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AP Chemistry Flashcards: Molecular Structure Of Acids And Bases

Study Molecular Structure Of Acids And Bases in AP Chemistry with focused flashcards that help you recognize the idea, recall the key rule, and apply it in practice-style prompts.

AP Chemistry

Molecular Structure Of Acids And Bases

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QUESTION
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Which is the conjugate base of H₂SO₄?

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ANSWER

HSO₄⁻. H2SO4H_2SO_4 loses one proton to form HSO4−HSO_4^-.

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This deck focuses on Molecular Structure Of Acids And Bases, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

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Flashcard 1: Which is the conjugate base of H₂SO₄?

Answer: HSO₄⁻. H2SO4H_2SO_4 loses one proton to form HSO4−HSO_4^-.

Flashcard 2: List one example of a strong acid.

Answer: Hydrochloric acid (HCl). One of the seven common strong acids.

Flashcard 3: Define the term 'strong acid'.

Answer: An acid that completely dissociates in solution. Nearly 100% ionization occurs in aqueous solution.

Flashcard 4: What is the Lewis definition of an acid?

Answer: A species that accepts an electron pair. Lewis theory focuses on electron pair interactions, not protons.

Flashcard 5: What is the general formula for calculating pH?

Answer: pH=−log⁡[H+]pH = -\log[H^+]. Negative log of hydrogen ion concentration.

Flashcard 6: What is the definition of a Bronsted-Lowry acid?

Answer: A species that donates a proton (H⁺). This is the proton transfer definition used in acid-base chemistry.

Flashcard 7: Identify the conjugate base of HCl.

Answer: Cl⁻. Formed when HCl loses its proton (H+H^+).

Flashcard 8: What is the general formula for calculating pH?

Answer: pH=−log⁡[H+]pH = -\log[H^+]. Negative log of hydrogen ion concentration.

Flashcard 9: What is the primary component of stomach acid?

Answer: Hydrochloric acid (HCl). Gastric acid is primarily HCl with pH around 1-2.

Flashcard 10: What is the Henderson-Hasselbalch equation for pOH?

Answer: pOH=pKb+log⁡([BH+][B])pOH = pK_b + \log\left(\frac{[BH⁺]}{[B]}\right). Relates buffer pOH to base/acid ratio.

Flashcard 11: What is the definition of a Bronsted-Lowry base?

Answer: A species that accepts a proton (H⁺). This is the proton acceptor definition in Bronsted-Lowry theory.

Flashcard 12: What does a small KaK_a value indicate about an acid?

Answer: The acid is weak, dissociating less in solution. Small KaK_a means lower ionization tendency.

Flashcard 13: What is the effect of dilution on the pH of a buffer?

Answer: Minimal change in pH. Buffer capacity maintains pH despite concentration changes.

Flashcard 14: Identify the Lewis acid in AlCl₃ + Cl⁻ → AlCl₄⁻.

Answer: AlCl₃. AlCl3AlCl_3 accepts the electron pair from Cl−Cl^-.

Flashcard 15: What is the definition of a Bronsted-Lowry acid?

Answer: A species that donates a proton (H⁺). This is the proton transfer definition used in acid-base chemistry.

Flashcard 16: What is the Lewis definition of an acid?

Answer: A species that accepts an electron pair. Lewis theory focuses on electron pair interactions, not protons.

Flashcard 17: State the relationship between pH and pOH.

Answer: pH+pOH=14pH + pOH = 14. This relationship holds at 25°C due to KwK_w.

Flashcard 18: Define the term 'amphoteric'.

Answer: A species that can act as both an acid and a base. Can donate or accept protons depending on conditions.

Flashcard 19: Identify the conjugate base of HCl.

Answer: Cl⁻. Formed when HCl loses its proton (H+H^+).

Flashcard 20: State the relationship between KaK_a and KbK_b for conjugate pairs.

Answer: Ka×Kb=KwK_a \times K_b = K_w. This relationship connects conjugate acid-base pairs.

Flashcard 21: What does a small KaK_a value indicate about an acid?

Answer: The acid is weak, dissociating less in solution. Small KaK_a means lower ionization tendency.

Flashcard 22: Which is stronger: HCl or HF?

Answer: HCl. HCl is a strong acid; HF is weak.

Flashcard 23: State the relationship between KaK_a and KbK_b for conjugate pairs.

Answer: Ka×Kb=KwK_a \times K_b = K_w. This relationship connects conjugate acid-base pairs.

