Question 1

Suppression of the solubility of one ion by the addition of the counter ion in its insoluble salt is known as the

Accepted Answer

A) ionic suppression effect. 
B) counter-ion effect. 
C) common-ion effect. 
D) excession effect. 
E) supersaturation effect. 
A) ionic suppression effect. 
B) counter-ion effect. 
C) common-ion effect. 
D) excession effect. 
E) supersaturation effect.

Question 2

What is the equilibrium concentration of ZN2+(aq) in a solution that is initially 0.0100 M solution in Zn(NO3)2 at a pH of 13.00? 
Zn2+(aq) + 4 OH - (aq) fi Zn(OH)42  - (aq) Kf=

Accepted Answer

A) 3.1 * 10-13 M 
B) 2.5 * 10-14 M 
C) 4.4 * 10-17 M 
D) 6.1* 10-10 M 
E) 5.0 * 105 M 
A) 3.1 * 10-13 M 
B) 2.5 * 10-14 M 
C) 4.4 * 10-17 M 
D) 6.1* 10-10 M 
E) 5.0 * 105 M

Question 3

Which of the statements below regarding hydrated metal ions is FALSE?

Accepted Answer

A) An aqueous metal ion can attract the electrons in the O-H bonds of the water molecules in its inner coordination sphere. 
B) Aqueous metal ions catalyze the autoionization of water, causing the solution to become more acidic. 
C) In solutions that are slightly acidic to slightly basic, most aqueous transition metal ions exist as complexes in which at least one ligand is OH-. 
D) Acid strength typically increases as the charge on the aqueous metal ion increases. 
E) Acid strength typically increases as the size of the aqueous metal ion decreases. 
A) An aqueous metal ion can attract the electrons in the O-H bonds of the water molecules in its inner coordination sphere. 
B) Aqueous metal ions catalyze the autoionization of water, causing the solution to become more acidic. 
C) In solutions that are slightly acidic to slightly basic, most aqueous transition metal ions exist as complexes in which at least one ligand is OH-. 
D) Acid strength typically increases as the charge on the aqueous metal ion increases. 
E) Acid strength typically increases as the size of the aqueous metal ion decreases.

Question 4

What reaction occurs as sodium hydroxide is added to a solution containing equal concentrations of acetic acid and sodium acetate?

Accepted Answer

A) CH3 COOH(aq) + OH-aq) $\rightarrow$ CH3 COO-(aq) + H2 O(l) 
B) CH3 COO-(aq) +H2 Ol) $\rightarrow$CH3 COOH(aq) + OH-(aq) 
C) CH3COO-(aq) + Na+(aq)$\rightarrow$NaCH3COO(aq) 
D) 2 CH3 COO-(aq) + 2 OH-(aq) $\rightarrow$2 CH3 COOH(aq) + O2 (g) 
E) CH3 COOH(aq) + Na+(aq) $\rightarrow$ NaCH3 COO(aq) + H+(aq) 
A) CH3 COOH(aq) + OH-aq) $\rightarrow$ CH3 COO-(aq) + H2 O(l) 
B) CH3 COO-(aq) +H2 Ol) $\rightarrow$CH3 COOH(aq) + OH-(aq) 
C) CH3COO-(aq) + Na+(aq)$\rightarrow$NaCH3COO(aq) 
D) 2 CH3 COO-(aq) + 2 OH-(aq) $\rightarrow$2 CH3 COOH(aq) + O2 (g) 
E) CH3 COOH(aq) + Na+(aq) $\rightarrow$ NaCH3 COO(aq) + H+(aq)

Question 5

A solution containing roughly equal concentrations of _______ is NOT a buffer solution.

Accepted Answer

A) fluoride ion and hydrofluoric acid 
B) bromide ion and hydrobromic acid 
C) phosphate ion and hydrogen phosphate ion 
D) carbonate ion and hydrogen carbonate ion 
E) phosphoric acid and dihydrogen phosphate ion 
A) fluoride ion and hydrofluoric acid 
B) bromide ion and hydrobromic acid 
C) phosphate ion and hydrogen phosphate ion 
D) carbonate ion and hydrogen carbonate ion 
E) phosphoric acid and dihydrogen phosphate ion

Question 6

The following titration curve is most likely to be associated with

Accepted Answer

A) the titration of a strong acid with a strong base titrant. 
B) the titration of a weak acid with a strong base titrant. 
C) the titration of a strong base with a strong acid titrant. 
D) the titration of a weak base with a strong acid titrant. 
A) the titration of a strong acid with a strong base titrant. 
B) the titration of a weak acid with a strong base titrant. 
C) the titration of a strong base with a strong acid titrant. 
D) the titration of a weak base with a strong acid titrant.

