AP Chemistry Flashcards: Acid Base Titrations

What this deck covers

This deck focuses on Acid Base Titrations, 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: Calculate the pH of a 0.01 M HCl solution.

Answer: pH = 2. Strong acid: pH = $-\log(0.01) = -\log(10^{-2}) = 2$.

Flashcard 2: Which option best describes a titration curve?

Answer: Graph of pH versus volume of titrant added. Visual representation showing pH changes during titration process.

Flashcard 3: What is the purpose of a titration in acid-base chemistry?

Answer: To determine the concentration of an unknown solution. Uses known titrant to find unknown concentration via stoichiometry.

Flashcard 4: State the formula for calculating molarity.

Answer: $M = \frac{\text{moles of solute}}{\text{liters of solution}}$. Defines concentration as moles of solute per liter of solution.

Flashcard 5: What is the equivalence point in a titration curve?

Answer: Where moles of acid equal moles of base. Stoichiometric neutralization point on titration curve.

Flashcard 6: What is the pH at the equivalence point for a strong acid-strong base titration?

Answer: pH = 7. Equal amounts of strong acid and base neutralize to neutral pH.

Flashcard 7: Which option describes a buffer solution?

Answer: Resists changes in pH upon addition of acid or base. Contains conjugate acid-base pair to maintain pH stability.

Flashcard 8: What is the effect of dilution on the pH of a strong acid?

Answer: Increases the pH. Dilution decreases $[H^+]$, raising pH toward neutral.

Flashcard 9: Choose the correct pH range for phenolphthalein.

Answer: 8.2 to 10.0. Indicator's transition range for color change.

Flashcard 10: Which acid-base pair has a higher pH at the equivalence point: strong acid-weak base or weak acid-strong base?

Answer: Weak acid-strong base. Weak acid-strong base gives basic equivalence point (pH > 7).

Flashcard 11: Calculate the volume of 0.1 M NaOH needed to neutralize 50 mL of 0.1 M HCl.

Answer: 50 mL. Equal molarity and volume means 1:1 mole ratio requires equal volume.

Flashcard 12: In a titration, what is the titrant?

Answer: The solution added from the burette. Standard solution delivered from burette during analysis.

Flashcard 13: What is the definition of a titrant?

Answer: A solution of known concentration used in titration. Standard solution added from burette to determine analyte concentration.

Flashcard 14: Calculate the moles of HCl in 25 mL of 0.1 M solution.

Answer: 0.0025 moles. Convert volume to L (0.025 L), multiply by molarity (0.1 M).

Flashcard 15: Find and correct the error: 'The equivalence point is always at pH 7.'

Answer: Not always; depends on the strength of acid and base. Only true for strong acid-strong base; weak acids/bases differ.

Flashcard 16: State the formula for converting pH to hydrogen ion concentration.

Answer: $[\text{H}^+] = 10^{-\text{pH}}$. Inverse relationship: pH is negative log of $[H^+]$

Flashcard 17: Which indicator is commonly used for strong acid-strong base titrations?

Answer: Phenolphthalein. Changes color at pH 8.2-10, ideal for strong acid-base endpoints.

Flashcard 18: Identify the endpoint in a titration.

Answer: The point at which the indicator changes color. Visual signal used to determine when to stop adding titrant.

Flashcard 19: What is the role of a burette in a titration?

Answer: To deliver a precise volume of titrant. Graduated tube allows controlled addition and volume measurement.

Flashcard 20: What is the endpoint of a titration?

Answer: The point where the indicator changes color. Observable color change indicating approximate equivalence point.

Flashcard 21: What is the relationship between $K_a$, the acid dissociation constant, and acid strength?

Answer: Higher $K_a$ indicates a stronger acid. Larger $K_a$ means greater ionization and stronger acid.

Flashcard 22: Find the pH of a solution with $[\text{OH}^-] = 10^{-3}$ M.

Answer: pH = 11. pOH = $-\log(10^{-3}) = 3$, so pH = $14 - 3 = 11$.

Flashcard 23: Which equation relates pH and pOH?

Answer: $\text{pH} + \text{pOH} = 14$. Fundamental relationship for aqueous solutions at 25°C.

Flashcard 24: What happens to pH when a strong acid is added to a buffer?

Answer: Slight decrease in pH. Buffer components consume added acid, minimizing pH change.

Flashcard 25: Identify the formula to convert pOH to hydroxide ion concentration.

Answer: $[\text{OH}^{-}] = 10^{-\text{pOH}}$. Inverse relationship: pOH is negative log of $[OH^-]$.

Flashcard 26: Identify the primary purpose of an indicator in a titration.

Answer: To signal the endpoint of the titration. Color change marks approximate equivalence point.

Flashcard 27: Determine the pH of a solution with $[\text{H}^+] = 10^{-6}$ M.

Answer: pH = 6. pH is defined as $-\log[H^+] = -\log(10^{-6}) = 6$.

Flashcard 28: What type of reaction occurs during a titration?

Answer: Neutralization. Acid and base react to form salt and water.

Flashcard 29: Calculate the pOH of a 0.01 M NaOH solution.

Answer: pOH = 2. Strong base: pOH = $-\log(0.01) = 2$.

Flashcard 30: What is the role of a pipette in a titration?

Answer: To measure and transfer a specific volume of solution. Precision instrument for accurate volume transfer.