Question 1

The bonds between the zinc ion and the nitrogen atoms in the complex Zn(NH3)42F1F1F1S1F1F1F10 are best described as ________

Accepted Answer

A) ionic. 
B) covalent. 
C) coordinate covalent. 
D) polar covalent. 
E) d-electron bonds. 
A) ionic. 
B) covalent. 
C) coordinate covalent. 
D) polar covalent. 
E) d-electron bonds.

Question 2

To simulate the pH of blood, which is 7.4, an undergraduate researcher in a biology lab produced a buffer solution by dissolving sodium dihydrogen phosphate (Ka F1F1F1S1F1F1F10 6.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108) and disodium hydrogen phosphate (Ka F1F1F1S1F1F1F10 3.6 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F1013) together in an aqueous solution. What mole ratio of Na2HPO4/NaH2PO4 did she need to use?

Accepted Answer

Question 3

Given the following titration curves, provide a potential reaction that describes each titration.
a)   
b)

Accepted Answer

a) @#IMG-DLM& (weak base-stron

Question 4

Describe the similarities and differences between a covalent bond and a coordinate covalent bond.

Accepted Answer

For both types of bonds, a pair of elect

Question 5

The pKa of a weak acid was determined to be 3.39 by measuring the pH of a solution containing the weak acid at 0.20 M and its conjugate base. The measured pH was 3.27. What was the concentration of the conjugate base?

Accepted Answer

A) 0.26 M 
B) 0.15 M 
C) 0.20 M 
D) 0.050 M 
E) 0.35 M 
A) 0.26 M 
B) 0.15 M 
C) 0.20 M 
D) 0.050 M 
E) 0.35 M

Question 6

Explain how a buffer solution manages to stabilize the pH against the addition of acid, base, or additional solvent (dilution).

Accepted Answer

A buffer consists of a weak acid and its

Question 7

Glycolic acid, which is a monoprotic acid and a constituent in sugar cane, 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

Question 8

Phenylephrine (PE, see the structure below) is a nasal decongestant and is the active ingredient in Sudafed, which contains phenylephrine hydrochloride (PEHCl). This conjugate acid of phenylephrine (PEHF1F1F1S1F1F1F10) has a pKa F1F1F1S1F1F1F10 5.5. At a physiological pH of 7.4, what is the ratio of concentrations, [PE]/[PEHF1F1F1S1F1F1F10]?

Accepted Answer

A) 6.7 
B) 0.01 
C) 0.14 
D) 79 
E) 21 
A) 6.7 
B) 0.01 
C) 0.14 
D) 79 
E) 21

Question 9

A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium hydroxide (Ka of hydrofluoric acid F1F1F1S1F1F1F10 7.20 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104). What is the final pH of this solution?

Accepted Answer

A) 3.33 
B) 3.56 
C) 4.57 
D) 10.44 
E) 11.27 
A) 3.33 
B) 3.56 
C) 4.57 
D) 10.44 
E) 11.27

Question 10

Which of the following species is a Lewis acid?

Accepted Answer

A) Cl2 
B) NH3 
C) FF1F1F1S1F1F1F10 
D) P(CH3)3 
E) Al3F1F1F1S1F1F1F10 
A) Cl2 
B) NH3 
C) FF1F1F1S1F1F1F10 
D) P(CH3)3 
E) Al3F1F1F1S1F1F1F10

Question 11

What is the molar concentration of AgF1F1F1S1F1F1F10(aq) in a 1.00 M solution of Ag(NH3)2F1F1F1S1F1F1F10 with no excess ammonia? Given: Kf F1F1F1S1F1F1F10 1.70 F1F1F1S1F1F1F10 107 for Ag (NH3)2F1F1F1S1F1F1F10.

Accepted Answer

A) 2.45 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
B) 3.09 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
C) 2.42 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
D) 1.47 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
E) 1.70 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
A) 2.45 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
B) 3.09 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F103 M 
C) 2.42 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 M 
D) 1.47 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M 
E) 1.70 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F108 M

Question 12

Identify the Lewis base in the following reaction:

Accepted Answer

A) PH3 
B) HF1F1F1S1F1F1F10 
C) PH4F1F1F1S1F1F1F10 
D) None of these is a base. 
E) All of these are bases. 
A) PH3 
B) HF1F1F1S1F1F1F10 
C) PH4F1F1F1S1F1F1F10 
D) None of these is a base. 
E) All of these are bases.

