STANDARDIZED TEST PREPARATION

Multiple Choice

Choose the best answer.

Question 1

1. What is a correct interpretation of the following chemical equation?

K2CO3(aq) + Mg(NO3)2(aq) → 2KNO3(aq) + MgCO3(s)

  1. A solution of potassium nitrate is added to solid magnesium carbonate to produce a solution of potassium carbonate and magnesium nitrate.

  2. Solutions of potassium carbonate, magnesium nitrate, and potassium nitrate are mixed to produce solid magnesium carbonate.

  3. A solution of potassium carbonate is added to a solution of magnesium nitrate to produce a solution of potassium nitrate and solid magnesium carbonate.

  4. Solid magnesium carbonate dissolves in potassium nitrate to form a solution of potassium carbonate and magnesium nitrate.

Question 2

2. What information can be obtained from a written chemical equation?

  1. the color change of the reactant

  2. the speed of the overall reaction

  3. the states of the products

  4. the probability of an explosion

Question 3

3. For the following equation, what would you expect to observe when this reaction is performed in the laboratory?

Na2CO3(aq) + 2HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l)

  1. The resulting solution contains bubbles.

  2. The resulting solution freezes.

  3. The resulting solution changes color.

  4. The resulting solution contains white crystals.

Question 4

4. Which of the following balanced chemical equations represents a physical change?

  1. 2H2(g) + O2(g) → 2H2O(g)

  2. N2(l) → N2(g)

  3. 2KClO3(s) → 2KCl(s) + 3O2(g)

  4. Zn(s) + 2HCl(aq) → ZnCl2(aq) + H2(g)

479

Question 5

5. Which of the following correctly matches a balanced chemical reaction to its type of reaction?

  1. single exchange:

  2. NaCl(aq) + AgNO3(aq) → NaNO3(aq) + AgCl(aq)

  3. double exchange: 2AlBr3(aq) + 3Cl2(g) →

  4. 2AlCl3(aq) + 3Br2(g)

  5. decomposition: Na2CO3(s) → Na2O(s) + CO2(g)

  6. combination: 2PbSe(s) + O2(g) → 2PbO(s) + 2Se(s)

Question 6

6. The LD50 for lead toxicity is 450 mg/kg. How many milligrams would be a lethal dose for a 132 lb adult?

  1. 0.13 mg

  2. 50 mg

  3. 27 g

  4. 59 g

Question 7

7. Which of the following correctly describes the comparison of one mole of copper, Cu, magnesium, Mg, and neon, Ne?

  1. Each mole sample has the same mass.

  2. Each mole sample has the same number of atoms.

  3. Each mole sample has the same molar mass.

  4. Each mole sample has a different number of atoms based on the atomic mass.

Question 8

8. Which correctly describes a 500 mL bottle filled completely with water?

  1. There are 9000 mol of water in this bottle.

  2. There are 1.67 × 1025 molecules of water in this bottle.

  3. The mass of the water in the bottle is 500 mL.

  4. The molarity of the water in this bottle is 1.00 M.

Question 9

9. How many moles of Ca(NO3)2 are there in a sample with a mass of 50.0 g?

  1. 0.305 mol

  2. 0.333 mol

  3. 0.490 mol

  4. 8200 mol

Question 10

10. What is the molarity of a sugar solution that has 45.0 g of sugar, C12H22O11, dissolved in 250 mL of water?

  1. 0.53 M

  2. 0.016 M

  3. 0.18 M

  4. 0.0010 M

Question 11

11. You want to make 100.0 mL of a 0.75 M solution of potassium sulfate. What mass of solid potassium sulfate should you use?

  1. 430 mg

  2. 1.3 g

  3. 13 g

  4. 13 kg

Question 12

12. What is the pH of a 1.0 × 10−5 M HCl solution?

  1. −5

  2. 5

  3. 9

  4. −9

Question 13

13. What is the pH of a 0.001 M NaOH solution?

  1. −3

  2. 2

  3. 3

  4. 11

Question 14

14. Which of the following is a balanced neutralization reaction?

  1. 2HNO3(aq) + CaOH2 (aq) → 2H2O(l) + Ca(NO3)2(aq)

  2. H2SO4(aq) + KOH(aq) → H2O(l) + K2SO4(aq)

  3. HC2H3O2(aq) + NH4OH(aq) → 2H2O(l) + NH2C2H3O(aq)

  4. 2H3PO4(aq) + 3Mg(OH)2(aq) → 6H2O(l) + Mg3(PO4)2(aq)

Question 15

15. If 15.0 mL of 0.50 M HCl solution is required to neutralize 34.1 mL of NaOH, what is the molarity of the base?

  1. 0.22 M NaOH

  2. 0.26 M NaOH

  3. 1.14 M NaOH

  4. 4.6 M NaOH

480

Question 16

16. Which solid would be best to add to a solution of Cu(NO3)2 in order to remove the Cu2+ from the solution?

  1. NaCl(s)

  2. KOH(s)

  3. Mg(NO3)2(s)

  4. PbCO3(s)

Question 17

17. The reaction to form ammonia gas, NH3, is shown in the chemical equation below. Which statement correctly describes this chemical reaction?

N2(g) + 3H2(g) → 2NH3(g)

  1. The mole ratio cannot be determined because the chemical equation is not balanced.

  2. More molecules of N2 are needed than H2 molecules to maximize the amount of NH3 produced.

  3. To produce 2 mol of NH3, three times as many moles of H2 are needed as moles of N2.

  4. If 6 mol of H2 and 2 mol of N2 are used, then 2 mol of NH3 will be produced.

Question 18

18. Consider the reaction below. What mass of sodium chloride will be produced if 5.0 g of calcium oxalate is made?

CaCl2(aq) + Na2C2O4(aq) → 2NaCl(aq) + CaC2O4(s)

  1. 2.3 g NaCl

  2. 4.6 g NaCl

  3. 11 g NaCl

  4. 22 g NaCl

Question 19

19. Consider the reaction below. How many grams of Zn3(PO4)2 can be made with 26.5 g of Zn(NO3)2 and 19.7 g of Na3PO4?

3Zn(NO3)2(aq) + 2Na3PO4(aq) → Zn3(PO4)2(s) + 6NaNO3(aq)

  1. 12.0 g Zn3(PO4)2 because Zn(NO3)2 is the limiting reagent

  2. 18.0 g Zn3(PO4)2 because Zn(NO3)2 is the limiting reagent

  3. 23.2 g Zn3(PO4)2 because Na3PO4 is the limiting reagent

  4. 34.8 g Zn3(PO4)2 because Na3PO4 is the limiting reagent

Question 20

20. Consider the balanced chemical equation below. Which substance is the limiting reactant, and how many moles of Fe3O4 can be obtained by reacting 16.8 g Fe with 10.0 g H2O?

3Fe(s) + 4H2O(g) → Fe3O4(s) + 4H2(g)

  1. Iron is the limiting reactant and 0.100 mol Fe3O4 can be formed.

  2. Water is the limiting reactant and 0.100 mol Fe3O4 can be formed.

  3. Iron is the limiting reactant and 0.902 mol Fe3O4 can be formed.

  4. Water is the limiting reactant and 0.902 mol Fe3O4 can be formed.