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Questions and Answers
What best describes an amphiprotic species?
What best describes an amphiprotic species?
- A species that can act only as an acid.
- A species that can act as either an acid or a base. (correct)
- A species that can act only as a base.
- A species that cannot donate or accept protons.
Lewis acids are defined as substances that can accept protons.
Lewis acids are defined as substances that can accept protons.
False (B)
Give two examples of Lewis bases.
Give two examples of Lewis bases.
Ammonia (NH3) and water (H2O)
The formula for calculating pH from the concentration of hydrogen ions, [H+], is ______.
The formula for calculating pH from the concentration of hydrogen ions, [H+], is ______.
Match the following compounds with their classification as Arrhenius acid or base:
Match the following compounds with their classification as Arrhenius acid or base:
What is the conjugate base of H2PO4−?
What is the conjugate base of H2PO4−?
HCl is considered a weak acid.
HCl is considered a weak acid.
In the reaction NH3 + H2PO4− ⇌ NH4+ + HPO4²−, what role does NH3 play?
In the reaction NH3 + H2PO4− ⇌ NH4+ + HPO4²−, what role does NH3 play?
The reaction of HCl with H2PO4− results in the formation of ______ and H3PO4.
The reaction of HCl with H2PO4− results in the formation of ______ and H3PO4.
Match the acid-base pairs with their respective classifications:
Match the acid-base pairs with their respective classifications:
Which statement correctly describes the relationship between a strong acid and its conjugate base?
Which statement correctly describes the relationship between a strong acid and its conjugate base?
What ions are formed during the auto ionization of water?
What ions are formed during the auto ionization of water?
Which of the following is an amphiprotic species?
Which of the following is an amphiprotic species?
All Brønsted-Lowry acids are also Lewis acids.
All Brønsted-Lowry acids are also Lewis acids.
What is the self-ionization of ammonia?
What is the self-ionization of ammonia?
According to the Lewis definition, an acid is any species that accepts an __________ pair to form a bond.
According to the Lewis definition, an acid is any species that accepts an __________ pair to form a bond.
Which of the following pairs demonstrates a correct Lewis acid-base reaction?
Which of the following pairs demonstrates a correct Lewis acid-base reaction?
What is a key limitation of the Brønsted-Lowry definition of acids and bases?
What is a key limitation of the Brønsted-Lowry definition of acids and bases?
Which group contains the strongest acid?
Which group contains the strongest acid?
Amphiprotic species can only donate protons.
Amphiprotic species can only donate protons.
Match the following species with their type:
Match the following species with their type:
Lewis acids accept __________ to form bonds.
Lewis acids accept __________ to form bonds.
What is the correct expression for the acid-dissociation constant (Ka) for a weak acid (HA)?
What is the correct expression for the acid-dissociation constant (Ka) for a weak acid (HA)?
Weak acids have higher Ka values compared to strong acids.
Weak acids have higher Ka values compared to strong acids.
What does the symbol Ka represent in acid-base chemistry?
What does the symbol Ka represent in acid-base chemistry?
The ionization constant of _____ acid is represented in the table.
The ionization constant of _____ acid is represented in the table.
Match the following weak acids with their corresponding Ka values:
Match the following weak acids with their corresponding Ka values:
Which weak acid has the highest Ka value based on the provided data?
Which weak acid has the highest Ka value based on the provided data?
The concentration of water in the acid-dissociation constant expression is constant.
The concentration of water in the acid-dissociation constant expression is constant.
List one characteristic of weak acids.
List one characteristic of weak acids.
The numerical value of _____ is a reflection of the strength of the acid.
The numerical value of _____ is a reflection of the strength of the acid.
Flashcards
Amphiprotic Species
Amphiprotic Species
A substance that can act as both an acid and a base, donating or accepting protons (H+).
Lewis Acid
Lewis Acid
A substance that can accept a pair of electrons to form a covalent bond.
Lewis Base
Lewis Base
A substance that can donate a pair of electrons to form a covalent bond.
pH Calculation
pH Calculation
Calculating pH from H+ concentration, or vice versa. Similarly for pOH from OH- concentration.
