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 conjugate base of $H_2O$.

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

Flashcard 2: What is a Lewis acid?

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

Flashcard 3: State the formula for calculating pH.

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

Flashcard 4: Identify the pH range for acidic solutions.

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

Flashcard 5: Identify the conjugate acid of $OH^-$.

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

Flashcard 6: What is the $pH$ of a $0.001$ M $NaOH$ solution?

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

Flashcard 7: What is the definition of a strong acid?

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

Flashcard 8: 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 9: Which base is stronger: $NaOH$ or $NH_3$?

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

Flashcard 10: 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 11: 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 12: What is the definition of a base according to Arrhenius?

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

Flashcard 13: What is the pH of pure water at 25°C?

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

Flashcard 14: 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 15: What is a Lewis base?

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

Flashcard 16: Define a Brønsted-Lowry base.

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

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

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

Flashcard 18: What is the definition of a strong base?

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

Flashcard 19: What is the pOH of a solution with $[OH^-] = 1.0 \times 10^{-4}$ M?

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

Flashcard 20: Which acid is stronger: $HCl$ or $HF$?

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

Flashcard 21: How does increasing $[OH^-]$ affect pOH?

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

Flashcard 22: What is the $K_w$ expression for water?

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

Flashcard 23: Which ion is common in all acidic solutions?

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

Flashcard 24: Identify the pH range for basic solutions.

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

Flashcard 25: Define a Brønsted-Lowry acid.

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

Flashcard 26: What is the $pH$ of a $0.01$ M $HCl$ solution?

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

Flashcard 27: What is the $pK_a$ expression for an acid?

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

Flashcard 28: What is the definition of an acid according to Arrhenius?

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

Flashcard 29: What is the $K_a$ expression for $HA \rightleftharpoons H^+ + A^-$?

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

Flashcard 30: What is the $pK_b$ expression for a base?

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

Flashcard 31: How does increasing $[H^+]$ affect pH?

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

Flashcard 32: Identify the conjugate base of $HCl$.

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

Flashcard 33: Which ion is common in all basic solutions?

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

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

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

Flashcard 35: What is the relationship between pH and pOH?

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

Flashcard 36: What is the pH of a solution with $[H^+] = 1.0 \times 10^{-3}$ M?

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

Flashcard 37: What is the effect of temperature on $K_w$ of water?

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

Flashcard 38: State the formula for calculating pOH.

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

Flashcard 39: What is the $K_b$ expression for $BOH \rightleftharpoons B^+ + OH^-$?

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