Flashcard 24: What does a large KaK_a value indicate about an acid?

Answer: The acid is strong, dissociating more in solution. Large KaK_a means greater ionization tendency.

Flashcard 25: What does a small KaK_a value indicate about an acid?

Answer: The acid is weak, dissociating less in solution. Small KaK_a means lower ionization tendency.

Flashcard 26: What is the Lewis definition of an acid?

Answer: A species that accepts an electron pair. Lewis theory focuses on electron pair interactions, not protons.

Flashcard 27: What is the Henderson-Hasselbalch equation for pH?

Answer: pH=pKa+log⁡([A−][HA])pH = pK_a + \log\left(\frac{[A⁻]}{[HA]}\right). Relates buffer pH to acid/base ratio.

Flashcard 28: Define the term 'weak base'.

Answer: A base that partially dissociates in solution. Only a small percentage ionizes in aqueous solution.

Flashcard 29: Define the term 'strong base'.

Answer: A base that completely dissociates in solution. Nearly 100% ionization occurs in aqueous solution.

Flashcard 30: Identify the conjugate base of HCl.

Answer: Cl⁻. Formed when HCl loses its proton (H+H^+).

Flashcard 31: What is the primary component of stomach acid?

Answer: Hydrochloric acid (HCl). Gastric acid is primarily HCl with pH around 1-2.

Flashcard 32: Identify the Lewis base in NH₃ + BF₃ → NH₃BF₃.

Answer: NH₃. NH3NH_3 donates its lone pair to BF3BF_3.

Flashcard 33: What is a buffer solution?

Answer: A solution that resists changes in pH when acids or bases are added. Contains weak acid/base and conjugate pairs.

Flashcard 34: What is the definition of a Bronsted-Lowry base?

Answer: A species that accepts a proton (H⁺). This is the proton acceptor definition in Bronsted-Lowry theory.

Flashcard 35: Define the term 'weak acid'.

Answer: An acid that partially dissociates in solution. Only a small percentage ionizes in aqueous solution.

Flashcard 36: List one example of a strong base.

Answer: Sodium hydroxide (NaOH). One of the common strong bases.

Flashcard 37: Which is the conjugate base of H₂SO₄?

Answer: HSO₄⁻. H2SO4H_2SO_4 loses one proton to form HSO4−HSO_4^-.

Flashcard 38: What is the Lewis definition of an acid?

Answer: A species that accepts an electron pair. Lewis theory focuses on electron pair interactions, not protons.

Flashcard 39: List one example of a weak base.

Answer: Ammonia (NH₃). A common weak base that accepts protons from water.

Flashcard 40: List one example of a weak base.

Answer: Ammonia (NH₃). A common weak base that accepts protons from water.

Flashcard 41: What is the formula for calculating pOH?

Answer: pOH=−log⁡[OH−]pOH = -\log[OH⁻]. Negative log of hydroxide ion concentration.

Flashcard 42: Which is stronger: HCl or HF?

Answer: HCl. HCl is a strong acid; HF is weak.

Flashcard 43: What is the Henderson-Hasselbalch equation for pH?

Answer: pH=pKa+log⁡([A−][HA])pH = pK_a + \log\left(\frac{[A⁻]}{[HA]}\right). Relates buffer pH to acid/base ratio.

Flashcard 44: What is the formula for the base dissociation constant, KbK_b?

Answer: Kb=[BH+][OH−][B]K_b = \frac{[BH⁺][OH⁻]}{[B]}. Measures the extent of base dissociation in solution.

Flashcard 45: What is a buffer solution?

Answer: A solution that resists changes in pH when acids or bases are added. Contains weak acid/base and conjugate pairs.

Flashcard 46: What is the common ion effect?

Answer: The shift in equilibrium due to the addition of a common ion. Suppresses ionization of weak acids or bases.

Flashcard 47: Identify an example of an amphoteric substance.

Answer: Water (H₂O). Can act as acid or base in different reactions.

Flashcard 48: What is the definition of a Bronsted-Lowry base?

Answer: A species that accepts a proton (H⁺). This is the proton acceptor definition in Bronsted-Lowry theory.

Flashcard 49: Define the term 'weak acid'.

Answer: An acid that partially dissociates in solution. Only a small percentage ionizes in aqueous solution.

Flashcard 50: Define the term 'weak acid'.

Answer: An acid that partially dissociates in solution. Only a small percentage ionizes in aqueous solution.

