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.

How to use these flashcards

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: 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 3: 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 4: 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 5: 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 6: 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 7: Identify the $pH$ of a 0.1 M $HNO_3$ solution.

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

Flashcard 8: Find the pOH of a solution where $pH = 3$.

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

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 main characteristic of a strong acid?

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

Flashcard 11: 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 12: 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 13: 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 14: What is the pH of a 0.01 M HCl solution?

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

Flashcard 15: 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 16: What is the main characteristic of a strong base?

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

Flashcard 17: 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 18: 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 19: 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 20: 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 21: What is the main characteristic of a strong base?

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

Flashcard 22: 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 23: 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 24: Find the pH of a solution where $pOH = 4$.

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

Flashcard 25: 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 26: 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 27: Identify the Lewis definition of a base.

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

Flashcard 28: Identify the Lewis definition of a base.

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

Flashcard 29: State the formula for calculating pOH.

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

Flashcard 30: 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 31: State the formula for calculating pH.

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

Flashcard 32: Find the pOH of a solution where $pH = 3$.

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

Flashcard 33: 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 34: 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 35: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

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

Flashcard 36: 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 37: 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 38: 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 39: 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 40: Identify the Lewis definition of an acid.

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

Flashcard 41: 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 42: 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 43: 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 44: 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 45: 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 46: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

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

Flashcard 47: State the formula for calculating pH.

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

Flashcard 48: 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 49: Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

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

Flashcard 50: What is the pH of a 0.01 M HCl solution?

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

Flashcard 51: Which is a stronger base: NaOH or ammonia?

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

Flashcard 52: 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 53: 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 54: State the formula for calculating pH.

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

Flashcard 55: 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 56: 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 57: 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 58: Which is a stronger base: NaOH or ammonia?

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

Flashcard 59: Calculate the pH given $[H^+] = 1 \times 10^{-8}$ M.

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

Flashcard 60: What is the pH of a 0.01 M NaOH solution?

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

Flashcard 61: 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 62: 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 63: 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 64: 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 65: What is the main characteristic of a strong base?

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

Flashcard 66: 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 67: 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 68: 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 69: Identify the $pH$ of a 0.1 M $KOH$ solution.

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

Flashcard 70: 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 71: Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

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

Flashcard 72: 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 73: What is the main characteristic of a strong acid?

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

Flashcard 74: What is the main characteristic of a strong acid?

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

Flashcard 75: 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 76: State the formula for calculating pH.

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

Flashcard 77: 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 78: What is the main characteristic of a strong acid?

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

Flashcard 79: 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 80: Identify the Lewis definition of an acid.

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

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

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

Flashcard 82: Identify the Lewis definition of a base.

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

Flashcard 83: 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 84: 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 85: Identify the $pH$ of a 0.1 M $HNO_3$ solution.

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

Flashcard 86: 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 87: Which is a stronger base: NaOH or ammonia?

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

Flashcard 88: Calculate the pOH given $[OH^-] = 1 \times 10^{-6}$ M.

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

Flashcard 89: Identify the Lewis definition of an acid.

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

Flashcard 90: What is the main characteristic of a strong base?

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

Flashcard 91: 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 92: 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 93: 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 94: 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 95: Identify the Lewis definition of a base.

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

Flashcard 96: 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 97: Find the pOH of a solution where $pH = 3$.

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

Flashcard 98: 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 99: Identify the Lewis definition of an acid.

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

Flashcard 100: What is the pH of a 0.01 M NaOH solution?

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