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Questions and Answers
What produces H+ ions in solution according to the Arrhenius definition?
What produces H+ ions in solution according to the Arrhenius definition?
What are the common formulas of bases?
What are the common formulas of bases?
NaOH, KOH, Ca(OH)2
A base produces H+ ions in solution.
A base produces H+ ions in solution.
False
Which of the following is an example of a strong acid?
Which of the following is an example of a strong acid?
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What is the conjugate base of HCl?
What is the conjugate base of HCl?
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Stronger acids have stronger conjugate bases.
Stronger acids have stronger conjugate bases.
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What defines a monoprotic acid?
What defines a monoprotic acid?
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H2SO4 (aq) + H2O (l) -> __________ + HSO4^-
H2SO4 (aq) + H2O (l) -> __________ + HSO4^-
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Which of the following is a property of weak acids?
Which of the following is a property of weak acids?
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The term for acids with more than one ionizable hydrogen is __________ acid.
The term for acids with more than one ionizable hydrogen is __________ acid.
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What is the strength comparison of HClO3 and HBrO3 based on electronegativity?
What is the strength comparison of HClO3 and HBrO3 based on electronegativity?
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Study Notes
Arrhenius Definition of Acids and Bases
- An Arrhenius acid produces H+ ions in solution.
- Common acids start with "H" in their formula.
- An Arrhenius base produces OH- ions in solution.
- Metal hydroxides are common bases: examples include NaOH, KOH, and Ca(OH)2.
Bronsted-Lowry Definition of Acids and Bases
- An acid is a proton (H+) donor.
- A base is a proton (H+) acceptor.
- Example: In the reaction HCl + NH3 → NH4+ + Cl-, HCl is the acid, NH3 is the base, NH4+ is the conjugate acid, and Cl- is the conjugate base.
Lewis Definition of Acids and Bases
- A Lewis acid is an electron pair acceptor.
- A Lewis base is an electron pair donor.
Strong Acids and Weak Acids
- Strong acids completely dissociate in solutions, behaving as strong electrolytes.
- Weak acids only partially dissociate, meaning they exist in equilibrium between the undissociated acid form and its ions.
- Strong acids include perchloric acid (HClO4), hydrochloric acid (HCl), sulfuric acid (H2SO4), and nitric acid (HNO3).
- Weak acids include carbonic acid (H2CO3), hydrocyanic acid (HCN), and hydrofluoric acid (HF).
Strong Bases and Weak Bases
- Strong bases include lithium hydroxide (LiOH), sodium hydroxide (NaOH), and potassium hydroxide (KOH)
- Other metal hydroxides, like Al(OH)3 and Mg(OH)2, classify as weak bases.
- Ammonia (NH3) and its derivatives are weak bases.
Binary Acids
- Contain acidic hydrogens attached to a nonmetal ion.
- Examples: HCl, HF.
- Their strength depends on the electronegativity of the nonmetal and the bond strength.
- For elements in the same group (F, Cl, Br, I), the strength increases down the group due to weaker bond strength.
- For elements in the same row, the strength increases with increasing electronegativity.
Oxy-Acids
- Contain acidic hydrogens attached to a nonmetal ion and an oxygen atom.
- Their general formula is H-O-Y, where "Y" is the nonmetal.
- The strength of oxy-acids depends on the electronegativity of Y.
- Greater electronegativity of Y correlates to a stronger acid.
Conjugate Bases
- Stronger acids have weaker conjugate bases (C-bases).
- Weaker acids have stronger conjugate bases.
Monoprotic and Polyprotic Acids
- Monoprotic acids release one proton (H+) per molecule.
- Polyprotic acids release more than one proton per molecule.
- Diprotic acids release two protons (H+).
- Triprotic acids release three protons (H+).
- In polyprotic acids, the first hydrogen ion is ionized easier than the second. For example, H2SO4 is a stronger acid than HSO4-.
Polyprotic Acid Example: Sulfuric Acid (H2SO4)
- First ionization: H2SO4 (aq) + H2O(l) -> (H3O+) + HSO4^-
- Second ionization: HSO4 (aq) + H2O(l) -> (H3O+) + SO4^2-
- The first hydrogen ion in sulfuric acid ionizes more easily than the second, making H2SO4 a stronger acid than HSO4-.
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Description
Test your understanding of acid-base theories including Arrhenius, Bronsted-Lowry, and Lewis definitions. Familiarize yourself with strong and weak acids and their characteristics. This quiz will help solidify your knowledge in chemistry.