Flashcard 51: What does a small KaK_a value indicate about an acid?

Answer: The acid is weak, dissociating less in solution. Small KaK_a means lower ionization tendency.

Flashcard 52: What is the Henderson-Hasselbalch equation for pOH?

Answer: pOH=pKb+log⁡([BH+][B])pOH = pK_b + \log\left(\frac{[BH^+]}{[B]}\right). Relates buffer pOH to base/acid ratio.

Flashcard 53: Identify the Lewis acid in AlCl₃ + Cl⁻ → AlCl₄⁻.

Answer: AlCl₃. AlCl3AlCl_3 accepts the electron pair from Cl−Cl^-.

Flashcard 54: Identify an example of an amphoteric substance.

Answer: Water (H₂O). Can act as acid or base in different reactions.

Flashcard 55: Identify the Lewis base in NH₃ + BF₃ → NH₃BF₃.

Answer: NH₃. NH3NH_3 donates its lone pair to BF3BF_3.

Flashcard 56: Identify the conjugate base of HCl.

Answer: Cl⁻. Formed when HCl loses its proton (H+H^+).

Flashcard 57: What is the Henderson-Hasselbalch equation for pOH?

Answer: pOH=pKb+log⁡([BH+][B])pOH = pK_b + \log\left(\frac{[BH^+]}{[B]}\right). Relates buffer pOH to base/acid ratio.

Flashcard 58: What does a large KaK_a value indicate about an acid?

Answer: The acid is strong, dissociating more in solution. Large KaK_a means greater ionization tendency.

Flashcard 59: Define the term 'strong base'.

Answer: A base that completely dissociates in solution. Nearly 100% ionization occurs in aqueous solution.

Flashcard 60: Which is stronger: HCl or HF?

Answer: HCl. HCl is a strong acid; HF is weak.

Flashcard 61: Identify the common ion in a mixture of HCl and NaCl.

Answer: Cl⁻. Both compounds contain chloride ions.

Flashcard 62: What is the pH of a solution with [H+]=1×10−3[H⁺] = 1 \times 10^{-3} M?

Answer:

  1. Using pH=−log⁡(1×10−3)=3pH = -\log(1 \times 10^{-3}) = 3.

Flashcard 63: Identify an example of an amphoteric substance.

Answer: Water (H₂O). Can act as acid or base in different reactions.

Flashcard 64: List one example of a strong base.

Answer: Sodium hydroxide (NaOH). One of the common strong bases.

Flashcard 65: State the relationship between pH and pOH.

Answer: pH+pOH=14pH + pOH = 14. This relationship holds at 25°C due to KwK_w.

Flashcard 66: What is the Lewis definition of a base?

Answer: A species that donates an electron pair. Lewis bases are electron pair donors in chemical reactions.

Flashcard 67: Define the term 'amphoteric'.

Answer: A species that can act as both an acid and a base. Can donate or accept protons depending on conditions.

Flashcard 68: Identify the Lewis base in NH₃ + BF₃ → NH₃BF₃.

Answer: NH₃. NH3NH_3 donates its lone pair to BF3BF_3.

Flashcard 69: What is the effect of dilution on the pH of a buffer?

Answer: Minimal change in pH. Buffer capacity maintains pH despite concentration changes.

Flashcard 70: Identify the Lewis acid in AlCl₃ + Cl⁻ → AlCl₄⁻.

Answer: AlCl₃. AlCl3AlCl_3 accepts the electron pair from Cl−Cl^-.

Flashcard 71: List one example of a weak base.

Answer: Ammonia (NH₃). A common weak base that accepts protons from water.

Flashcard 72: Define the term 'strong acid'.

Answer: An acid that completely dissociates in solution. Nearly 100% ionization occurs in aqueous solution.

Flashcard 73: Identify the Lewis base in NH₃ + BF₃ → NH₃BF₃.

Answer: NH₃. NH3NH_3 donates its lone pair to BF3BF_3.

Flashcard 74: Identify the Lewis acid in AlCl₃ + Cl⁻ → AlCl₄⁻.

Answer: AlCl₃. AlCl3AlCl_3 accepts the electron pair from Cl−Cl^-.

Flashcard 75: What is the Lewis definition of a base?

Answer: A species that donates an electron pair. Lewis bases are electron pair donors in chemical reactions.

Flashcard 76: What is the value of KwK_w at 25°C?

