A buffer solution contains 0.150 M HCO2H and 0.225M HCO2Na and has a pH of 3.75. What is the final pH if 5.00 mL of 1.00M HCl are added to 100.0 mL of this solution?

A) 4.85 B) 5.81 C) 2.23 D) 6.46 E) 3.51 A) 4.85 B) 5.81 C) 2.23 D) 6.46 E) 3.51 E

Exam 16: Aqueous Acidbase Equilibriums

A(n) _____ takes place when atoms or groups of atoms in a molecule other than those to which H is bonded induces a change in the distribution of electrons within the molecule.

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Question 1

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Verified

inductive effect

A buffer solution contains 0.150 M HCO₂H and 0.225M HCO₂Na and has a pH of 3.75. What is the final pH if 5.00 mL of 1.00M HCl are added to 100.0 mL of this solution?

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Question 2

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The analytical concentration of an acid or a base is the final concentration.

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(True/False)

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Question 3

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False

The percent ionization in a solution of a weak acid increases as the analytical concentration decreases.

(True/False)

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Question 4

_____ are solutions that maintain a relatively constant pH when an acid or a base is added.

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Question 5

An acid-base equilibrium always favors the side with the stronger acid and base.

(True/False)

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Question 6

An acid-base reaction involves the reaction of a proton with a hydroxide ion to form _____.

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Question 7

The most important parameter for predicting the effect of a metal ion on the acidity of coordinated water molecules is the _____ of the metal ion.

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Question 8

If the pK_b of a conjugate base is equal to 10.9 at $45.0 ^ { \circ } \mathrm { C }$ , the value of its K_b is _____.

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Question 9

The pH at the midpoint of the titration of a weak acid is equal to the pK_a of the weak acid.

(True/False)

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Question 10

_____ is the only common oxoacid in which a hydrogen atom is bonded to the central atom rather than oxygen.

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Question 11

In the reaction $\mathrm { HCl } + \mathrm { H } _ { 2 } \mathrm { Of } \quad \mathrm { H } _ { 3 } \mathrm { O } ^ { + } + \mathrm { Cl } ^ { - }$ , the number of conjugate acid-base pairs is ____.

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Question 12

The amount of excess CH₃CO₂H after 6.00 mL of 0.300 M NaOH has been added to 20.0 mL of 0.100M CH₃CO₂H is _____ mmol CH₃CO₂H.

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Question 13

The $\mathrm { p } K _ { a }$ of hydrochloric acid is _____, if the $\mathrm { p } K _ { b }$ of its conjugate base is 8.56 at $25 ^ { \circ } \mathrm { C }$ .

(Multiple Choice)

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Question 14

The shape of the titration curve involving a strong acid and a strong base depends only on their identities, not their concentrations.

(True/False)

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Question 15

Which of the following acids will most likely be the strongest?

(Multiple Choice)

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Question 16

The larger the atom to which hydrogen is bonded, the stronger the bond.

(True/False)

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Question 17

If the $K _ { w }$ for water at $80 ^ { \circ } \mathrm { C }$ is $5.60 \times 10 ^ { - 11 }$ , the $\mathrm { p } K _ { w }$ for water at the same temperature is _____.

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Question 18

The pH of any neutral solution is equal to the solution's $\mathrm { p } K _ { w }$ at that temperature.

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Question 19

Electron delocalization in the conjugate base decreases acid strength.

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Question 20

Showing 1 - 20 of 97

Exam 16: Aqueous Acidbase Equilibriums

A(n) _____ takes place when atoms or groups of atoms in a molecule other than those to which H is bonded induces a change in the distribution of electrons within the molecule.

A buffer solution contains 0.150 M HCO2H and 0.225M HCO2Na and has a pH of 3.75. What is the final pH if 5.00 mL of 1.00M HCl are added to 100.0 mL of this solution?

The analytical concentration of an acid or a base is the final concentration.

The percent ionization in a solution of a weak acid increases as the analytical concentration decreases.

