Question 1

The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.

Accepted Answer

A) 0.193 M 
B) 0.386 M 
C) 0.0965 M 
D) 0.579 M 
E) 0.0643 M 
A) 0.193 M 
B) 0.386 M 
C) 0.0965 M 
D) 0.579 M 
E) 0.0643 M

Question 2

HNO2 is a strong acid.

Accepted Answer

A) True 
 B)False

Question 3

How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?

Accepted Answer

A) 0.436 
B) 0.871 
C) 1.31 
D) 3.70 
E) 11.1 
A) 0.436 
B) 0.871 
C) 1.31 
D) 3.70 
E) 11.1

Question 4

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

Accepted Answer

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. 
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.

Question 5

Of the metals below, only ________ will not dissolve in an aqueous solution containing nickel ions. aluminum
Chromium
Barium
Tin
Potassium

Accepted Answer

A) aluminum 
B) chromium 
C) barium 
D) tin 
E) potassium 
A) aluminum 
B) chromium 
C) barium 
D) tin 
E) potassium

Question 6

A 0.100 M solution of ________ will contain the highest concentration of potassium ions.

Accepted Answer

A) potassium phosphate 
B) potassium hydrogen carbonate 
C) potassium hypochlorite 
D) potassium iodide 
E) potassium oxide 
A) potassium phosphate 
B) potassium hydrogen carbonate 
C) potassium hypochlorite 
D) potassium iodide 
E) potassium oxide

Question 7

Which solution contains the largest number of moles of chloride ions?

Accepted Answer

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 
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

Question 8

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?

Accepted Answer

A) 11.9 
B) 0.00159 
C) 1.59 
D) 4.67 
E) 5.31 
A) 11.9 
B) 0.00159 
C) 1.59 
D) 4.67 
E) 5.31

Question 9

The concentration of chloride ions in a 0.193 M solution of potassium chloride is ________.

Accepted Answer

A) 0.0643 M 
B) 0.386 M 
C) 0.0965 M 
D) 0.579 M 
E) 0.193 M 
A) 0.0643 M 
B) 0.386 M 
C) 0.0965 M 
D) 0.579 M 
E) 0.193 M

Question 10

What is the concentration (M)of sodium ions in 4.57 L of a 2.98 M Na3PO4 solution?

Accepted Answer

Question 11

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.

Accepted Answer

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) 
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)

Question 12

The total concentration of ions in a 0.250 M solution of HCl is ________.

Accepted Answer

A) 0 
B) 0.125 M 
C) 0.250 M 
D) 0.500 M 
E) 0.750 M 
A) 0 
B) 0.125 M 
C) 0.250 M 
D) 0.500 M 
E) 0.750 M

Question 13

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?

Accepted Answer

A) NH4+ 
B) K+ 
C) Cr3+ 
D) Rb+ 
E) Na+ 
A) NH4+ 
B) K+ 
C) Cr3+ 
D) Rb+ 
E) Na+

Question 14

Lead ions can be precipitated from aqueous solutions by the addition of aqueous iodide: Pb2+ (aq) + 2I- (aq) → PbI2 (s)
Lead iodide is virtually insoluble in water so that the reaction appears to go to completion. How many milliliters of 3.550 M HI(aq)must be added to a solution containing 0.600 mol of Pb(NO3)2 (aq)to completely precipitate the lead?

Accepted Answer

A) 2.96 × 10-3 
B) 338 
C) 169 
D) 0.169 
E) 0.338 
A) 2.96 × 10-3 
B) 338 
C) 169 
D) 0.169 
E) 0.338

Question 15

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?

Accepted Answer

A) 11.9 
B) 1.11 
C) 0.00159 
D) 1.59 
E) 0.0841 
A) 11.9 
B) 1.11 
C) 0.00159 
D) 1.59 
E) 0.0841

Question 16

Ca(OH)2 is a strong base.

Accepted Answer

A) True 
 B)False

Question 17

Of the following elements, ________ is the most easily oxidized. oxygen
Fluorine
Nitrogen
Aluminum
Gold

Accepted Answer

A) oxygen 
B) fluorine 
C) nitrogen 
D) aluminum 
E) gold 
A) oxygen 
B) fluorine 
C) nitrogen 
D) aluminum 
E) gold

Question 18

Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH?

Accepted Answer

A) 20.0 mL of 0.200 M solution of NaOH 
B) 25.0 mL of 0.175 M solution of NaOH 
C) 30.0 mL of 0.145 M solution of NaOH 
D) 50.0 mL of 0.125 M solution of NaOH 
E) 100.0 mL of 0.0500 M solution of NaOH 
A) 20.0 mL of 0.200 M solution of NaOH 
B) 25.0 mL of 0.175 M solution of NaOH 
C) 30.0 mL of 0.145 M solution of NaOH 
D) 50.0 mL of 0.125 M solution of NaOH 
E) 100.0 mL of 0.0500 M solution of NaOH

Question 19

A 11.5 mL aliquot of 0.162 M H3PO4 (aq)is to be titrated with 0.229 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

Accepted Answer

A) 24.4 
B) 1.28 
C) 8.14 
D) 2.71 
E) 103 
A) 24.4 
B) 1.28 
C) 8.14 
D) 2.71 
E) 103

Question 20

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?

Accepted Answer

A) 4.59 
B) 2.30 
C) 25.7 
D) 0.130 
E) 25,700 
A) 4.59 
B) 2.30 
C) 25.7 
D) 0.130 
E) 25,700

Exam 4: Aqueous Reactions and Solution Stoichiometry

The concentration of iodide ions in a 0.193 M solution of barium iodide is ________.

HNO2 is a strong acid.

How many moles of Na+ are present in 343 mL of a 1.27 M solution of Na2SO4?

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

Of the metals below, only ________ will not dissolve in an aqueous solution containing nickel ions. aluminum Chromium Barium Tin Potassium

A 0.100 M solution of ________ will contain the highest concentration of potassium ions.

Which solution contains the largest number of moles of chloride ions?

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?

The concentration of chloride ions in a 0.193 M solution of potassium chloride is ________.

What is the concentration (M)of sodium ions in 4.57 L of a 2.98 M Na3PO4 solution?

The balanced reaction between aqueous nitric acid and aqueous strontium hydroxide is ________.

The total concentration of ions in a 0.250 M solution of HCl is ________.

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?

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?

Ca(OH)2 is a strong base.

Of the following elements, ________ is the most easily oxidized. oxygen Fluorine Nitrogen Aluminum Gold

Which solution has the same number of moles of NaOH as 50.0 mL of 0.100 M solution of NaOH?

A 11.5 mL aliquot of 0.162 M H3PO4 (aq)is to be titrated with 0.229 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

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?

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

HNO₂ is a strong acid.

How many moles of Na⁺ are present in 343 mL of a 1.27 M solution of Na₂SO₄?

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?

What is the concentration (M)of sodium ions in 4.57 L of a 2.98 M Na₃PO₄ solution?

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?

Ca(OH)₂ is a strong base.

A 11.5 mL aliquot of 0.162 M H₃PO₄ (aq)is to be titrated with 0.229 M NaOH (aq). What volume (mL)of base will it take to reach the equivalence point?

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?