Choose the correct answer for each question.

1. Determine the Molar Mass for: barium arsenate

   1.   ?    689.74 ^g / _mol
   2.   ?    276.22 ^g / _mol
   3.   ?    547.36 ^g / _mol
   4.   ?    177.25 ^g / _mol

2. Determine the Number of Moles for: 2.30 kg of aluminum oxide

   1.   ?    2.3 x 10² mol aluminum oxide
   2.   ?    102 mol aluminum oxide
   3.   ?    2.2 x 10^-2 mol aluminum oxide
   4.   ?    22.56 mol aluminum oxide

3. Determine the Number of Moles for: 845.0 grams of NaC₃H₅O₃

   1.   ?    9.45 x 10⁴ mol NaC₃H₅O₃
   2.   ?    112.0 mol NaC₃H₅O₃
   3.   ?    7.55 mol NaC₃H₅O₃
   4.   ?    0.133 mol NaC₃H₅O₃

4. Determine the Number of Moles for: 7.50 g of calcium carbonate

   1.   ?    100 mol calcium carbonate
   2.   ?    13.3 mol calcium carbonate
   3.   ?    7.50 x 10^-2 mol calcium carbonate
   4.   ?    751 mol calcium carbonate

5. Determine the Molar Mass for: ammonium phosphate

   1.   ?    45.97 ^g / _mol
   2.   ?    109.97 ^g / _mol
   3.   ?    148.97 ^g / _mol
   4.   ?    299.91 ^g / _mol

6. Determine the Molar Mass for: copper(II)sulfate

   1.   ?    95.61 ^g / _mol
   2.   ?    159.61 ^g / _mol
   3.   ?    223.16 ^g / _mol
   4.   ?    143.61 ^g / _mol

7. Determine the Number of Grams needed to prepare 10.0 liters of a 1.0 M sulfuric acid, H₂SO₄, solution.

   1.   ?    9.81 grams of H₂SO₄
   2.   ?    98.1 grams of H₂SO₄
   3.   ?    981 grams of H₂SO₄
   4.   ?    9810 grams of H₂SO₄

8. Determine the Percent Composition of oxygen in calcium phosphate.

   1.   ?    47.4 % oxygen
   2.   ?    52.6 % oxygen
   3.   ?    41.3 % oxygen
   4.   ?    58.7 % oxygen

9. Determine the Number of Grams needed to prepare 3 liters of a 2.0 M hypochlorous acid, HClO, solution. (Cl = chlorine, this test program does not differentiate between lower-case "L" and "I")

   1.   ?    315 grams of hypochlorous acid
   2.   ?    52.4 grams of hypochlorous acid
   3.   ?    0.114 grams of hypochlorous acid
   4.   ?    78.7 grams of hypochlorous acid

10. Determine the Molar Mass for: diphosphorus pentoxide

    1.   ?    46.97 ^g / _mol
    2.   ?    110.97 ^g / _mol
    3.   ?    93.94 ^g / _mol
    4.   ?    141.94 ^g / _mol

11. Determine the Percent Composition of aluminum in aluminum oxide.

    1.   ?    52.9 % aluminum
    2.   ?    47.1 % aluminum
    3.   ?    0.053 % aluminum
    4.   ?    54.0 % aluminum

12. Determine the Molarity of a potassium chloride solution where 25.0 g is dissolved in enough solvent so that the final volume is 0.50 L.

    1.   ?    5.96 M potassium chloride solution
    2.   ?    0.671 M potassium chloride solution
    3.   ?    0.335 M potassium chloride solution
    4.   ?    1.07 x 10^-3 M potassium chloride solution

13. Determine the Number of Moles dissolved in 4.0 L of 3.0 M sodium chloride solution.

    1.   ?    77.7 moles of sodium chloride
    2.   ?    701 moles of sodium chloride
    3.   ?    12 moles of sodium chloride
    4.   ?    1.33 moles of sodium chloride

14. Determine the Percent Composition of oxygen in cobalt(II) iodate.

    1.   ?    14.5 % oxygen
    2.   ?    0.024 % oxygen
    3.   ?    23.6 % oxygen
    4.   ?    62.0 % oxygen

15. Determine the Number of Moles for: 1.50 kg of sulfuric acid, H₂SO₄

    1.   ?    15.3 mol H₂SO₄
    2.   ?    1.52 x 10^-2 mol H₂SO₄
    3.   ?    147 mol H₂SO₄
    4.   ?    98.1 mol H₂SO₄

16. Determine the Molarity of a lead(II) nitrate solution where 550 grams is dissolved in enough solvent so that the final volume is 900.0 mL.