Question 13

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (Ka of benzoic acid F1F1F1S1F1F1F10 6.46 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105). What is the final pH of this solution?

Accepted Answer

Question 14

When an acetic acid solution is titrated with sodium hydroxide, the slope of the titration curve (pH versus 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 15

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

Accepted Answer

The answer of Derive the Henderson-Hasselbalch equation from the acid...

Question 16

The solubility of PbI2 is 0.756 g per 100 mL of solution at 20F1F1F1S1F1F1F10C. Determine the value of the solubility product constant for this compound at 20F1F1F1S1F1F1F10C. Lead(II) iodide does not react with water.

Accepted Answer

A) 4.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
B) 3.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
D) 1.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
E) 4.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
A) 4.9 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
B) 3.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F104 
C) 1.8 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F105 
D) 1.2 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106 
E) 4.3 F1F1F1S1F1F1F10 10F1F1F1S1F1F1F106

Question 17

A buffer system is set up with [HA] F1F1F1S1F1F1F10 2[AF1F1F1S1F1F1F10]. If pKa F1F1F1S1F1F1F10 5.5, what is the pH of the buffer?

Accepted Answer

A) 5.2 
B) 5.8 
C) 7.5 
D) 3.5 
E) 7.0 
A) 5.2 
B) 5.8 
C) 7.5 
D) 3.5 
E) 7.0

Question 18

Aqueous solutions of many metal cations have a pH different from 7. Which one of the following statements about these cations is not correct?

Accepted Answer

A) Alkali metal cations such as NaF1F1F1S1F1F1F10 and KF1F1F1S1F1F1F10 have a negligible effect on the pH. 
B) Small and highly charged main group metals such as Al3F1F1F1S1F1F1F10 produce acidic aqueous solutions. 
C) For transition metal cations, the cation with the higher oxidation state produces more acidic solution; for example, Fe3F1F1F1S1F1F1F10(aq) is more acidic than Fe2F1F1F1S1F1F1F10(aq). 
D) A solution containing Cr2F1F1F1S1F1F1F10 is expected to be considerably more acidic than a solution of equal concentration containing Ni2F1F1F1S1F1F1F10. 
E) The Lewis acidity of a metal cation is a good measure of its ability to activate a water molecule to lose a proton and produce a hydronium ion. 
A) Alkali metal cations such as NaF1F1F1S1F1F1F10 and KF1F1F1S1F1F1F10 have a negligible effect on the pH. 
B) Small and highly charged main group metals such as Al3F1F1F1S1F1F1F10 produce acidic aqueous solutions. 
C) For transition metal cations, the cation with the higher oxidation state produces more acidic solution; for example, Fe3F1F1F1S1F1F1F10(aq) is more acidic than Fe2F1F1F1S1F1F1F10(aq). 
D) A solution containing Cr2F1F1F1S1F1F1F10 is expected to be considerably more acidic than a solution of equal concentration containing Ni2F1F1F1S1F1F1F10. 
E) The Lewis acidity of a metal cation is a good measure of its ability to activate a water molecule to lose a proton and produce a hydronium ion.

Question 19

A solution of hydrochloric acid (HCl, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the hydrochloric acid?

Accepted Answer

A) 0.07048 M 
B) 0.1410 M 
C) 0.2819 M 
D) 0.0353 M 
E) 0.0533 M 
A) 0.07048 M 
B) 0.1410 M 
C) 0.2819 M 
D) 0.0353 M 
E) 0.0533 M

Question 20

Write the reaction equation and the equilibrium constant expression that describes lead chloride (PbCl2) dissolving in water.

Accepted Answer

@#IMG-DLM& K_sp F1F1F1S1F1F1F10

The bonds between the zinc ion and the nitrogen atoms in the complex Zn(NH₃)₄²^ are best described as ________

Given the following titration curves, provide a potential reaction that describes each titration. a) b)

Describe the similarities and differences between a covalent bond and a coordinate covalent bond.

The pK_a of a weak acid was determined to be 3.39 by measuring the pH of a solution containing the weak acid at 0.20 M and its conjugate base. The measured pH was 3.27. What was the concentration of the conjugate base?

Explain how a buffer solution manages to stabilize the pH against the addition of acid, base, or additional solvent (dilution).

Glycolic acid, which is a monoprotic acid and a constituent in sugar cane, 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?

A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium hydroxide (K_a of hydrofluoric acid  7.20  10^⁴). What is the final pH of this solution?