_____ are solutions that maintain a relatively constant pH when an acid or a base is added.

An acid-base equilibrium always favors the side with the stronger acid and base.

An acid-base reaction involves the reaction of a proton with a hydroxide ion to form _____.

The most important parameter for predicting the effect of a metal ion on the acidity of coordinated water molecules is the _____ of the metal ion.

If the pKb of a conjugate base is equal to 10.9 at 45.0∘C45.0 ^ { \circ } \mathrm { C }45.0∘C , the value of its Kb is _____.

The pH at the midpoint of the titration of a weak acid is equal to the pKa of the weak acid.

_____ is the only common oxoacid in which a hydrogen atom is bonded to the central atom rather than oxygen.

In the reaction HCl+H2OfH3O++Cl−\mathrm { HCl } + \mathrm { H } _ { 2 } \mathrm { Of } \quad \mathrm { H } _ { 3 } \mathrm { O } ^ { + } + \mathrm { Cl } ^ { - }HCl+H2​OfH3​O++Cl− , the number of conjugate acid-base pairs is ____.

The amount of excess CH3CO2H after 6.00 mL of 0.300 M NaOH has been added to 20.0 mL of 0.100M CH3CO2H is _____ mmol CH3CO2H.

The pKa\mathrm { p } K _ { a }pKa​ of hydrochloric acid is _____, if the pKb\mathrm { p } K _ { b }pKb​ of its conjugate base is 8.56 at 25∘C25 ^ { \circ } \mathrm { C }25∘C .

The shape of the titration curve involving a strong acid and a strong base depends only on their identities, not their concentrations.

Which of the following acids will most likely be the strongest?

The larger the atom to which hydrogen is bonded, the stronger the bond.

If the KwK _ { w }Kw​ for water at 80∘C80 ^ { \circ } \mathrm { C }80∘C is 5.60×10−115.60 \times 10 ^ { - 11 }5.60×10−11 , the pKw\mathrm { p } K _ { w }pKw​ for water at the same temperature is _____.

The pH of any neutral solution is equal to the solution's pKw\mathrm { p } K _ { w }pKw​ at that temperature.

Electron delocalization in the conjugate base decreases acid strength.

Introduction to Chemistry

Molecules, Ions, and Chemical Formulas

Chemical Reactions

Reactions in Aqueous Solution

Energy Changes in Chemical Reactions

The Structure of Atoms

The Periodic Table and Periodic Trends

Ionic Versus Covalent Bonding

Molecular Geometry and Covalent Bonding Models

Gases

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Solutions

Chemical Kinetics

Chemical Equilibrium

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A buffer solution contains 0.150 M HCO₂H and 0.225M HCO₂Na and has a pH of 3.75. What is the final pH if 5.00 mL of 1.00M HCl are added to 100.0 mL of this solution?

If the pK_b of a conjugate base is equal to 10.9 at $45.0 ^ { \circ } \mathrm { C }$ , the value of its K_b is _____.

The pH at the midpoint of the titration of a weak acid is equal to the pK_a of the weak acid.

In the reaction $\mathrm { HCl } + \mathrm { H } _ { 2 } \mathrm { Of } \quad \mathrm { H } _ { 3 } \mathrm { O } ^ { + } + \mathrm { Cl } ^ { - }$ , the number of conjugate acid-base pairs is ____.

The amount of excess CH₃CO₂H after 6.00 mL of 0.300 M NaOH has been added to 20.0 mL of 0.100M CH₃CO₂H is _____ mmol CH₃CO₂H.

The $\mathrm { p } K _ { a }$ of hydrochloric acid is _____, if the $\mathrm { p } K _ { b }$ of its conjugate base is 8.56 at $25 ^ { \circ } \mathrm { C }$ .

If the $K _ { w }$ for water at $80 ^ { \circ } \mathrm { C }$ is $5.60 \times 10 ^ { - 11 }$ , the $\mathrm { p } K _ { w }$ for water at the same temperature is _____.

The pH of any neutral solution is equal to the solution's $\mathrm { p } K _ { w }$ at that temperature.