    1.   ?    1.66 M lead(II) nitrate solution
    2.   ?    0.542 M lead(II) nitrate solution
    3.   ?    0.602 M lead(II) nitrate solution
    4.   ?    1.84 M lead(II) nitrate solution

17. Determine the Number of Moles for: 45.0 grams of magnesium hydroxide

    1.   ?    58.3 mol magnesium hydroxide
    2.   ?    0.77 mol magnesium hydroxide
    3.   ?    1.09 mol magnesium hydroxide
    4.   ?    2620 mol magnesium hydroxide

18. Determine the Number of Moles dissolved in 4.50 liters of 2.0 M CaCl₂ solution.

    1.   ?    999 moles of CaCl₂
    2.   ?    8.11 x 10^-2 moles of CaCl₂
    3.   ?    9.0 moles of CaCl₂
    4.   ?    2.3 moles of CaCl₂

19. Determine the Number of Moles for: 5.20 kilograms of sodium hydroxide

    1.   ?    2.08 x 10^-1 mol sodium hydroxide
    2.   ?    2.08 x 10⁵ mol sodium hydroxide
    3.   ?    40.0 mol sodium hydroxide
    4.   ?    208 mol sodium hydroxide

20. Determine the Molar Mass for: lead(IV) chromate

    1.   ?    1135.2 ^g / _mol
    2.   ?    439.2 ^g / _mol
    3.   ?    323.2 ^g / _mol
    4.   ?    880.8 ^g / _mol

21. Determine the Molar Mass for: silver nitrate

    1.   ?    137.9 ^g / _mol
    2.   ?    277.8 ^g / _mol
    3.   ?    169.9 ^g / _mol
    4.   ?    259.0 ^g / _mol

22. Determine the Molar Mass for: iron(III) oxide

    1.   ?    159.7 ^g / _mol
    2.   ?    183.55 ^g / _mol
    3.   ?    199.55 ^g / _mol
    4.   ?    71.85 ^g / _mol

23. Determine the Number of Moles for: 7.50 kilograms of silicon dioxide

    1.   ?    0.125 mol silicon dioxide
    2.   ?    0.451 mol silicon dioxide
    3.   ?    60.1 mol silicon dioxide
    4.   ?    125 mol silicon dioxide

24. Determine the Number of Moles for: 0.0500 grams of potassium permanganate

    1.   ?    3.16 x 10^-1 mol potassium permanganate
    2.   ?    3.16 x 10^-4 mol potassium permanganate
    3.   ?    7.14 x 10^-4 mol potassium permanganate
    4.   ?    158 mol potassium permanganate

25. Determine the Molar Mass for: carbon tetrachloride

    1.   ?    153.8 ^g / _mol
    2.   ?    47.45 ^g / _mol
    3.   ?    189.25 ^g / _mol
    4.   ?    82.9 ^g / _mol

26. Determine the Number of Moles dissolved in 10.0 L of 5.0 M HCl solution.

    1.   ?    1.82 x 10³ moles of HCl
    2.   ?    50 moles of HCl
    3.   ?    2.0 moles of HCl
    4.   ?    1.37 moles of HCl

27. Determine the Number of Grams needed to prepare 2500 milliliters of a 3.5 M phosphoric acid, H₃PO₄, solution.

    1.   ?    8.57 x 10⁵ grams of H₃PO₄
    2.   ?    857 grams of H₃PO₄
    3.   ?    98.0 grams of H₃PO₄
    4.   ?    8.93 x 10^-2 grams of H₃PO₄

28. Determine the Number of Moles dissolved in 100.0 mL of 7.0 M nitric acid, HNO₃, solution.

    1.   ?    1.1 x 10^-2 moles of HNO₃
    2.   ?    44.1 moles of HNO₃
    3.   ?    700 moles of HNO₃
    4.   ?    0.7 moles of HNO₃

29. Determine the Molarity of a copper(II) sulfate solution where 0.075 kg is dissolved in enough solvent so that the final volume is 300.0 mL.

