AP Chemistry Flashcards: Introduction To Acid Base Reactions

What this deck covers

This deck focuses on Introduction To Acid Base Reactions, giving you a quick way to review the definitions, rules, and examples that matter most for AP Chemistry.

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Work through these flashcards in short sessions. Try to answer each prompt before flipping the card, then revisit any cards you miss until the explanation feels automatic.

Flashcard 1: State the formula for calculating pOH.

Answer: $pOH = -\text{log}[OH^-]$. Negative logarithm converts hydroxide concentration to pOH scale.

Flashcard 2: What is the conjugate base of $H_2SO_4$?

Answer: The conjugate base of $H_2SO_4$ is $HSO_4^-$. Sulfuric acid loses one proton to form bisulfate ion.

Flashcard 3: What is the $K_b$ value indicative of a strong base?

Answer: A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.

Flashcard 4: What is the $K_b$ expression for ammonia, $NH_3$?

Answer: $K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$. Equilibrium expression for weak base ionization.

Flashcard 5: Identify the $pH$ of a 0.1 M $HNO_3$ solution.

Answer: $pH = 1$. Strong acid: $pH = -\log(0.1) = 1$.

Flashcard 6: Find the pOH of a solution where $pH = 3$.

Answer: $pOH = 11$. Use relationship: $pH + pOH = 14$.

Flashcard 7: What are the products of a neutralization reaction?

Answer: A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.

Flashcard 8: Which equation represents the ion-product constant for water ($K_w$)?

Answer: $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.

Flashcard 9: Which ion forms when an acid donates a proton?

Answer: The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.

Flashcard 10: What is the pH of a 0.01 M HCl solution?

Answer: $pH = 2$. Strong acid: $pH = -\log(0.01) = 2$.

Flashcard 11: What is the $K_a$ expression for acetic acid, $CH_3COOH$?

Answer: $K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.

Flashcard 12: What is the $K_a$ value indicative of a strong acid?

Answer: A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.

Flashcard 13: What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

Answer: $K_a \times K_b = K_w$. Fundamental relationship for conjugate acid-base pairs.

Flashcard 14: What is the main characteristic of a strong base?

Answer: A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.

Flashcard 15: What is the term for the equilibrium constant for water?

Answer: The term is $K_w$, the ion-product constant for water. Represents autoionization equilibrium of pure water.

Flashcard 16: What is the definition of an acid according to the Arrhenius theory?

Answer: An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.

Flashcard 17: Identify the Lewis definition of a base.

Answer: A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.

Flashcard 18: Identify the Lewis definition of a base.

Answer: A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.

Flashcard 19: What is the pH of a neutral solution at 25°C?

Answer: The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.

Flashcard 20: State the formula for calculating pH.

Answer: $pH = -\text{log}[H^+]$. Negative logarithm converts concentration to pH scale.

Flashcard 21: Find the pOH of a solution where $pH = 3$.

Answer: $pOH = 11$. Use relationship: $pH + pOH = 14$.

Flashcard 22: What is the $K_a$ expression for acetic acid, $CH_3COOH$?

Answer: $K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.

Flashcard 23: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

Answer: $pH = 8$. Direct application: $pH = -\log(1 \times 10^{-8}) = 8$.

Flashcard 24: Find the $K_a$ value given $pK_a = 3.5$.

Answer: $K_a = 3.16 \times 10^{-4}$. Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$.

Flashcard 25: What is the $K_a$ value indicative of a strong acid?

Answer: A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.

Flashcard 26: What is the relationship between pH and pOH at 25°C?

Answer: $pH + pOH = 14$. Derived from the water equilibrium constant at 25°C.

Flashcard 27: What is the $K_b$ value indicative of a strong base?

Answer: A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.

Flashcard 28: Find the $K_a$ value given $pK_a = 3.5$.

Answer: $K_a = 3.16 \times 10^{-4}$. Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$.

Flashcard 29: What are the products of a neutralization reaction?

Answer: A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.

Flashcard 30: What is the definition of a base according to the Arrhenius theory?

Answer: A base is a substance that increases the concentration of $OH^-$ ions in aqueous solution. Arrhenius theory focuses on $OH^-$ ion production in water.

Flashcard 31: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

Answer: $pH = 8$. Direct application: $pH = -\log(1 \times 10^{-8}) = 8$.

Flashcard 32: State the formula for calculating pH.

Answer: $pH = -\text{log}[H^+]$. Negative logarithm converts concentration to pH scale.

Flashcard 33: Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

Answer: $pOH = 6$. Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$.

Flashcard 34: Which is a stronger base: NaOH or ammonia?

Answer: NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.

Flashcard 35: Name the conjugate base of hydrochloric acid (HCl).

Answer: The conjugate base of HCl is $Cl^-$.. Formed by removing one proton from the acid.

Flashcard 36: State the formula for calculating pH.

Answer: $pH = -\text{log}[H^+]$. Negative logarithm converts concentration to pH scale.

Flashcard 37: What is the $K_b$ value indicative of a strong base?

Answer: A large $K_b$ value indicates a strong base. Large $K_b$ means extensive ionization and stronger basicity.