Question 7

Which solution below would make the best buffer? (Ac = acetate)

Accepted Answer

A) hydrochloric acid and sodium chloride, HCl and NaCl 
B) acetic acid and ammonia, HAc and NH3 
C) acetic acid and ammonium chloride, HAc and NH4Cl 
D) sodium acetate and ammonium chloride, NaAc and NH4Cl 
E) ammonia and ammonium chloride, NH3 and NH4Cl 
A) hydrochloric acid and sodium chloride, HCl and NaCl 
B) acetic acid and ammonia, HAc and NH3 
C) acetic acid and ammonium chloride, HAc and NH4Cl 
D) sodium acetate and ammonium chloride, NaAc and NH4Cl 
E) ammonia and ammonium chloride, NH3 and NH4Cl

Question 8

A ligand is any _______ forming a coordinate bond to a metal cation.

Accepted Answer

A) Lewis acid 
B) ion 
C) Lewis base 
D) organic compound 
E) species 
A) Lewis acid 
B) ion 
C) Lewis base 
D) organic compound 
E) species

Question 9

Which statement below regarding complex ions and coordination compounds is FALSE?

Accepted Answer

A) Ligands function as electron pair donors. 
B) A metal cation acts as a Lewis acid in a complex ion. 
C) Ligands occupy the inner coordination sphere of the cation. 
D) The information constant Kf for complex ions are generally much greater than 1. 
E) Counter ions form coordinate covalent bonds with the ligands in a complex. 
A) Ligands function as electron pair donors. 
B) A metal cation acts as a Lewis acid in a complex ion. 
C) Ligands occupy the inner coordination sphere of the cation. 
D) The information constant Kf for complex ions are generally much greater than 1. 
E) Counter ions form coordinate covalent bonds with the ligands in a complex.

Question 10

When an acetic acid solution is titrated with sodium hydroxide, the slope of the titration curve (pH vs.volume of NaOH added) increases when sodium hydroxide is first added.This change shows that

Accepted Answer

A) nothing is happening during this part of the titration. 
B) the reaction is very slow during this part of the titration. 
C) a more concentrated solution of NaOH needs to be present to initiate the reaction. 
D) acetic acid is being converted to sodium acetate. 
E) the pH is not affected until all the acetic acid is consumed. 
A) nothing is happening during this part of the titration. 
B) the reaction is very slow during this part of the titration. 
C) a more concentrated solution of NaOH needs to be present to initiate the reaction. 
D) acetic acid is being converted to sodium acetate. 
E) the pH is not affected until all the acetic acid is consumed.

Question 11

A buffer solution is made such that the initial concentrations of lactic acid (HC3H5O3 ) and the lactate ion (C3H5O3-) are 0.600 M and 0.620 M, respectively.What is the resulting pH if 100.0 mL of 0.100 M potassium hydroxide is added to 0.500 L of the buffer solution? (The Ka of HC3H5O3 is 1.4 * 10-4.)

Accepted Answer

A) 3.81 
B) 3.90 
C) 2.75 
D) 4.96 
E) 3.85 
A) 3.81 
B) 3.90 
C) 2.75 
D) 4.96 
E) 3.85

Question 12

The solubility product for PbCl2 is written as _______, where s is the molar solubility.

Accepted Answer

A) Ksp = s2 
B) Ksp = 2s2 
C) Ksp= S3 
D) Ksp = 2S3 
E) Ksp = 4S3 
A) Ksp = s2 
B) Ksp = 2s2 
C) Ksp= S3 
D) Ksp = 2S3 
E) Ksp = 4S3

Question 13

What is the pH of a solution in which [A-] = 2[HA] and the pKa of HA is 4.5?

Accepted Answer

A) 2.5 
B) 4.2 
C) 4.5 
D) 4.8 
E) 6.5 
A) 2.5 
B) 4.2 
C) 4.5 
D) 4.8 
E) 6.5

Question 14

Write the equation for the Lewis acid-base equilibrium that exists in aqueous HF.Identify the Lewis acid and the Lewis base.

Accepted Answer

@#LAT-DLM&
The acid

Question 15

What is true about the pKa of the most suitable acid-base indicator for a titration of hydrochloric acid with NaOH?

Accepted Answer

A) pKa of the indicator =pKa of the acid 
B) pKa of the indicator = pKb of the base 
C) pK a of the indicator =the concentration of the acid 
D) pK a of the indicator = the concentration of the base 
E) pK a of the indicator =7.0 
A) pKa of the indicator =pKa of the acid 
B) pKa of the indicator = pKb of the base 
C) pK a of the indicator =the concentration of the acid 
D) pK a of the indicator = the concentration of the base 
E) pK a of the indicator =7.0

Question 16

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pKa of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

Accepted Answer

A) 4.12 
B) 9.88 
C) 6.01 
D) 7.99 
E) Insufficient information is provided to determine the pH. 
A) 4.12 
B) 9.88 
C) 6.01 
D) 7.99 
E) Insufficient information is provided to determine the pH.

Question 17

A 0.500 g sample of an unknown substance was titrated with a 0.1 M HCl solution.Another 0.500 g sample of it was titrated with a 0.1 M NaOH solution.The resulting titration curves are illustrated here.Given the following possibilities, what is the sample?

Accepted Answer

A) Na2CO3 
B) NaHCO3 
C) H2CO3 
D) CO2 
E) There is no way to tell. 
A) Na2CO3 
B) NaHCO3 
C) H2CO3 
D) CO2 
E) There is no way to tell.