    1.   ?    1.57 x 10^-2 M copper(II) sulfate solution
    2.   ?    39.9 M copper(II) sulfate solution
    3.   ?    0.47 M copper(II) sulfate solution
    4.   ?    1.57 M copper(II) sulfate solution

30. Determine the Molar Mass for: aluminum sulfite

    1.   ?    59.04 ^g / _mol
    2.   ?    150.14 ^g / _mol
    3.   ?    246.14 ^g / _mol
    4.   ?    294.14 ^g / _mol

31. Determine the Percent Composition of hydrogen in ammonium phosphate.

    1.   ?    0.0805 % hydrogen
    2.   ?    8.06 % hydrogen
    3.   ?    3.54 % hydrogen
    4.   ?    0.0354 % hydrogen

32. Determine the Number of Grams needed to prepare 600 milliliters of a 2.0 M Pb(NO₃)₂ solution.

    1.   ?    331.2 grams of Pb(NO₃)₂
    2.   ?    3.97 x 10⁵ grams of Pb(NO₃)₂
    3.   ?    397.4 grams of Pb(NO₃)₂
    4.   ?    3.62 x 10^-3 grams of Pb(NO₃)₂

33. Determine the Number of Moles dissolved in 450 milliliters of 3.5 M CuSO₄ solution.

    1.   ?    2.86 x 10⁷ moles of CuSO₄
    2.   ?    129 moles of CuSO₄
    3.   ?    251 moles of CuSO₄
    4.   ?    1.58 moles of CuSO₄

34. Determine the Molarity of a nickel(II) sulfate solution where 56.70 grams is dissolved in enough solvent so that the final volume is 5.0 liters.

    1.   ?    7.32 x 10^-2 M nickel(II) sulfate solution
    2.   ?    31.0 M nickel(II) sulfate solution
    3.   ?    1.25 x 10^-1 M nickel(II) sulfate solution
    4.   ?    5.46 x 10^-1 M nickel(II) sulfate solution

35. Determine the Percent Composition of iron in iron(III) oxide.

    1.   ?    65.0 % of iron
    2.   ?    16.0 % of iron
    3.   ?    84.0 % of iron
    4.   ?    35.0 % of iron

36. Determine the Number of Grams needed to prepare 1000 mL of a 0.5 M MgCl₂ solution.

    1.   ?    381 grams of MgCl₂
    2.   ?    190 grams of MgCl₂
    3.   ?    95.2 grams of MgCl₂
    4.   ?    47.6 grams of MgCl₂

37. Determine the Number of Moles for: 1.50 kilograms of potassium chloride

    1.   ?    20.1 mol potassium chloride
    2.   ?    2.01 x 10^-2 mol potassium chloride
    3.   ?    49.7 mol potassium chloride
    4.   ?    74.6 mol potassium chloride

38. Determine the Molar Mass for: calcium citrate

    1.   ?    229.08 ^g / _mol
    2.   ?    647.16 ^g / _mol
    3.   ?    309.24 ^g / _mol
    4.   ?    498.24 ^g / _mol

39. Determine the Molarity of a sodium hydroxide solution where 3.5 kg is dissolved in enough solvent so that the final volume is 30 liters.

    1.   ?    87.5 M sodium hydroxide solution
    2.   ?    2.92 M sodium hydroxide
    3.   ?    2.92 x 10^-3 M sodium hydroxide
    4.   ?    2.92 x 10^-6 M sodium hydroxide

40. Determine the Number of Moles for: 92.5 g of magnesium hydroxide

    1.   ?    1.59 mol magnesium hydroxide
    2.   ?    2.24 mol magnesium hydroxide
    3.   ?    0.630 mol magnesium hydroxide
    4.   ?    5390 mol magnesium hydroxide