Thursday, March 20, 2014

Review for Test

  1. Definitions of acids/bases.
    • Properties
    • Arrhenius defnition
    • Bronsted-Lowry definiton
      • Conjugate pairs
    • Lewis definition
  2. Acid Base Equilibria
  3. Self-Ionization of Water (Kw)
  4. pH, pOH, [H3O+], [OH-]
  5. pH scale and values
  6. Acid-Base Strength (Concentration vs. Strength)
    • Ka and Kb
  7. Polyprotic Acids
  8. Titration
  9. Buffers
  10. Important Equations:
    • Kw = [H3O+][OH-] = 1.0 x 10-14
    • pH = -log[H3O+]
    • [H3O+] = 10-pH
    • pOH = -log[OH-]
    • [OH-] = 10-pOH
    • pH + pOH = 14
    • (MK)(VK)=(MU)(VU)



  1. In the following chemical reactions, identify the acid, base, conjugate acid, and conjugate base.
    • HC2H3O2 + H2O ⇌ H3O+ + C2H3O2-
    • NH3 + H2O ⇌ NH4+ + OH-
    • HNO3 + H2O ⇌ NO3- + H3O+
  2. Find the [H3O+] and pH of the following:
    • 0.025 M HNO3
    • 3.4 x 10-4 M H2SO4
  3. Calculate the [H3O+] and pOH of the following solutions:
    • pH = 3.2
    • pH = 5.0
    • [OH-] = 8.2 x 10-9
    • pH = 12.4
  4. Find the [OH-] of the following solutions:
    • [H3O+] = 3.9 x 10-6 M
    • [H3O+] = 0.0014 M
    • pH = 4.2
  5. If 35.2 mL of 12M HCl is used to titrate 50.0 mL of KOH, what is the concentration of the KOH?
  6. What is the volume of 2.5 M NaOH needed to titrate 25.0 mL of 1.0 M HCl?
  7. Given the following equation, find the concentration of NaOH when 24.09 mL of 1.605 M H2SO4 is needed to titrate 50.0 mL of NaOH.      H2SO4 + 2NaOH ➝ Na2SO4 + 2H2O
  8. What is the salt that is formed during the following neutralization reactions?
    • Mg(OH)2 + HCl ➝ ? + H2O
    • H2SO4 + 2NH4O ➝ ? + 2H2O
    • Ni(OH)2 + 2HClO4 ➝ ? + 2H2O
    • Mg(OH)2 + H2SO4 ➝ ? + 2H2O


Answers:
  1. Identifying the acid, base, conjugate acid, and conjugate base.
    • Acid: HC2H3O2Base: H2OC. Acid: H3O+C. Base: C2H3O2-
    • Acid: H2OBase: NH3C. Acid: OH-C. Base: NH4+ 
    • Acid: HNO3Base: H2OC. Acid: H3O+C. Base: NO3- 
  2. Find the [H3O+] and pH of the following:
    • [H3O+] = 0.025 & pH = 1.6
    • [H3O+] = 6.8 x 10-4 & pH = 3.1
  3. Calculate the [H3O+] and pOH of the following solutions:
    • [H3O+] = 6.0 x 10-4 & pOH = 10.8
    • [H3O+] = 1.0 x 10-5 & pOH = 9
    • [H3O+] = 1.2 x 10-6 & pOH = 8.1
    • [H3O+] = 4.0 x 10-13 & pOH = 1.6
  4. Find the [OH-] of the following solutions:
    • [OH-] = 2.5 x 10-9
    • [OH-] = 7.1 x 10-12
    • [OH-] = 1.6 x 10-10
  5. 8.4 M KOH
  6. 10.0 mL of NaOH
  7. 1.5 M NaOH
  8. What is the salt that is formed during the following neutralization reactions?
    • MgCl2
    • (NH4)2SO4
    • Ni(ClO4)2
    • MgSO4
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