AP Chemistry Flashcards: Introduction To Acids And Bases

What this deck covers

This deck focuses on Introduction To Acids And Bases, 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: Identify the pH range for acidic solutions.

Answer: Acidic solutions have a pH less than 7. Higher $[H^+]$ than $[OH^-]$.

Flashcard 2: What is the $pK_b$ expression for a base?

Answer: $pK_b = -\text{log}_{10} K_b$. Negative logarithm of base dissociation constant.

Flashcard 3: Identify the conjugate base of $H_2O$.

Answer: The conjugate base of $H_2O$ is $OH^-$.. Loses a proton to form the conjugate base.

Flashcard 4: What is a Lewis acid?

Answer: A Lewis acid is an electron pair acceptor. Receives an electron pair from a donor.

Flashcard 5: State the formula for calculating pH.

Answer: $pH = -\text{log}_{10} [H^+]$. Negative logarithm of hydrogen ion concentration.

Flashcard 6: Identify the pH range for acidic solutions.

Answer: Acidic solutions have a pH less than 7. Higher $[H^+]$ than $[OH^-]$.

Flashcard 7: What is the relationship between pH and pOH?

Answer: $pH + pOH = 14$ at 25°C. Based on the ion product of water.

Flashcard 8: Identify the conjugate acid of $OH^-$.

Answer: The conjugate acid of $OH^-$ is $H_2O$. Gains a proton to form the conjugate acid.

Flashcard 9: Which ion is common in all basic solutions?

Answer: The common ion is $OH^-$. Present in all aqueous base solutions.

Flashcard 10: What is the $pH$ of a $0.001$ M $NaOH$ solution?

Answer: $pH = 11$. Strong base: $pOH = 3$, so $pH = 14 - 3$.

Flashcard 11: What is the definition of a strong acid?

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

Flashcard 12: What is the $pH$ of a $0.01$ M $HCl$ solution?

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

Flashcard 13: Identify the conjugate acid of $NH_3$.

Answer: The conjugate acid of $NH_3$ is $NH_4^+$.. Gains a proton to form the conjugate acid.

Flashcard 14: What is the definition of an acid according to Arrhenius?

Answer: An acid increases $[H^+]$ in aqueous solution. Releases hydrogen ions when dissolved.

Flashcard 15: What is the $K_a$ expression for $HA \rightleftharpoons H^+ + A^-$?

Answer: $K_a = \frac{[H^+][A^-]}{[HA]}$. Equilibrium expression for acid dissociation.

Flashcard 16: Which base is stronger: $NaOH$ or $NH_3$?

Answer: $NaOH$ is stronger than $NH_3$. $NaOH$ is strong, $NH_3$ is weak.

Flashcard 17: What is the definition of a weak acid?

Answer: A weak acid partially ionizes in solution. Incomplete dissociation in aqueous solution.

Flashcard 18: What is a Lewis base?

Answer: A Lewis base is an electron pair donor. Provides an electron pair to an acceptor.

Flashcard 19: Which base is stronger: $NaOH$ or $NH_3$?

Answer: $NaOH$ is stronger than $NH_3$. $NaOH$ is strong, $NH_3$ is weak.

Flashcard 20: What is the pH of a neutral solution at 25°C?

Answer: The pH of a neutral solution is 7. Equal concentrations of $H^+$ and $OH^-$.

Flashcard 21: Identify the conjugate base of $H_2SO_4$.

Answer: The conjugate base of $H_2SO_4$ is $HSO_4^-$. Loses one proton from diprotic acid.

Flashcard 22: What is the definition of a strong base?

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

Flashcard 23: What is the definition of a base according to Arrhenius?

Answer: A base increases $[OH^-]$ in aqueous solution. Releases hydroxide ions when dissolved.

Flashcard 24: How does increasing $[OH^-]$ affect pOH?

Answer: Increasing $[OH^-]$ decreases pOH. pOH decreases as basicity increases.

Flashcard 25: What is the pH of pure water at 25°C?

Answer: The pH of pure water is 7. Neutral because $[H^+] = [OH^-]$.

Flashcard 26: What is the pH of pure water at 25°C?

