Chapter 4 Part 1 Practice

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Chapter 4 Part 1 Practice"

Transcription

1 Chapter 4 Part 1 Practice Student: 1. Which of these compounds is a strong electrolyte? A. H 2 O B. O 2 C. H 2 SO 4 D. C 6 H 12 O 6 (glucose) E. CH 3 COOH (acetic acid) 2. Which of these compounds is a weak electrolyte? A. HCl B. CH 3 COOH (acetic acid) C. C 6 H 12 O 6 (glucose) D. O 2 E. NaCl 3. Which of these compounds is a nonelectrolyte? A. NaOH B. HNO 3 C. C 2 H 6 O (ethanol) D. KF E. CH 3 COOH (acetic acid) 4. Identify the major ionic species present in an aqueous solution of Na 2 CO 3. A. Na 2 +, CO 3 2- B. Na 2 +, C 2-, O 3 C. Na +, C 4+, O 3 2- D. Na +, C +, O 2- E. Na +, CO The distinguishing characteristic of all electrolyte solutions is that they A. contain molecules. B. conduct electricity. C. react with other solutions. D. always contain acids. E. conduct heat. 6. Based on the solubility rules, which one of these compounds should be insoluble in water? A. NaCl B. MgBr 2 C. FeCl 2 D. AgBr E. ZnCl 2 7. Based on the solubility rules, which one of these compounds should be insoluble in water? A. Na 2 SO 4 B. BaSO 4 C. CuSO 4 D. MgSO 4 E. Rb 2 SO 4 8. Based on the solubility rules, which one of these compounds should be insoluble in water? A. CaCO 3 B. (NH 4 ) 2 CO 3 C. Na 2 CO 3 D. K 2 CO 3 E. KNO 3 9. Based on the solubility rules, which one of these compounds should be soluble in water? A. Hg 2 Cl 2 B. Na 2 S C. Ag 2 CO 3 D. Ag 2 S E. BaSO 4

2 10. Based on the solubility rules, which one of these compounds should be soluble in water? A. AgBr B. AgCl C. Ag 2 CO 3 D. AgNO 3 E. Ag 2 S 11. Based on the solubility rules, which one of these compounds should be soluble in water? A. (NH 4 ) 3 PO 4 B. Ca 3 (PO 4 ) 2 C. AlPO 4 D. Ag 3 PO 4 E. Mg 3 (PO 4 ) Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO 3 ) 2 (aq) is mixed with a solution containing 0.1 g of KI(aq)/100 ml? A. KNO 3 will precipitate; Pb 2+ and I - are spectator ions. B. No precipitate will form. C. Pb(NO 3 ) 2 will precipitate; K + and I - are spectator ions. D. PbI 2 will precipitate; K + and NO 3 - are spectator ions. E. Pb 2+ and I - are spectator ions, and PbI 2 will precipitate. 13. Based on the solubility rules, which of these processes will occur if solutions of CuSO 4 (aq) and BaCl 2 (aq) are mixed? A. CuCl 2 will precipitate; Ba 2+ and SO 2-4 are spectator ions. B. CuSO 4 will precipitate; Ba 2+ and Cl - are spectator ions. C. BaSO 4 will precipitate; Cu 2+ and Cl - are spectator ions. D. BaCl 2 will precipitate; Cu 2+ and SO 2-4 are spectator ions. E. No precipitate will form. 14. Based on the solubility rules, which of these processes will occur when solutions of ZnSO 4 (aq) and MgCl 2 (aq) are mixed? A. ZnCl 2 will precipitate; Mg 2+ and SO 2-4 will be spectator ions. B. ZnSO 4 will precipitate; Mg 2+ and Cl - will be spectator ions. C. MgSO 4 will precipitate; Zn 2+ and Cl - will be spectator ions. D. MgCl 2 will precipitate; Zn 2+ and SO 2-4 will be spectator ions. E. No precipitate will form. 15. The common constituent in all acid solutions is A. H 2. B. H +. C. OH -. D. H 2 SO 4. E. Cl Identify the major ions present in an aqueous LiOH solution. A. Li 2+, O -, H - B. Li +, OH - C. LiO -, H + D. Li +, O 2-, H + E. Li -, OH Identify the major ions present in an aqueous HNO 3 solution. A. HN +, O 2- B. OH -, NO - 3 C. OH -, NO D. H +, N 3-, O 2- E. H +, NO What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide? A. CaO B. CaCl 2 C. CaH 2 D. CaCl E. CaClH

