic equation is ________.

Accepted Answer

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) 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)

Question 11

Based on the activity series, which one of the reactions below will occur?

Accepted Answer

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) 
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 12

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

Accepted Answer

A) 2H+ (aq) + 2OH- (aq) → 2H2O (l) 
B) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq) 
C) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) 
D) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 
E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq) 
A) 2H+ (aq) + 2OH- (aq) → 2H2O (l) 
B) 2H+ (aq) + 2KOH (aq) → 2H2O (l) + 2K+ (aq) 
C) H2SO4 (aq) + 2OH- (aq) → 2H2O (l) + SO42- (aq) 
D) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (s) 
E) H2SO4 (aq) + 2KOH (aq) → 2H2O (l) + K2SO4 (aq)

Question 13

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?

Accepted Answer

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 0.600 mol of Ca2+. 
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 0.600 mol of Ca2+.

Question 14

How many grams of CH3OH must be added to water to prepare 175 mL of a solution that is 1.0 M CH3OH?

Accepted Answer

Question 15

In which species does nitrogen have the highest oxidation number?

Accepted Answer

A) NaNO3 
B) HNO2 
C) NO2- 
D) NH3 
E) N2 
A) NaNO3 
B) HNO2 
C) NO2- 
D) NH3 
E) N2

Question 16

A 24.5 mL aliquot of 0.0938 M H2SO4 (aq)is to be titrated with 0.0295 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

Accepted Answer

A) 156 
B) 0.136 
C) 77.9 
D) 39.0 
E) 4430 
A) 156 
B) 0.136 
C) 77.9 
D) 39.0 
E) 4430

Question 17

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 ________.

Accepted Answer

A) 0.0102 
B) 0.00508 
C) 0.0204 
D) 0.102 
E) 0.227 
A) 0.0102 
B) 0.00508 
C) 0.0204 
D) 0.102 
E) 0.227

Question 18

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?

Accepted Answer

A) 99.9 
B) 3600 
C) 287 
D) 0.104 
E) 0.0100 
A) 99.9 
B) 3600 
C) 287 
D) 0.104 
E) 0.0100

Question 19

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

Accepted Answer

A) 0.436 
B) 1.31 
C) 0.145 
D) 3.70 
E) 11.1 
A) 0.436 
B) 1.31 
C) 0.145 
D) 3.70 
E) 11.1

Question 20

How many milliliters of 0.188 M HClO4 solution are needed to neutralize 50.00 mL of 0.0832 M NaOH?

Accepted Answer

A) 0.782 
B) 8.85 × 10-3 
C) 113 
D) 0.0452 
E) 22.1 
A) 0.782 
B) 8.85 × 10-3 
C) 113 
D) 0.0452 
E) 22.1

Exam 4: Aqueous Reactions and Solution Stoichiometry

How many grams of H3PO4 are in 145 mL of a 3.50 M solution of H3PO4?

The molarity of an aqueous solution containing 75.3 g of glucose (C6H12O6)in 35.5 mL of solution is ________.

How many grams of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?

How many grams of H3PO4 are in 415 mL of a 4.00 M solution of H3PO4?

Which of the following are weak acids?

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is ________ M sodium ion and ________ M sulfate ion.

Aqueous potassium chloride will react with which one of the following in an exchange (metathesis)reaction?

How many grams of NaOH (MW = 40.0)are there in 500.0 mL of a 0.250 M NaOH solution?

Ammonia is a strong base.

When aqueous solutions of Pb(NO3)2 and NaCl are mixed, PbCl2 precipitates. The balanced net ionic equation is ________.

Based on the activity series, which one of the reactions below will occur?

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

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca3(PO4)2?

How many grams of CH3OH must be added to water to prepare 175 mL of a solution that is 1.0 M CH3OH?

In which species does nitrogen have the highest oxidation number?

A 24.5 mL aliquot of 0.0938 M H2SO4 (aq)is to be titrated with 0.0295 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

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 ________.

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?

How many moles of K+ are present in 343 mL of a 1.27 M solution of K3PO4?

How many milliliters of 0.188 M HClO4 solution are needed to neutralize 50.00 mL of 0.0832 M NaOH?

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

How many grams of H₃PO₄ are in 145 mL of a 3.50 M solution of H₃PO₄?

The molarity of an aqueous solution containing 75.3 g of glucose (C₆H₁₂O₆)in 35.5 mL of solution is ________.

How many grams of H₃PO₄ are in 415 mL of a 4.00 M solution of H₃PO₄?

The concentration of species in 500 mL of a 2.104 M solution of sodium sulfate is M sodium ion and M sulfate ion.

When aqueous solutions of Pb(NO₃)₂ and NaCl are mixed, PbCl₂ precipitates. The balanced net ionic equation is ________.

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

Which one of the following is not true concerning 2.00 L of 0.100 M solution of Ca₃(PO₄)₂?

How many grams of CH₃OH must be added to water to prepare 175 mL of a solution that is 1.0 M CH₃OH?

A 24.5 mL aliquot of 0.0938 M H₂SO₄ (aq)is to be titrated with 0.0295 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

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 ________.

How many moles of K⁺ are present in 343 mL of a 1.27 M solution of K₃PO₄?

How many milliliters of 0.188 M HClO₄ solution are needed to neutralize 50.00 mL of 0.0832 M NaOH?