Which of the following species is a Lewis acid?

What is the molar concentration of Ag^(aq) in a 1.00 M solution of Ag(NH₃)₂^with no excess ammonia? Given: K_f  1.70  10⁷ for Ag (NH₃)₂^.

Identify the Lewis base in the following reaction:

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (K_a of benzoic acid  6.46  10^⁵). What is the final pH of this solution?

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

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

The solubility of PbI₂ is 0.756 g per 100 mL of solution at 20C. Determine the value of the solubility product constant for this compound at 20C. Lead(II) iodide does not react with water.

A buffer system is set up with [HA]  2[A^]. If pK_a  5.5, what is the pH of the buffer?

Aqueous solutions of many metal cations have a pH different from 7. Which one of the following statements about these cations is not correct?

A solution of hydrochloric acid (HCl, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the hydrochloric acid?

Write the reaction equation and the equilibrium constant expression that describes lead chloride (PbCl₂) dissolving in water.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 16: Additional Aqueous Equilibria: Chemistry and the Oceans

The bonds between the zinc ion and the nitrogen atoms in the complex Zn(NH3)42 are best described as ________

Given the following titration curves, provide a potential reaction that describes each titration. a) b)

Describe the similarities and differences between a covalent bond and a coordinate covalent bond.

The pKa of a weak acid was determined to be 3.39 by measuring the pH of a solution containing the weak acid at 0.20 M and its conjugate base. The measured pH was 3.27. What was the concentration of the conjugate base?

Explain how a buffer solution manages to stabilize the pH against the addition of acid, base, or additional solvent (dilution).

Glycolic acid, which is a monoprotic acid and a constituent in sugar cane, 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 solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium hydroxide (Ka of hydrofluoric acid  7.20  104). What is the final pH of this solution?

Which of the following species is a Lewis acid?

What is the molar concentration of Ag(aq) in a 1.00 M solution of Ag(NH3)2 with no excess ammonia? Given: Kf  1.70  107 for Ag (NH3)2.

Identify the Lewis base in the following reaction:

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (Ka of benzoic acid  6.46  105). What is the final pH of this solution?

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

Derive the Henderson-Hasselbalch equation from the acid ionization constant expression.

The solubility of PbI2 is 0.756 g per 100 mL of solution at 20C. Determine the value of the solubility product constant for this compound at 20C. Lead(II) iodide does not react with water.

A buffer system is set up with [HA]  2[A]. If pKa  5.5, what is the pH of the buffer?

Aqueous solutions of many metal cations have a pH different from 7. Which one of the following statements about these cations is not correct?

A solution of hydrochloric acid (HCl, 25.00 mL) was titrated to completion with 34.55 mL of 0.1020 M sodium hydroxide. What was the concentration of the hydrochloric acid?

Write the reaction equation and the equilibrium constant expression that describes lead chloride (PbCl2) dissolving in water.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

A Quantum Model of Atoms: Waves and Particles

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

The bonds between the zinc ion and the nitrogen atoms in the complex Zn(NH₃)₄²^ are best described as ________

The pK_a of a weak acid was determined to be 3.39 by measuring the pH of a solution containing the weak acid at 0.20 M and its conjugate base. The measured pH was 3.27. What was the concentration of the conjugate base?

Glycolic acid, which is a monoprotic acid and a constituent in sugar cane, 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?

A solution of hydrofluoric acid (0.27 M, 10.00 mL) was titrated with 15.0 mL of 0.13 M sodium hydroxide (K_a of hydrofluoric acid  7.20  10^⁴). What is the final pH of this solution?

What is the molar concentration of Ag^(aq) in a 1.00 M solution of Ag(NH₃)₂^with no excess ammonia? Given: K_f  1.70  10⁷ for Ag (NH₃)₂^.

A solution of benzoic acid (0.21 M, 25.00 mL), a monoprotic acid, was titrated with 53.10 mL of 0.10 M sodium hydroxide (K_a of benzoic acid  6.46  10^⁵). What is the final pH of this solution?

The solubility of PbI₂ is 0.756 g per 100 mL of solution at 20C. Determine the value of the solubility product constant for this compound at 20C. Lead(II) iodide does not react with water.

A buffer system is set up with [HA]  2[A^]. If pK_a  5.5, what is the pH of the buffer?

Write the reaction equation and the equilibrium constant expression that describes lead chloride (PbCl₂) dissolving in water.