Answer: The pH of pure water is 7. Neutral because $[H^+] = [OH^-]$.

Flashcard 27: Which ion is common in all acidic solutions?

Answer: The common ion is $H^+$. Present in all aqueous acid solutions.

Flashcard 28: Identify the conjugate acid of $OH^-$.

Answer: The conjugate acid of $OH^-$ is $H_2O$. Gains a proton to form the conjugate acid.

Flashcard 29: What is the ion product constant for water ($K_w$) at 25°C?

Answer: $K_w = 1.0 \times 10^{-14}$ at 25°C. Product of $[H^+]$ and $[OH^-]$ concentrations.

Flashcard 30: What is the effect of temperature on $K_w$ of water?

Answer: $K_w$ increases with temperature. Higher temperature increases ion product.

Flashcard 31: What is a Lewis base?

Answer: A Lewis base is an electron pair donor. Provides an electron pair to an acceptor.

Flashcard 32: Define a Brønsted-Lowry base.

Answer: A Brønsted-Lowry base is a proton acceptor. Receives $H^+$ from another species.

Flashcard 33: Define a Brønsted-Lowry base.

Answer: A Brønsted-Lowry base is a proton acceptor. Receives $H^+$ from another species.

Flashcard 34: What is the definition of a weak base?

Answer: A weak base partially dissociates in solution. Incomplete dissociation in aqueous solution.

Flashcard 35: What is the definition of a strong base?

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

Flashcard 36: What is the definition of a base according to Arrhenius?

Answer: A base increases $[OH^-]$ in aqueous solution. Releases hydroxide ions when dissolved.

Flashcard 37: Which acid is stronger: $HCl$ or $HF$?

Answer: $HCl$ is stronger than $HF$. $HCl$ is a strong acid, $HF$ is weak.

Flashcard 38: What is the pOH of a solution with $[OH^-] = 1.0 \times 10^{-4}$ M?

Answer: $pOH = 4$. Calculated using $pOH = -\log[OH^-]$.

Flashcard 39: Which acid is stronger: $HCl$ or $HF$?

Answer: $HCl$ is stronger than $HF$. $HCl$ is a strong acid, $HF$ is weak.

Flashcard 40: How does increasing $[OH^-]$ affect pOH?

Answer: Increasing $[OH^-]$ decreases pOH. pOH decreases as basicity increases.

Flashcard 41: What is the $pK_a$ expression for an acid?

Answer: $pK_a = -\text{log}_{10} K_a$. Negative logarithm of acid dissociation constant.

Flashcard 42: What is the $K_w$ expression for water?

Answer: $K_w = [H^+][OH^-]$. Autoionization equilibrium expression for water.

Flashcard 43: What is the $K_w$ expression for water?

Answer: $K_w = [H^+][OH^-]$. Autoionization equilibrium expression for water.

Flashcard 44: Which ion is common in all acidic solutions?

Answer: The common ion is $H^+$. Present in all aqueous acid solutions.

Flashcard 45: Identify the conjugate base of $H_2SO_4$.

Answer: The conjugate base of $H_2SO_4$ is $HSO_4^-$. Loses one proton from diprotic acid.

Flashcard 46: Identify the conjugate acid of $NH_3$.

Answer: The conjugate acid of $NH_3$ is $NH_4^+$.. Gains a proton to form the conjugate acid.

Flashcard 47: Identify the pH range for basic solutions.

Answer: Basic solutions have a pH greater than 7. Higher $[OH^-]$ than $[H^+]$.

Flashcard 48: Define a Brønsted-Lowry acid.

Answer: A Brønsted-Lowry acid is a proton donor. Gives up $H^+$ to another species.

Flashcard 49: What is the $pH$ of a $0.01$ M $HCl$ solution?

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

Flashcard 50: What is the $pK_a$ expression for an acid?

Answer: $pK_a = -\text{log}_{10} K_a$. Negative logarithm of acid dissociation constant.

Flashcard 51: Identify the conjugate base of $H_2O$.

Answer: The conjugate base of $H_2O$ is $OH^-$.. Loses a proton to form the conjugate base.

Flashcard 52: What is the definition of an acid according to Arrhenius?

