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AP Chemistry Flashcards: Introduction To Acids And Bases

Study Introduction To 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

Introduction To Acids And Bases

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QUESTION
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Identify the pH range for acidic solutions.

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ANSWER

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

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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.

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Flashcard 1: Identify the pH range for acidic solutions.

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

Flashcard 2: What is the pKbpK_b expression for a base?

Answer: pKb=−log10KbpK_b = -\text{log}_{10} K_b. Negative logarithm of base dissociation constant.

Flashcard 3: Identify the conjugate base of H2OH_2O.

Answer: The conjugate base of H2OH_2O is OH−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=−log10[H+]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+][H^+] than [OH−][OH^-].

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

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

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

Answer: The conjugate acid of OH−OH^- is H2OH_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−OH^-. Present in all aqueous base solutions.

Flashcard 10: What is the pHpH of a 0.0010.001 M NaOHNaOH solution?

Answer: pH=11pH = 11. Strong base: pOH=3pOH = 3, so pH=14−3pH = 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 pHpH of a 0.010.01 M HClHCl solution?

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

Flashcard 13: Identify the conjugate acid of NH3NH_3.

Answer: The conjugate acid of NH3NH_3 is NH4+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+][H^+] in aqueous solution. Releases hydrogen ions when dissolved.

Flashcard 15: What is the KaK_a expression for HA⇌H++A−HA \rightleftharpoons H^+ + A^-?

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

Flashcard 16: Which base is stronger: NaOHNaOH or NH3NH_3?

Answer: NaOHNaOH is stronger than NH3NH_3. NaOHNaOH is strong, NH3NH_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: NaOHNaOH or NH3NH_3?

Answer: NaOHNaOH is stronger than NH3NH_3. NaOHNaOH is strong, NH3NH_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+H^+ and OH−OH^-.

Flashcard 21: Identify the conjugate base of H2SO4H_2SO_4.

Answer: The conjugate base of H2SO4H_2SO_4 is HSO4−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−][OH^-] in aqueous solution. Releases hydroxide ions when dissolved.

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

Answer: Increasing [OH−][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−][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−][H^+] = [OH^-].

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

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

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

Answer: The conjugate acid of OH−OH^- is H2OH_2O. Gains a proton to form the conjugate acid.

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

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

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

Answer: KwK_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+H^+ from another species.

Flashcard 33: Define a Brønsted-Lowry base.

Answer: A Brønsted-Lowry base is a proton acceptor. Receives H+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−][OH^-] in aqueous solution. Releases hydroxide ions when dissolved.

Flashcard 37: Which acid is stronger: HClHCl or HFHF?

Answer: HClHCl is stronger than HFHF. HClHCl is a strong acid, HFHF is weak.

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

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

Flashcard 39: Which acid is stronger: HClHCl or HFHF?

Answer: HClHCl is stronger than HFHF. HClHCl is a strong acid, HFHF is weak.

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

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

Flashcard 41: What is the pKapK_a expression for an acid?

Answer: pKa=−log10KapK_a = -\text{log}_{10} K_a. Negative logarithm of acid dissociation constant.

Flashcard 42: What is the KwK_w expression for water?

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

Flashcard 43: What is the KwK_w expression for water?

Answer: Kw=[H+][OH−]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+H^+. Present in all aqueous acid solutions.

Flashcard 45: Identify the conjugate base of H2SO4H_2SO_4.

Answer: The conjugate base of H2SO4H_2SO_4 is HSO4−HSO_4^-. Loses one proton from diprotic acid.

Flashcard 46: Identify the conjugate acid of NH3NH_3.

Answer: The conjugate acid of NH3NH_3 is NH4+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−][OH^-] than [H+][H^+].

Flashcard 48: Define a Brønsted-Lowry acid.

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

Flashcard 49: What is the pHpH of a 0.010.01 M HClHCl solution?

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

Flashcard 50: What is the pKapK_a expression for an acid?

Answer: pKa=−log10KapK_a = -\text{log}_{10} K_a. Negative logarithm of acid dissociation constant.

Flashcard 51: Identify the conjugate base of H2OH_2O.

Answer: The conjugate base of H2OH_2O is OH−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+][H^+] in aqueous solution. Releases hydrogen ions when dissolved.

Flashcard 53: What is the KaK_a expression for HA⇌H++A−HA \rightleftharpoons H^+ + A^-?

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

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

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

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

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

Flashcard 56: What is the KbK_b expression for BOH⇌B++OH−BOH \rightleftharpoons B^+ + OH^-?

Answer: Kb=[B+][OH−][BOH]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+H^+ to another species.

Flashcard 58: Identify the pH range for basic solutions.

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

Flashcard 59: What is the pKbpK_b expression for a base?

Answer: pKb=−log10KbpK_b = -\text{log}_{10} K_b. Negative logarithm of base dissociation constant.

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

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

Flashcard 61: Identify the conjugate base of HClHCl.

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

Flashcard 62: Identify the conjugate base of HClHCl.

Answer: The conjugate base of HClHCl is Cl−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−OH^-. Present in all aqueous base solutions.

Flashcard 64: State the formula for calculating pH.

Answer: pH=−log10[H+]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 pHpH of a 0.0010.001 M NaOHNaOH solution?

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

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

Answer: pH=3pH = 3. Calculated using pH=−log⁡[H+]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=14pH + pOH = 14 at 25°C. Based on the ion product of water.

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

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

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

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

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

Answer: KwK_w increases with temperature. Higher temperature increases ion product.

Flashcard 75: State the formula for calculating pOH.

Answer: pOH=−log10[OH−]pOH = -\text{log}_{10} [OH^-]. Negative logarithm of hydroxide ion concentration.

Flashcard 76: What is the KbK_b expression for BOH⇌B++OH−BOH \rightleftharpoons B^+ + OH^-?

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