Flashcard 38: What is the term for the equilibrium constant for water?

Answer: The term is $K_w$, the ion-product constant for water. Represents autoionization equilibrium of pure water.

Flashcard 39: Which ion is responsible for the acidity of a solution?

Answer: The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.

Flashcard 40: What is the pH of a 0.01 M NaOH solution?

Answer: $pH = 12$. Strong base: $pOH = 2$, so $pH = 14 - 2 = 12$.

Flashcard 41: Which equation represents the ion-product constant for water ($K_w$)?

Answer: $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.

Flashcard 42: What is the definition of an acid according to the Arrhenius theory?

Answer: An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.

Flashcard 43: Identify the Bronsted-Lowry definition of an acid.

Answer: A Bronsted-Lowry acid is a proton ($H^+$) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.

Flashcard 44: What is the main characteristic of a strong base?

Answer: A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.

Flashcard 45: Find the $K_b$ value given $pK_b = 4.5$.

Answer: $K_b = 3.16 \times 10^{-5}$. Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$.

Flashcard 46: Which ion is responsible for the acidity of a solution?

Answer: The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.

Flashcard 47: What is the definition of an acid according to the Arrhenius theory?

Answer: An acid is a substance that increases the concentration of $H^+$ ions in aqueous solution. Arrhenius theory focuses on $H^+$ ion production in water.

Flashcard 48: What is the term for the equilibrium constant for water?

Answer: The term is $K_w$, the ion-product constant for water. Represents autoionization equilibrium of pure water.

Flashcard 49: What is the main characteristic of a strong acid?

Answer: A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.

Flashcard 50: What is the main characteristic of a strong acid?

Answer: A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.

Flashcard 51: What is the $K_b$ expression for ammonia, $NH_3$?

Answer: $K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$. Equilibrium expression for weak base ionization.

Flashcard 52: What is the $K_a$ expression for acetic acid, $CH_3COOH$?

Answer: $K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Equilibrium expression for weak acid ionization.

Flashcard 53: What is the main characteristic of a strong acid?

Answer: A strong acid completely ionizes in solution. Nearly 100% ionization in aqueous solution.

Flashcard 54: Identify the Lewis definition of an acid.

Answer: A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.

Flashcard 55: Identify the $pH$ of a 0.1 M $KOH$ solution.

Answer: $pH = 13$. Strong base: $pOH = 1$, so $pH = 14 - 1 = 13$.

Flashcard 56: Name the conjugate base of hydrochloric acid (HCl).

Answer: The conjugate base of HCl is $Cl^-$.. Formed by removing one proton from the acid.

Flashcard 57: Identify the $pH$ of a 0.1 M $HNO_3$ solution.

Answer: $pH = 1$. Strong acid: $pH = -\log(0.1) = 1$.

Flashcard 58: What is the pH of a neutral solution at 25°C?

Answer: The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.

Flashcard 59: Which is a stronger base: NaOH or ammonia?

Answer: NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.

Flashcard 60: Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

Answer: $pOH = 6$. Direct application: $pOH = -\log(1 \times 10^{-6}) = 6$.

Flashcard 61: Identify the Lewis definition of an acid.

Answer: A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.

Flashcard 62: What is the main characteristic of a strong base?

Answer: A strong base completely dissociates in solution. Nearly 100% dissociation in aqueous solution.

Flashcard 63: What is the definition of a base according to the Arrhenius theory?

Answer: A base is a substance that increases the concentration of $OH^-$ ions in aqueous solution. Arrhenius theory focuses on $OH^-$ ion production in water.

Flashcard 64: What is the relationship between pH and pOH at 25°C?

Answer: $pH + pOH = 14$. Derived from the water equilibrium constant at 25°C.

Flashcard 65: What is the $K_a$ value indicative of a strong acid?

Answer: A large $K_a$ value indicates a strong acid. Large $K_a$ means extensive ionization and stronger acidity.

Flashcard 66: Identify the Lewis definition of a base.

Answer: A Lewis base is an electron pair donor. Lewis theory focuses on electron pair interactions.

Flashcard 67: What is the $K_b$ expression for ammonia, $NH_3$?

Answer: $K_b = \frac{[NH_4^+][OH^-]}{[NH_3]}$. Equilibrium expression for weak base ionization.

Flashcard 68: Which is a stronger acid: HCl or acetic acid?

Answer: HCl is a stronger acid than acetic acid. HCl completely ionizes; acetic acid only partially ionizes.

Flashcard 69: Identify the Lewis definition of an acid.

Answer: A Lewis acid is an electron pair acceptor. Lewis theory focuses on electron pair interactions.

Flashcard 70: Find the $K_b$ value given $pK_b = 4.5$.

Answer: $K_b = 3.16 \times 10^{-5}$. Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$.

Flashcard 71: Find the $K_a$ value given $pK_a = 3.5$.

Answer: $K_a = 3.16 \times 10^{-4}$. Use formula: $K_a = 10^{-pK_a} = 10^{-3.5}$.

Flashcard 72: Which ion is responsible for the acidity of a solution?