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Arrhenius Acid
Arrhenius Acid
A substance that increases the concentration of H+ ions in an aqueous solution.
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Brønsted-Lowry Acid
Brønsted-Lowry Acid
A substance that donates a proton (H+).
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Brønsted-Lowry Base
Brønsted-Lowry Base
A substance that accepts a proton (H+).
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Conjugate Acid
Conjugate Acid
The species formed when a base accepts a proton.
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Conjugate Base
Conjugate Base
The species formed when an acid loses a proton.
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Strong Acid
Strong Acid
An acid that completely dissociates in water to release H+ ions.
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Strong Base
Strong Base
A base that completely accepts protons from water, dissociating completely.
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Autoionization of Water
Autoionization of Water
The reaction of two water molecules forming a hydroxide ion and a hydronium ion.
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H2PO4- is amphiprotic
H2PO4- is amphiprotic
H2PO4- can act as an acid by donating a proton to form HPO42-, and it can act as a base by accepting a proton to form H3PO4.
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H2O is amphiprotic
H2O is amphiprotic
Water can act as an acid by donating a proton to form OH-, and it can act as a base by accepting a proton to form H3O+.
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Strongest base? (OH-, Cl-, NO2-, CH3COO-, NH3)
Strongest base? (OH-, Cl-, NO2-, CH3COO-, NH3)
OH- is the strongest base in the given group. Bases accept protons. Hydroxide readily accepts protons.
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Strongest acid? (HClO4, CH3COOH, HNO3, HCl)
Strongest acid? (HClO4, CH3COOH, HNO3, HCl)
HClO4 (perchloric acid) is the strongest acid in the group. Acids donate protons. Perchloric acid readily ionizes to donate H+.
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Brønsted-Lowry Theory Weakness
Brønsted-Lowry Theory Weakness
The Brønsted-Lowry theory focuses solely on proton transfer and cannot explain acid-base reactions in non-aqueous solvents.
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Self-ionization of Ammonia
Self-ionization of Ammonia
2NH3(l) ⇌ NH4+(am) + NH2-(am)
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Lewis Acid-Base vs. Brønsted-Lowry
Lewis Acid-Base vs. Brønsted-Lowry
Lewis definition is broader, including electron pair donation/acceptance. Brønsted-Lowry only deals with proton transfer.
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Are ALL Brønsted-Lowry acids/bases Lewis acids/bases?
Are ALL Brønsted-Lowry acids/bases Lewis acids/bases?
Yes, all Brønsted-Lowry acids/bases are also Lewis acids/bases. Proton transfer involves electron pair movement.
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Weak Acid
Weak Acid
An acid that only partially ionizes in water, meaning it doesn't completely donate all its protons (H+).
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Acid Dissociation Constant (Ka)
Acid Dissociation Constant (Ka)
A measure of the strength of a weak acid. It represents the equilibrium constant for the ionization of the acid in water.
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What does a higher Ka value mean for an acid?
What does a higher Ka value mean for an acid?
A higher Ka value indicates a stronger acid, meaning it ionizes to a greater extent in water, releasing more H+ ions.
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Equilibrium Constant Expression for Weak Acid
Equilibrium Constant Expression for Weak Acid
The ratio of the product of the concentrations of the hydronium ions (H3O+) and the conjugate base (A-) to the concentration of the undissociated acid (HA).
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Why is water's concentration not included in Ka?
Why is water's concentration not included in Ka?
The concentration of water in dilute solutions is nearly constant and doesn't significantly change during the ionization process.
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How is Ka related to the strength of an acid?
How is Ka related to the strength of an acid?
A higher Ka value indicates a stronger acid, as it ionizes to a greater extent, generating more H+ ions.
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Monoprotic Acid
Monoprotic Acid
An acid that can donate only one proton (H+) per molecule when dissolved in water.
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Ionization of Weak Acid
Ionization of Weak Acid
The process where a weak acid partially donates protons (H+) to water molecules, forming hydronium ions (H3O+) and the conjugate base of the acid.
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What does the table of ionization constants indicate?
What does the table of ionization constants indicate?
The table shows the Ka values for various weak monoprotic acids. It highlights the relative strengths of these acids based on their respective Ka values.
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