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 K_a)
8. A 0.15 M weak base solution with a percent ionization of 0.17% (bonus challenge: calculate K_b)

Part 2: Understanding the pH scale and K_w

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?

CH302 · 50520 Principles of Chemistry II

Spring 2023 · © mccord