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Acid-Base Titration Problem Solutions

May 6, 2025

Solving Acid-Base Titration Problems

Problem 1: Concentration of HCl Solution

  • Given:
    • 24.7 mL of HCl solution
    • Neutralized by 35.8 mL of 0.25 M NaOH solution
  • Objective: Find concentration of the original HCl solution.
  • Method 1: Using Equation
    • Equation: (M_1V_1 = M_2V_2)
    • Reason: Multiplying molarity by volume gives moles, and in neutralization, moles of acid = moles of base.
    • Calculation:
      • (M_1 = \frac{0.25 \times 35.8}{24.7})
      • Result: (M_1 = 0.362 \text{ M})
  • Method 2: Using Dimensional Analysis
    • Balanced Equation: HCl + NaOH → H2O + NaCl
    • Steps:
      1. Find moles of NaOH using molarity-volume multiplication.
      2. Convert moles of NaOH to moles of HCl (1:1 ratio).
      3. Divide moles of HCl by liters to find molarity.
    • Result: (0.362 \text{ M})

Problem 2: Volume of Barium Hydroxide Solution

  • Given:
    • 0.15 M Barium Hydroxide required to neutralize 45 mL of 0.29 M HNO3
  • Objective: Find volume of Barium Hydroxide solution needed.
  • Method 1: Using Equation
    • Equation: (M_1V_1 = 2M_2V_2) (due to two hydroxides in Ba(OH)2)
    • Calculation:
      • (0.29 \times 45 = 2 \times 0.15 \times V_2)
      • (V_2 = \frac{13.05}{0.3} = 43.5 \text{ mL})
  • Method 2: Using Stoichiometry
    • Balanced Equation: Ba(OH)2 + 2 HNO3 → 2 H2O + Ba(NO3)2
    • Steps:
      1. Calculate moles of HNO3.
      2. Use 2:1 ratio to find moles of Ba(OH)2.
      3. Convert moles to volume using molarity.
    • Result: 43.5 mL

Problem 3: Mass of KHP Neutralized by NaOH

  • Given:
    • 32.57 mL of 0.175 M NaOH
  • Objective: Find mass of KHP neutralized.
  • Method: Stoichiometry
    • Balanced Equation: KHP + NaOH → H2O + NaKP
    • Steps:
      1. Convert volume of NaOH to moles.
      2. Use 1:1 ratio to find moles of KHP.
      3. Convert moles of KHP to grams using molar mass (204.22 g/mol).
    • Result: 1.164 grams of KHP

Problem 4: Concentration of KOH Solution

  • Given:
    • 42.6 mL of KOH for titration
    • 0.137 grams of KHP
  • Objective: Find concentration of KOH.
  • Method: Stoichiometry
    • Balanced Equation: KHP + KOH → H2O + K2P
    • Steps:
      1. Convert mass of KHP to moles.
      2. Use 1:1 ratio to find moles of KOH.
      3. Divide moles by volume of KOH solution (in liters).
    • Result: 0.01 M

These problems illustrate fundamental concepts in acid-base titration, emphasizing the importance of understanding molarity, volume, and stoichiometry to solve for unknowns in chemical reactions.

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