Answer: 1.0×10−141.0 \times 10^{-14}. The ion product constant for water at standard temperature.

Flashcard 77: What does a large KaK_a value indicate about an acid?

Answer: The acid is strong, dissociating more in solution. Large KaK_a means greater ionization tendency.

Flashcard 78: What is the pH of a buffer with equal concentrations of acid and base?

Answer: pH = pK_a. When log⁡(1)=0\log(1) = 0, so pH equals pKapK_a.

Flashcard 79: What is the pOH of a solution with [OH−]=1×10−5[OH⁻] = 1 \times 10^{-5} M?

Answer:

  1. Using pOH=−log⁡(1×10−5)=5pOH = -\log(1 \times 10^{-5}) = 5.

Flashcard 80: Which is stronger: HCl or HF?

Answer: HCl. HCl is a strong acid; HF is weak.

Flashcard 81: What is the primary component of stomach acid?

Answer: Hydrochloric acid (HCl). Gastric acid is primarily HCl with pH around 1-2.

Flashcard 82: What is the Henderson-Hasselbalch equation for pH?

Answer: pH=pKa+log⁡([A−][HA])pH = pK_a + \log\left(\frac{[A⁻]}{[HA]}\right). Relates buffer pH to acid/base ratio.

Flashcard 83: What is the effect of dilution on the pH of a buffer?

Answer: Minimal change in pH. Buffer capacity maintains pH despite concentration changes.

Flashcard 84: List one example of a weak base.

Answer: Ammonia (NH₃). A common weak base that accepts protons from water.

Flashcard 85: What is a buffer solution?

Answer: A solution that resists changes in pH when acids or bases are added. Contains weak acid/base and conjugate pairs.

Flashcard 86: What is the formula for the base dissociation constant, KbK_b?

Answer: Kb=[BH+][OH−][B]K_b = \frac{[BH^+][OH^-]}{[B]}. Measures the extent of base dissociation in solution.

Flashcard 87: Define the term 'amphoteric'.

Answer: A species that can act as both an acid and a base. Can donate or accept protons depending on conditions.

Flashcard 88: What is the pH of a buffer with equal concentrations of acid and base?

Answer: pH = pK_a. When log⁡(1)=0\log(1) = 0, so pH equals pKapK_a.

Flashcard 89: What is the pOH of a solution with [OH−]=1×10−5[OH⁻] = 1 \times 10^{-5} M?

Answer:

  1. Using pOH=−log⁡(1×10−5)=5pOH = -\log(1 \times 10^{-5}) = 5.

Flashcard 90: List one example of a strong acid.

Answer: Hydrochloric acid (HCl). One of the seven common strong acids.

Flashcard 91: What is the formula for calculating pOH?

Answer: pOH=−log⁡[OH−]pOH = -\log[OH^{-}]. Negative log of hydroxide ion concentration.

Flashcard 92: What is the primary component of stomach acid?

Answer: Hydrochloric acid (HCl). Gastric acid is primarily HCl with pH around 1-2.

Flashcard 93: List one example of a strong acid.

Answer: Hydrochloric acid (HCl). One of the seven common strong acids.

Flashcard 94: State the relationship between KaK_a and KbK_b for conjugate pairs.

Answer: Ka×Kb=KwK_a \times K_b = K_w. This relationship connects conjugate acid-base pairs.

Flashcard 95: What is the formula for the base dissociation constant, KbK_b?

Answer: Kb=[BH+][OH−][B]K_b = \frac{[BH⁺][OH⁻]}{[B]}. Measures the extent of base dissociation in solution.

Flashcard 96: What is the Henderson-Hasselbalch equation for pOH?

Answer: pOH=pKb+log⁡([BH+][B])pOH = pK_b + \log\left(\frac{[BH⁺]}{[B]}\right). Relates buffer pOH to base/acid ratio.

Flashcard 97: What is the common ion effect?

Answer: The shift in equilibrium due to the addition of a common ion. Suppresses ionization of weak acids or bases.

Flashcard 98: What is the general formula for calculating pH?

Answer: pH=−log⁡[H+]pH = -\log[H^+]. Negative log of hydrogen ion concentration.

Flashcard 99: What is the general formula for calculating pH?

Answer: pH=−log⁡[H+]pH = -\log[H⁺]. Negative log of hydrogen ion concentration.

Flashcard 100: What is a buffer solution?

Answer: A solution that resists changes in pH when acids or bases are added. Contains weak acid/base and conjugate pairs.