3 19. What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium hydroxide? A. CaNO 3 B. Ca 2 (NO 3 ) 3 C. Ca 3 (NO 3 ) 2 D. Ca 2 NO 3 E. Ca(NO 3 ) What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with sulfuric acid? A. KSO 3 B. K 2 (SO 4 ) 3 C. K 2 SO 4 D. K(SO 4 ) 2 E. KSO The oxidation number of N in NaNO 3 is A. +6. B. +5. C. +3. D. -3. E. none of these. 22. The oxidation number of S in K 2 SO 4 is A. +6. B. +4. C. +2. D. -1. E. none of these. 23. The oxidation number of Mn in KMnO 4 is A. +8. B. +7. C. +5. D. -7. E The oxidation number of Cr in Cr 2 O 2-7 is A B. -7. C. -2. D. +6. E The oxidation number of Cl in ClO - 3 is A. -1. B. +7. C. +5. D. +3. E. none of these. 26. The oxidation number of N in N 2 H 4 is A. +4. B. -4. C. +2. D. -2. E Which choice gives the correct oxidation numbers for all three elements in Rb 2 SO 3 in the order that the elements are shown in the formula? A. -2, +6, -2 B. -1, +4, -3 C. +2, +4, -2 D. +1, +4, -2 E. +1, +6, -6

4 28. Which one of these equations describes a redox reaction? A. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) B. 2KBr(aq) + Pb(NO3 ) 2 (aq) 2KNO 3 (aq) + PbBr 2 (s) C. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) D. H + (aq) + OH - (aq) H 2 O(l) E. CO3 2- (aq) + HSO 4 - (aq) HCO 3 - (aq) + SO 4 2- (aq) 29. Which of these equations does not represent an oxidation-reduction reaction? A. 3Al + 6HCl 3H2 + AlCl 3 B. 2H2 O 2H 2 + O 2 C. 2NaCl + Pb(NO3 ) 2 PbCl 2 + 3NaNO 3 D. 2NaI + Br2 2NaBr + I 2 E. Cu(NO3 ) 2 + Zn Zn(NO 3 ) 2 + Cu 30. In the chemical reaction 5H 2 O 2 + 2MnO H + 2Mn H 2 O + 5O 2, the oxidizing agent is A. H 2 O 2. B. MnO 4 -. C. H +. D. Mn 2+. E. O In the chemical reaction 5S + 6KNO 3 + 2CaCO 3 3K 2 SO 4 + 2CaSO 4 + CO 2 + 3N 2, the oxidizing agent is A. S. B. N 2. C. KNO 3. D. CaSO 4. E. CaCO Identify the reducing agent in the chemical reaction 5Fe 2+ (aq) + MnO 4 - (aq) + 8H + (aq) 5Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l). A. Fe 2+ B. MnO 4 - C. H + D. Mn 2+ E. Fe Identify the reducing agent in the chemical reaction Cd + NiO 2 + 2H 2 O Cd(OH) 2 + Ni(OH) 2. A. Cd B. NiO 2 C. H 2 O D. Cd(OH) 2 E. Ni(OH) What element is oxidized in the chemical reaction 3Cu + 8HNO 3 3Cu(NO 3 ) 2 + 2NO + 4H 2 O? A. Cu B. H C. N D. O E. H 2 O 35. What element is oxidized in the chemical reaction NiO 2 + Cd + 2H 2 O Ni(OH) 2 + Cd(OH) 2? A. Ni B. Cd C. O D. H E. This is not a redox reaction.

5 36. What element is reduced in the chemical reaction Cu + 2H 2 SO 4 CuSO 4 + SO 2 + 2H 2 O? A. Cu B. H C. S D. O E. H 2 O 37. Predict the products of the single replacement reaction Fe(s) + CuSO 4 (aq)? A. Cu(s) + FeSO 4 (aq) B. Fe(s) + Cu(s) + SO 4 (aq) C. CuS(s) + Fe 2 SO 4 (aq) D. FeCuSO 4 (aq) E. FeO(s) + CuSO 3 (aq) 38. Which of these chemical equations describes a precipitation reaction? A. 2H2 (g) + O 2 (g) 2H 2 O(l) B. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) C. 2KNO3 (s) 2KNO 2 (s) + O 2 (g) D. 2KBr(aq) + Cl2 (g) 2KCl(aq) + Br 2 (l) E. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) 39. Which of these chemical equations describes an acid-base neutralization reaction? A. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) B. SO2 (g) + H 2 O(l) H 2 SO 3 (g) C. LiOH(aq) + HNO3 (aq) LiNO 3 (aq) + H 2 O(l) D. 2KBr(aq) + Cl2 (g) 2KCl(aq) + Br 2 (l) E. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) 40. Which of these chemical equations describes a combustion reaction? A. 2C2 H 6 (g) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(l) B. LiOH(aq) + HNO3 (aq) LiNO 3 (aq) + H 2 O(l) C. N2 (g) + 3H 2 (g) 2NH 3 (g) D. 2Na(s) + 2H2 O(l) 2NaOH(aq) + H 2 (g) E. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) 41. What are three characteristics of a base? 42. What are three characteristics of an acid?

