Tuesday, May 20, 2014

Practice for Final Exam

  1. 9.35g of Al2O3 contains how many molecules?
  2. 0.253 moles of BN has a mass of…
  3. Calculate the number of moles of 8.46 x 1024 atoms of F.
  4. Calculate the number of moles of 4.35g of Cs2CO3.
  5. 0.692moles of CsH contains how many molecules?
  6. How many moles are in 14.49 g of CoSO4.
  7. What is the mass of 7.20 x 1023 atoms of Ne?
  8. 50.82 g of Cr2O3 has how many moles?
  9. 2.84 moles of N2H4 has how many molecules?
  10. 5.29 x 1024 molecules of HCl has a mass of…
  11. In a 30.0 g sample of Pb(NO3)2, Pb has a mass of 2.535 g, N a mass of 8.694 g, and O a mass of 18.768 g. What is the % composition?
  12. In a 25.0 g sample of Hg2Cl2, Hg has a mass of 3.755 g and Cl has a mass of 21.245 g. What is the % composition.
  13. In a 20.0 g sample of Ni(NO3)2, Ni has a mass of 3.066 g, Ni has a mass of 6.426 g, and O has a mass of 10.508 g. What is the % composition?
  14. What is the % composition of the following:
    • KMnO4
    • Sc2O3
    • H2SeO4
    • Cl3HSi
    • NaBrO
  15. What volume of 0.075 M HCl is required to neutralize 100 mL of 0.01 M NaOH solution?
  16. What is the concentration of NaOH if 45.2 mL of 1.5 M H2SO4 is needed to neutralize 20.0 mL of NaOH: H2SO4 + 2NaOH ➝ Na2SO4 + 2H2O?
  17. Find the [H3O+] and pH of the following: 0.075 M HCl 
  18. Find the [H3O+] and pH of the following: 0.122 M H2SO4
  19. Calculate the [H3O+] and pOH of the following solution: pH = 9.5
  20. Calculate the [H3O+] and pOH of the following solution: [OH-] = 3.9 x 10-12
  21. Find the [OH-] of the following solutions: pOH = 1.5, pH = 4.6, & [H3O+] = 2.5 x 10-9
  22. 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+
  23. Find the [H3O+] and pH of the following:
    • 0.025 M HNO3
    • 3.4 x 10-4 M H2SO4
  24. Calculate the [H3O+] and pOH of the following solutions:
    • pH = 3.2
    • pH = 5.0
    • [OH-] = 8.2 x 10-9
    • pH = 12.4
  25. Find the [OH-] of the following solutions:
    • [H3O+] = 3.9 x 10-6 M
    • [H3O+] = 0.0014 M
    • pH = 4.2
  26. If 35.2 mL of 12M HCl is used to titrate 50.0 mL of KOH, what is the concentration of the KOH?
  27. What is the volume of 2.5 M NaOH needed to titrate 25.0 mL of 1.0 M HCl?
  28. 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
  29. 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
  30. Balance the following redox reactions:
    • Na + H2O → NaOH + H2
    • HCl + HNO3 → HOCl + NO + H2O (*Cl on the product side has an oxidation number of +1)
    • SnCl4 + Fe → SnCl2 + FeCl3
    • CO + I2O5 → I2 + CO2
    • MnO4- + Fe2+ + H+ → Fe3+ + Mn2+ + H2O
    • Cu+ + Fe → Fe3+ + Cu
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