Answer: The $H^+$ ion is responsible for the acidity of a solution. Higher $[H^+]$ means lower pH and greater acidity.

Flashcard 73: What is the conjugate base of $H_2SO_4$?

Answer: The conjugate base of $H_2SO_4$ is $HSO_4^-$. Sulfuric acid loses one proton to form bisulfate ion.

Flashcard 74: Identify the Bronsted-Lowry definition of a base.

Answer: A Bronsted-Lowry base is a proton ($H^+$) acceptor. Bronsted-Lowry theory emphasizes proton transfer reactions.

Flashcard 75: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

Answer: $pH = 8$. Direct application: $pH = -\log(1 \times 10^{-8}) = 8$.

Flashcard 76: Which is a stronger base: NaOH or ammonia?

Answer: NaOH is a stronger base than ammonia. NaOH completely dissociates; ammonia only partially ionizes.

Flashcard 77: Which ion is responsible for the basicity of a solution?

Answer: The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.

Flashcard 78: What is the pH of a 0.01 M NaOH solution?

Answer: $pH = 12$. Strong base: $pOH = 2$, so $pH = 14 - 2 = 12$.

Flashcard 79: What is the pH of a 0.01 M HCl solution?

Answer: $pH = 2$. Strong acid: $pH = -\log(0.01) = 2$.

Flashcard 80: What are the products of a neutralization reaction?

Answer: A salt and water are the products of a neutralization reaction. General form: acid + base → salt + water.

Flashcard 81: Identify the $pH$ of a 0.1 M $HNO_3$ solution.

Answer: $pH = 1$. Strong acid: $pH = -\log(0.1) = 1$.

Flashcard 82: Name the conjugate base of hydrochloric acid (HCl).

Answer: The conjugate base of HCl is $Cl^-$.. Formed by removing one proton from the acid.

Flashcard 83: What is the pH of a 0.01 M NaOH solution?

Answer: $pH = 12$. Strong base: $pOH = 2$, so $pH = 14 - 2 = 12$.

Flashcard 84: Find the pH of a solution where $pOH = 4$.

Answer: $pH = 10$. Use relationship: $pH + pOH = 14$.

Flashcard 85: Which ion is responsible for the basicity of a solution?

Answer: The $OH^-$ ion is responsible for the basicity of a solution. Higher $[OH^-]$ means higher pH and greater basicity.

Flashcard 86: Name the conjugate acid of ammonia (NH₃).

Answer: The conjugate acid of NH₃ is $NH_4^+$. Formed by adding one proton to the base.

Flashcard 87: What is the conjugate acid of $OH^-$?

Answer: The conjugate acid of $OH^-$ is $H_2O$. Hydroxide ion gains one proton to form water.

Flashcard 88: Which ion forms when an acid donates a proton?

Answer: The conjugate base forms when an acid donates a proton. Result of proton donation in acid-base reactions.

Flashcard 89: What is the pH of a neutral solution at 25°C?

Answer: The pH of a neutral solution at 25°C is 7. At neutral pH, $[H^+] = [OH^-]$ at standard temperature.

Flashcard 90: Identify the $pH$ of a 0.1 M $KOH$ solution.

Answer: $pH = 13$. Strong base: $pOH = 1$, so $pH = 14 - 1 = 13$.

Flashcard 91: State the formula for calculating pOH.

Answer: $pOH = -\text{log}[OH^-]$. Negative logarithm converts hydroxide concentration to pOH scale.

Flashcard 92: What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

Answer: $K_a \times K_b = K_w$. Fundamental relationship for conjugate acid-base pairs.

Flashcard 93: What is the relationship between $K_a$ and $K_b$ for a conjugate acid-base pair?

Answer: $K_a \times K_b = K_w$. Fundamental relationship for conjugate acid-base pairs.

Flashcard 94: What is the conjugate acid of $OH^-$?

Answer: The conjugate acid of $OH^-$ is $H_2O$. Hydroxide ion gains one proton to form water.

Flashcard 95: What is the pH of a 0.01 M HCl solution?

Answer: $pH = 2$. Strong acid: $pH = -\log(0.01) = 2$.

Flashcard 96: Which equation represents the ion-product constant for water ($K_w$)?

Answer: $K_w = [H^+][OH^-] = 1.0 \times 10^{-14}$ at 25°C. This equilibrium constant applies to pure water at 25°C.

Flashcard 97: Identify the Bronsted-Lowry definition of an acid.

Answer: A Bronsted-Lowry acid is a proton ($H^+$) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.

Flashcard 98: Identify the Bronsted-Lowry definition of an acid.

Answer: A Bronsted-Lowry acid is a proton ($H^+$) donor. Bronsted-Lowry theory emphasizes proton transfer reactions.

Flashcard 99: Find the $K_b$ value given $pK_b = 4.5$.

Answer: $K_b = 3.16 \times 10^{-5}$. Use formula: $K_b = 10^{-pK_b} = 10^{-4.5}$.

Flashcard 100: What is the relationship between pH and pOH at 25°C?

Answer: $pH + pOH = 14$. Derived from the water equilibrium constant at 25°C.