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Questions and Answers
An acid is a proton (H+) ______.
An acid is a proton (H+) ______.
donor
A base is a proton (H+) ______.
A base is a proton (H+) ______.
acceptor
Protons are highly solvated in water and represented by the ______ ion.
Protons are highly solvated in water and represented by the ______ ion.
hydronium
For any base B, its conjugate acid is represented as ______.
For any base B, its conjugate acid is represented as ______.
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The equilibrium constant for proton transfer reactions is represented by ______.
The equilibrium constant for proton transfer reactions is represented by ______.
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The acidity of aqueous solutions is determined by ______.
The acidity of aqueous solutions is determined by ______.
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Sørensen defined pH as ______.
Sørensen defined pH as ______.
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A strong acid has a high ______ and a low pKa.
A strong acid has a high ______ and a low pKa.
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The pKa value is calculated as pKa = ______.
The pKa value is calculated as pKa = ______.
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An example of a polyprotic acid is ______.
An example of a polyprotic acid is ______.
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Study Notes
Acids and Bases
- Acids are proton donors.
- Bases are proton acceptors.
- The most common definition of acids and bases is the Brønsted-Lowry definition.
- A more general definition for acids and bases is the Lewis definition, where:
- An acid is defined as an electron-pair acceptor.
- A base is defined as an electron-pair donor.
Protons in Water
- Protons are highly solvated in water and are represented by the hydronium ion (H3O+).
Conjugate Acids and Bases
- When an acid transfers a proton to water, the acid becomes a conjugate base.
- When a base accepts a proton from water, the base becomes a conjugate acid.
- Acids can be neutral, cationic, or anionic.
- Bases can be anionic, neutral, or cationic.
General Equilibrium for Proton Transfer
- The proton transfer reaction is in equilibrium.
- An equilibrium constant (K) is defined for this reaction, which measures the ratio of products to reactants at equilibrium.
Activity and Concentration
- Equilibrium constants (K) are calculated using the activities of the components in the solution.
- For dilute solutions, activities can be approximated by concentrations.
- The activity (and concentration) of water is considered constant.
Acidity of Aqueous Solutions
- The acidity of an aqueous solution is determined by the concentration of hydronium ions ([H3O+]).
- The pH scale, defined by Sørensen, measures the acidity of a solution.
- The pH scale is expressed as: pH = -log10[H3O+]
- A lower pH value indicates a higher concentration of H3O+ and a more acidic solution.
Acid Dissociation in Water
- The dissociation of an acid (AH) in water is described by an equilibrium constant known as Ka, the acidity constant.
pKa
- The pKa is defined as: pKa = -log10Ka
- pKa is a measure of acid strength.
- A strong acid has a high Ka and a low pKa.
- A weak acid has a low Ka and a high pKa.
Polyprotic Acids
- Polyprotic acids can donate more than one proton.
- The concentration of H3O+ in an aqueous solution of a polyprotic acid is determined by the dissociation constants of each proton.
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Description
This quiz covers the fundamentals of acids and bases, including their definitions according to Brønsted-Lowry and Lewis theories. It also discusses the behavior of protons in water and the concept of conjugate acids and bases. Test your knowledge of these essential chemical concepts.
