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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.

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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.

AP Chemistry Flashcards: Introduction To Acids And Bases

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QUESTION

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

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ANSWER

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

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Flashcard 1: 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^+H+ and OH−OH^-OH−.

Flashcard 2: What is a Lewis base?

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

Flashcard 3: State the formula for calculating pH.

Answer: pH=−log10[H+]pH = -\text{log}_{10} [H^+]pH=−log10​[H+]. Negative logarithm of hydrogen ion concentration.

Flashcard 4: Which ion is common in all basic solutions?

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

Flashcard 5: What is the ion product constant for water (KwK_wKw​) at 25°C?

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

Flashcard 6: Which acid is stronger: HClHClHCl or HFHFHF?

Answer: HClHClHCl is stronger than HFHFHF. HClHClHCl is a strong acid, HFHFHF is weak.

Flashcard 7: What is the effect of temperature on KwK_wKw​ of water?

Answer: KwK_wKw​ increases with temperature. Higher temperature increases ion product.

Flashcard 8: Identify the conjugate base of H2SO4H_2SO_4H2​SO4​.

Answer: The conjugate base of H2SO4H_2SO_4H2​SO4​ is HSO4−HSO_4^-HSO4−​. Loses one proton from diprotic acid.

Flashcard 9: Define a Brønsted-Lowry acid.

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

Flashcard 10: What is the KwK_wKw​ expression for water?

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

Flashcard 11: What is the pKbpK_bpKb​ expression for a base?

Answer: pKb=−log10KbpK_b = -\text{log}_{10} K_bpKb​=−log10​Kb​. Negative logarithm of base dissociation constant.

Flashcard 12: What is the pHpHpH of a 0.010.010.01 M HClHClHCl solution?

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

Flashcard 13: What is the pHpHpH of a 0.0010.0010.001 M NaOHNaOHNaOH solution?

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

Flashcard 14: What is the definition of a weak base?

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

Flashcard 15: Which ion is common in all acidic solutions?

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

Flashcard 16: What is the KaK_aKa​ expression for HA⇌H++A−HA \rightleftharpoons H^+ + A^-HA⇌H++A−?

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

Flashcard 17: Identify the conjugate base of HClHClHCl.

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

Flashcard 18: What is the pOH of a solution with [OH−]=1.0×10−4[OH^-] = 1.0 \times 10^{-4}[OH−]=1.0×10−4 M?

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

Flashcard 19: How does increasing [H+][H^+][H+] affect pH?

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

Flashcard 20: Which base is stronger: NaOHNaOHNaOH or NH3NH_3NH3​?

Answer: NaOHNaOHNaOH is stronger than NH3NH_3NH3​. NaOHNaOHNaOH is strong, NH3NH_3NH3​ is weak.

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

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

Flashcard 22: What is the pKapK_apKa​ expression for an acid?

Answer: pKa=−log10KapK_a = -\text{log}_{10} K_apKa​=−log10​Ka​. Negative logarithm of acid dissociation constant.

Flashcard 23: What is the pH of pure water at 25°C?

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

Flashcard 24: State the formula for calculating pOH.

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

Flashcard 25: What is the relationship between pH and pOH?

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

Flashcard 26: Identify the pH range for acidic solutions.

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

Flashcard 27: What is a Lewis acid?

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

Flashcard 28: What is the pH of a solution with [H+]=1.0×10−3[H^+] = 1.0 \times 10^{-3}[H+]=1.0×10−3 M?

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

Flashcard 29: What is the definition of an acid according to Arrhenius?

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

Flashcard 30: What is the definition of a strong base?

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