Answer: An acid increases $[H^+]$ in aqueous solution. Releases hydrogen ions when dissolved.

Flashcard 53: What is the $K_a$ expression for $HA \rightleftharpoons H^+ + A^-$?

Answer: $K_a = \frac{[H^+][A^-]}{[HA]}$. Equilibrium expression for acid dissociation.

Flashcard 54: What is the pOH of a solution with $[OH^-] = 1.0 \times 10^{-4}$ M?

Answer: $pOH = 4$. Calculated using $pOH = -\log[OH^-]$.

Flashcard 55: How does increasing $[H^+]$ affect pH?

Answer: Increasing $[H^+]$ decreases pH. pH decreases as acidity increases.

Flashcard 56: What is the $K_b$ expression for $BOH \rightleftharpoons B^+ + OH^-$?

Answer: $K_b = \frac{[B^+][OH^-]}{[BOH]}$. Equilibrium expression for base dissociation.

Flashcard 57: Define a Brønsted-Lowry acid.

Answer: A Brønsted-Lowry acid is a proton donor. Gives up $H^+$ to another species.

Flashcard 58: Identify the pH range for basic solutions.

Answer: Basic solutions have a pH greater than 7. Higher $[OH^-]$ than $[H^+]$.

Flashcard 59: What is the $pK_b$ expression for a base?

Answer: $pK_b = -\text{log}_{10} K_b$. Negative logarithm of base dissociation constant.

Flashcard 60: How does increasing $[H^+]$ affect pH?

Answer: Increasing $[H^+]$ decreases pH. pH decreases as acidity increases.

Flashcard 61: Identify the conjugate base of $HCl$.

Answer: The conjugate base of $HCl$ is $Cl^-$. Loses a proton to form the conjugate base.

Flashcard 62: Identify the conjugate base of $HCl$.

Answer: The conjugate base of $HCl$ is $Cl^-$. Loses a proton to form the conjugate base.

Flashcard 63: Which ion is common in all basic solutions?

Answer: The common ion is $OH^-$. Present in all aqueous base solutions.

Flashcard 64: State the formula for calculating pH.

Answer: $pH = -\text{log}_{10} [H^+]$. Negative logarithm of hydrogen ion concentration.

Flashcard 65: What is the definition of a strong acid?

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

Flashcard 66: What is a Lewis acid?

Answer: A Lewis acid is an electron pair acceptor. Receives an electron pair from a donor.

Flashcard 67: What is the $pH$ of a $0.001$ M $NaOH$ solution?

Answer: $pH = 11$. Strong base: $pOH = 3$, so $pH = 14 - 3$.

Flashcard 68: What is the pH of a solution with $[H^+] = 1.0 \times 10^{-3}$ M?

Answer: $pH = 3$. Calculated using $pH = -\log[H^+]$.

Flashcard 69: What is the definition of a weak acid?

Answer: A weak acid partially ionizes in solution. Incomplete dissociation in aqueous solution.

Flashcard 70: What is the definition of a weak base?

Answer: A weak base partially dissociates in solution. Incomplete dissociation in aqueous solution.

Flashcard 71: What is the relationship between pH and pOH?

Answer: $pH + pOH = 14$ at 25°C. Based on the ion product of water.

Flashcard 72: What is the pH of a solution with $[H^+] = 1.0 \times 10^{-3}$ M?

Answer: $pH = 3$. Calculated using $pH = -\log[H^+]$.

Flashcard 73: What is the ion product constant for water ($K_w$) at 25°C?

Answer: $K_w = 1.0 \times 10^{-14}$ at 25°C. Product of $[H^+]$ and $[OH^-]$ concentrations.

Flashcard 74: What is the effect of temperature on $K_w$ of water?

Answer: $K_w$ increases with temperature. Higher temperature increases ion product.

Flashcard 75: State the formula for calculating pOH.

Answer: $pOH = -\text{log}_{10} [OH^-]$. Negative logarithm of hydroxide ion concentration.

Flashcard 76: What is the $K_b$ expression for $BOH \rightleftharpoons B^+ + OH^-$?

Answer: $K_b = \frac{[B^+][OH^-]}{[BOH]}$. Equilibrium expression for base dissociation.