Part 1: Calculating pH

Calculate the pH for each of the following solutions.

  1. 0.00867 M HClO4
  2. 0.152 M HI
  3. 0.00772 M Ba(OH)2
  4. 0.000331 M LiOH
  5. 1.54 g HNO3 dissolved in 431 mL
  6. 3.61 g Sr(OH)2 dissolved in 1.75 gallons
  7. A 0.15 M weak acid solution with a percent ionization of 0.17% (bonus challenge: calculate Ka)
  8. A 0.15 M weak base solution with a percent ionization of 0.17% (bonus challenge: calculate Kb)

Part 2: Understanding the pH scale and Kw

  1. What is the [H+] concentration if [OH] = 3.76 × 10-4? Is this an acidic or basic solution?
  2. What is the [H+] in a 0.00012 M NaOH solution?
  3. What is the pH when [OH] = 1.9 × 10-3?

Part 3: Neutralization Reactions

  1. What volume of 0.81 M Ba(OH)2 is needed to neutralize 1.78 L 0.052 M CH3COOH solution?
  2. A titration experiment is performed where 1.00 M NaOH is added dropwise to a 50 mL unknown weak acid solution. It takes exactly 12 mL of the NaOH solution to neutralize the weak acid solution.
    1. How many moles of weak acid are in the solution
    2. What is the concentration of the weak acid solution?
  3. Determine the relative pH (acidic, basic, or neutral) of the following salts:
    1. LiCH3COO
    2. NaI
    3. NH4ClO4

Last challenge question: The Dead Sea has a pH equal to about 5.8 and a volume of 3.01 × 1013 gallons. About many moles of H+ are in the Dead Sea?








CH302N · 50600 Chemistry In Our World II


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