1.	Calcium reacts with water to form calcium hydroxide and hydrogen. In the balanced equation for this reaction, what is the coefficient of hydrogen? A. 2 B. 1 C. 4 D. 3 E. ½

2.	When aqueous solutions of barium nitrate and ammonium sulfate are mixed, what are the "spectator ions" in the reaction? A. NH4+ and NO3– B. NH4+ and SO42– C. Ba2+ and NO3– D. SO42– and NO3– E. Ba2+ and SO42–

3.	Which of the following is insoluble in water? A. Pb(ClO4)2 B. (NH4)2CO3 C. Na2SO4 D. CaCO3 E. MgCl2

4.

Consider the possible reactions below:    1. Hg2(ClO4)2(aq) + NH4I(aq) ®    2. Hg(ClO4)2(aq) + NaI(aq) ®    3. HgI2(aq) + KI(aq) ®    4. Hg2(NO3)2(aq) + KI(aq) ® Which of the possible reactions above gives the net ionic equation, Hg22+(aq) + 2I-(aq) ® Hg2I2(s)? A. 2 and 3 B. 1 and 2 C. 1 only D. 1 and 4 E. 1, 2, 3, and 4

5.	Which of the following oxides gives an acidic solution when dissolved in water? A. P4O10 B. CaO C. Na2O D. SrO E. K2O

6.	What salt is produced by the reaction between aqueous solutions of calcium hydroxide and sulfuric acid? A. CaSO4 B. CaO C. CaHSO4 D. Ca(HSO4)(OH) E. H2O

7.	What is the oxidation number of chromium in Na2CrO4? A. +6 B. +3 C. +4 D. +7 E. 0

8.	In a redox reaction, the reducing agent A. contains an element that undergoes a decrease in oxidation number. B. loses electrons and is reduced. C. gains electrons and is oxidized. D. gains electrons and is reduced. E. loses electrons and is oxidized.

9.	Charcoal "filters" are used to remove dissolved chlorine gas from drinking water. In acidic solution, Cl2(aq), reacts with carbon to form carbon dioxide and chloride ions. Which species is oxidized? A. carbon B. Cl2 C. CO2 D. H2O E. H+

10.	Ammonia gas and NO(g) react to form nitrogen gas and H2O(g). Which species is the oxidizing agent? A. NO(g) B. NH3(g) C. H2O(g) D. N2(g) E. Since this is not a redox reaction, there is no oxidizing agent.

11.	All of the following are redox reactions except A. 2KClO3(s) ® 2KCl(s) + 3O2(g) B. Zn(s) + 2HCl(aq) ® ZnCl2(aq) + H2(g) C. 2Na(s) + S(s) ® Na2S(s) D. 2Mg(s) + O2(g) ® 2MgO(s) E. NH3(g) + HCl(g) ® NH4Cl(s)

12.	Consider the following reaction:    3NO2(g) + H2O(l) ® 2HNO3(l) + NO(g) How many moles of nitric acid are produced starting from 5.00 moles of NO2(g) and excess water? A. 10.0 mol B. 0.300 mol C. 3.33 mol D. 1.67 mol E. 7.50 mol

13.	A 25.00-mL sample of HClO4(aq) was titrated to the stoichiometric point with 36.80 mL of 0.1011 M NaOH(aq). What is the molarity of the perchloric acid solution? A. 0.06868 M B. 0.06020 M C. 0.003720 M D. 0.09301 M E. 0.1488 M

14.	How many mL of 0.100 M HCl(aq) are neutralized by 1.00 g of Mg(OH)2(s)? A. 171 mL B. 5.85 mL C. 343 mL D. 85.7 mL E. 686 mL

15.	Consider the following reaction.    6Na(l) + Al2O3(s) ® 2Al(l) + 3Na2O(s) When 5.52 g of sodium react with excess Al2O3(s), 1.00 g of Al(l) is produced. What is the percent yield? A. 11.1% B. 18.1% C. 15.4% D. 39.1% E. 46.3%

16.	If 16.0 mL of 1.80 M AgNO3(aq) are added to 64.00 mL of 0.200 M HCl(aq), how many moles of AgCl(s) are produced? A. 0.0128 mol B. 1.80 mol C. 0.0256 mol D. 0.0288 mol E. 0.200 mol

17.	Calculate the molarity of a solution prepared by dissolving 20.0 g of glucose, C6H12O6, in enough water to prepare 2500 mL of solution. A. 0.278 M B. 4.44 × 10–5 M C. 0.111 M D. 1.44 M E. 0.0444 M

18.	Calculate the mass of sodium chloride required to make 75.00 mL of a 0.538 M NaCl(aq) solution. A. 8.16 g B. 2.36 g C. 23.6 g D. 6.90 g E. 0.690 g

19.	If you have a 0.500 M NaCl(aq) solution, what volume of this solution should you transfer so as to have a sample of solution that contains 0.150 mol NaCl? A. 100. mL B. 75 mL C. 30. mL D. 15 mL E. 300. mL

20.	Calculate the volume of a solution of 2.38 M glucose, C6H12O6(aq), that should be used to make 3.00 L of 0.0333 M glucose(aq). A. 238 mL B. 37.9 mL C. 99.9 mL D. 42.0 mL E. 26.4 mL

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