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Questions and Answers
What characterizes an Arrhenius acid?
What characterizes an Arrhenius acid?
- Forms a covalent bond with bases
- Is only defined in gaseous states
- Releases H+ ions in solution (correct)
- Produces OH- ions in water
How does the Bronsted–Lowry definition of a base differ from that of Arrhenius?
How does the Bronsted–Lowry definition of a base differ from that of Arrhenius?
- It is restricted to specific reactions
- It only considers gas-phase reactions
- It applies to non-aqueous solutions (correct)
- It only includes hydroxide ions
What is an example of a monoprotic acid?
What is an example of a monoprotic acid?
- H3PO4
- HCl (correct)
- H2SO4
- H2CO3
Which of the following statements is true about polyprotic acids?
Which of the following statements is true about polyprotic acids?
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In the reaction between NH3 and HCl, which component acts as a Bronsted–Lowry acid?
In the reaction between NH3 and HCl, which component acts as a Bronsted–Lowry acid?
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Which of the following describes a Lewis acid?
Which of the following describes a Lewis acid?
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What is the primary factor affecting the pH calculation of a monoprotic acid?
What is the primary factor affecting the pH calculation of a monoprotic acid?
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What is the active species in the Bronsted–Lowry model of acid-base reactions?
What is the active species in the Bronsted–Lowry model of acid-base reactions?
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Study Notes
Arrhenius Acid-Base Theory
- Arrhenius defined acids as substances that produce hydrogen ions (H+) when dissolved in water.
- Arrhenius defined bases as substances that produce hydroxide ions (OH-) when dissolved in water.
Limitations of Arrhenius Theory
- The Arrhenius theory only applies to substances in aqueous solutions, doesn't account for reactions in other solvents.
- The theory only considers the production of H+ and OH- ions, limiting its applicability to substances that release these ions explicitly.
Bronsted-Lowry Acid-Base Theory
- The Bronsted-Lowry definition of an acid is similar to Arrhenius, but it is not limited to aqueous solutions.
- Bronsted-Lowry defines an acid as a proton donor (H+).
- Bronsted-Lowry defines a base as a proton acceptor (H+).
Lewis Acid-Base Theory
- The Lewis theory defines an acid as an electron pair acceptor.
- The Lewis theory defines a base as an electron pair donor.
Polyprotic Acids
- Polyprotic acids donate multiple protons per molecule.
- They have more than one ionizable H+ atom in their structure.
- Protons are released in stages, with the first proton being the easiest to remove.
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