Question 18

What is indicated by the shape of the titration curve?

Accepted Answer

A) A diprotic acid was titrated with a strong base. 
B) A triprotic acid was titrated with a strong base. 
C) A dibasic base was titrated with a strong acid. 
D) A tribasic base was titrated with a strong acid. 
E) A strong acid was titrated with a strong base. 
A) A diprotic acid was titrated with a strong base. 
B) A triprotic acid was titrated with a strong base. 
C) A dibasic base was titrated with a strong acid. 
D) A tribasic base was titrated with a strong acid. 
E) A strong acid was titrated with a strong base.

Question 19

Write the equation for the Lewis acid-base reaction of BCl3 and NH3.Identify the Lewis acid and the Lewis base.

Accepted Answer

NH₃ (g) + BCl₃

Question 20

Which combination of solutions is the best choice for making a buffer solution?

Accepted Answer

A) equal volumes of 1 M ammonia (NH3) and 0.001 M ammonium chloride (NH4Cl) 
B) equal volumes of 0.5 M hydrochloric acid (HCl) and 0.5 M sodium hydroxide (NaOH) 
C) equal volumes of 0.5 M hydrochloric acid (HCl) and 0.5 M sodium chloride (NaCl) 
D) equal volumes of 2 M ammonia (NH3) and 1 M hydrochloric acid (HCl) 
E) equal volumes of 2 M ammonium chloride (NH4Cl) and 1 M hydrochloric acid (HCl) 
A) equal volumes of 1 M ammonia (NH3) and 0.001 M ammonium chloride (NH4Cl) 
B) equal volumes of 0.5 M hydrochloric acid (HCl) and 0.5 M sodium hydroxide (NaOH) 
C) equal volumes of 0.5 M hydrochloric acid (HCl) and 0.5 M sodium chloride (NaCl) 
D) equal volumes of 2 M ammonia (NH3) and 1 M hydrochloric acid (HCl) 
E) equal volumes of 2 M ammonium chloride (NH4Cl) and 1 M hydrochloric acid (HCl)

Exam 16: Additional Aqueous Equilibria Chemistry and the Oceans

Suppression of the solubility of one ion by the addition of the counter ion in its insoluble salt is known as the

What is the equilibrium concentration of ZN2+(aq) in a solution that is initially 0.0100 M solution in Zn(NO3)2 at a pH of 13.00? Zn2+(aq) + 4 OH - (aq) fi Zn(OH)42 - (aq) Kf=

Which of the statements below regarding hydrated metal ions is FALSE?

What reaction occurs as sodium hydroxide is added to a solution containing equal concentrations of acetic acid and sodium acetate?

A solution containing roughly equal concentrations of _______ is NOT a buffer solution.

The following titration curve is most likely to be associated with

Which solution below would make the best buffer? (Ac = acetate)

A ligand is any _______ forming a coordinate bond to a metal cation.

Which statement below regarding complex ions and coordination compounds is FALSE?

When an acetic acid solution is titrated with sodium hydroxide, the slope of the titration curve (pH vs.volume of NaOH added) increases when sodium hydroxide is first added.This change shows that

The solubility product for PbCl2 is written as _______, where s is the molar solubility.

What is the pH of a solution in which [A-] = 2[HA] and the pKa of HA is 4.5?

Write the equation for the Lewis acid-base equilibrium that exists in aqueous HF.Identify the Lewis acid and the Lewis base.

What is true about the pKa of the most suitable acid-base indicator for a titration of hydrochloric acid with NaOH?

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pKa of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

A 0.500 g sample of an unknown substance was titrated with a 0.1 M HCl solution.Another 0.500 g sample of it was titrated with a 0.1 M NaOH solution.The resulting titration curves are illustrated here.Given the following possibilities, what is the sample?

What is indicated by the shape of the titration curve?

Write the equation for the Lewis acid-base reaction of BCl3 and NH3.Identify the Lewis acid and the Lewis base.

Which combination of solutions is the best choice for making a buffer solution?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

What is the equilibrium concentration of ZN^₂+(aq) in a solution that is initially 0.0100 M solution in Zn(NO₃)₂ at a pH of 13.00? Zn²⁺(aq) + 4 OH ^- (aq) fi Zn(OH)₄² ^- (aq) K_f=

The solubility product for PbCl₂ is written as _______, where s is the molar solubility.

What is the pH of a solution in which [A^-] = 2[HA] and the pK_a of HA is 4.5?

What is true about the pK_a of the most suitable acid-base indicator for a titration of hydrochloric acid with NaOH?

Glycolic acid, which is a monoprotic acid and a constituent in sugarcane, has a pK_a of 3.9.A 25.0 mL solution of glycolic acid is titrated to the equivalence point with 35.8 mL of 0.020 M sodium hydroxide solution.What is the pH of the resulting solution at the equivalence point?

Write the equation for the Lewis acid-base reaction of BCl₃ and NH₃.Identify the Lewis acid and the Lewis base.