• 1) Determine the molarity of a solution formed by dissolving 468 mg Of M812 in enough water to yield 50.0 mL
    • A) 0.0297 M
    • B) 0.0337 M
    • C) 0.0936 M
    • D) 0.0107 M
    • E) 0.0651 M
  • 2) Identify acetic acid.
  • A) strong electrolyte, weak acid
  • B) weak electrolyte, weak acid
  • C) strong electrolyte, strong acid
  • D) weak electrolyte, strong acid

  • E) nonelectrolyte

  • 3) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of HOSOA and KOH are mixed.
    • A) H+(aq) + oH-(aq) -> H2O(l)
    • B) 2 K+(aq) + SO4^2-(aq) -> K2SO4(s)
    • C) H+(aq) + OH-(aq) + 2 K+(aq) + SO4^2-(aq) -> H2O(l) + K2SO4(S)
    • D) H2^2+(aq) + OH-(ao) -> H2(0H)2(l)
    • E) No reaction occurs.
  • 4) Pure acetic acid (CH3COOH) is a liquid and is known as glacial acetic acid. Calculate the molarity of a solution prepared by dissolving 15.00 mL of glacial acetic acid at 25°C in sufficient water to give 500.0 n1L of solution. The density of glacial acetic acid at 25°C is 1.05 g/mL.
    • A) 1.89 * 10^3 M
    • B) 31.5 M
    • C) 0.0315 M
    • D) 0.525 M
    • E) 5.25 * 10^-4M
  • 5) When 7.80 mL of 0.500 M AgNO3 is added to 6.25 mL of 0.300 M NH4Cl, how many grams of AgCl are formed?
    • AgN03(aq) + NH4Cl(aq) -> AgCl(s) + NH4NO3(aq)
    • A) 0.269 g
    • B) 0.553 g
    • C) 0.822 g
    • D) 1.61 g
  • 6) Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution?
    • A) CH3COOH
    • B) HF
    • C) HCl
    • D) H2SO4
    • E) H2CO3
  • 7) Determine the concentration of a solution prepared by diluting 20.0 mL of a 0.200 M KCl to 250.0 mL.
    • A) 0.l60 M
    • B) 0.0320 M
    • C) 2.50 M
    • D) 0.00800 M
    • E) 0.0160 M
  • 8) What mass (in g) of AgCl is formed from the reaction of 75.0 mL of a 0.078 M AgC2H302 solution with 55.0 mL of 0.109 M MgCl2 solution?
    • 2 AgC2H3O2(aq) + MgCl2(aq) -> 2 AgCl(S) + Mg(C2H3O2)2(aq)
    • A) 0.838 g
    • B) 1.72 g
    • C) 0.859 g
    • D) 2.56 g
    • E) 1.70 g
  • 9) Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of K2S and Fe(NO3)2 are mixed.
    • A) K+(aq) + N03-(aq) -> KNO3(s)
    • B) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 N03-(aq) -> FeS(s) + 2 K+(aq) + 2 NO3-(aq)
    • C) Fe2+(aq) + S2-(aq) + 2 K+(aq) + 2 N03-(aq) -> Fe2+(aq) + S2-(aq) + 2 KNO3(s)
    • D) Fe2+(aq) + S2-(aq) -> FeS(s)
    • E) No reaction occurs
  • 10) All of the following compounds are soluble except
    • A) Ba(OH)2
    • B) Pb(NO3)2
    • C) ZnCl2
    • D) AgBr
    • E) Cu(C2H3O2)2
  • 11) Two samples of potassium iodide are decomposed into their constituent elements. The first sample produced 13.0 g of potassium and 42.3 g of iodine. If the second sample produced 24.4 kg of potassium, how many kg of iodine were produced?
    • A) 13.3 kg
    • B) 22.5 kg
    • C) 79.4 kg
    • D) 44.4 kg
    • E) 92.4 kg
  • 12 Determine the number of grams H2 formed when 250.0 mL of 0.743 M HCl solution reacts with 3.41 * 10^23 atoms of Fe according to the following reaction
    • 2HCl(aq) + Fe(s) -> H2(g) + FeCl2(aq)
    • A) 0.374g
    • B) 1.33g
    • C) 1.l4g
    • D) 0.l87g
    • E) l.5l g