6 43. Give an example of a diprotic acid. 44. Write the net ionic equation for the following reaction. Aqueous iron(iii) sulfate is added to aqueous sodium sulfide to produce solid iron(iii) sulfide and aqueous sodium sulfate.

7 Chapter 4 Part 1 Practice Key 1. Which of these compounds is a strong electrolyte? A. H 2 O B. O 2 C. H 2 SO 4 D. C 6 H 12 O 6 (glucose) E. CH 3 COOH (acetic acid) 2. Which of these compounds is a weak electrolyte? A. HCl B. CH 3 COOH (acetic acid) C. C 6 H 12 O 6 (glucose) D. O 2 E. NaCl 3. Which of these compounds is a nonelectrolyte? A. NaOH B. HNO 3 C. C 2 H 6 O (ethanol) D. KF E. CH 3 COOH (acetic acid) 4. Identify the major ionic species present in an aqueous solution of Na 2 CO 3. A. Na 2 +, CO 3 2- B. Na 2 +, C 2-, O 3 C. Na +, C 4+, O 3 2- D. Na +, C +, O 2- E. Na +, CO The distinguishing characteristic of all electrolyte solutions is that they A. contain molecules. B. conduct electricity. C. react with other solutions. D. always contain acids. E. conduct heat. Raymond Reactions... #1 Raymond Reactions... #3 Raymond Reactions... #6 Raymond Reactions... #7 Raymond Reactions... #9 6. Based on the solubility rules, which one of these compounds should be insoluble in water? A. NaCl B. MgBr 2 C. FeCl 2 D. AgBr E. ZnCl 2 Raymond Reactions... #10 7. Based on the solubility rules, which one of these compounds should be insoluble in water? A. Na 2 SO 4 B. BaSO 4 C. CuSO 4 D. MgSO 4 E. Rb 2 SO 4 Raymond Reactions... #11

8 8. Based on the solubility rules, which one of these compounds should be insoluble in water? A. CaCO 3 B. (NH 4 ) 2 CO 3 C. Na 2 CO 3 D. K 2 CO 3 E. KNO 3 9. Based on the solubility rules, which one of these compounds should be soluble in water? A. Hg 2 Cl 2 B. Na 2 S C. Ag 2 CO 3 D. Ag 2 S E. BaSO Based on the solubility rules, which one of these compounds should be soluble in water? A. AgBr B. AgCl C. Ag 2 CO 3 D. AgNO 3 E. Ag 2 S 11. Based on the solubility rules, which one of these compounds should be soluble in water? A. (NH 4 ) 3 PO 4 B. Ca 3 (PO 4 ) 2 C. AlPO 4 D. Ag 3 PO 4 E. Mg 3 (PO 4 ) 2 Raymond Reactions... #12 Raymond Reactions... #13 Raymond Reactions... #14 Raymond Reactions... # Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO 3 ) 2 (aq) is mixed with a solution containing 0.1 g of KI(aq)/100 ml? A. KNO 3 will precipitate; Pb 2+ and I - are spectator ions. B. No precipitate will form. C. Pb(NO 3 ) 2 will precipitate; K + and I - are spectator ions. D. PbI 2 will precipitate; K + and NO 3 - are spectator ions. E. Pb 2+ and I - are spectator ions, and PbI 2 will precipitate. Raymond Reactions... # Based on the solubility rules, which of these processes will occur if solutions of CuSO 4 (aq) and BaCl 2 (aq) are mixed? A. CuCl 2 will precipitate; Ba 2+ and SO 2-4 are spectator ions. B. CuSO 4 will precipitate; Ba 2+ and Cl - are spectator ions. C. BaSO 4 will precipitate; Cu 2+ and Cl - are spectator ions. D. BaCl 2 will precipitate; Cu 2+ and SO 2-4 are spectator ions. E. No precipitate will form. Raymond Reactions... # Based on the solubility rules, which of these processes will occur when solutions of ZnSO 4 (aq) and MgCl 2 (aq) are mixed? A. ZnCl 2 will precipitate; Mg 2+ and SO 4 2- will be spectator ions. B. ZnSO 4 will precipitate; Mg 2+ and Cl - will be spectator ions. C. MgSO 4 will precipitate; Zn 2+ and Cl - will be spectator ions. D. MgCl 2 will precipitate; Zn 2+ and SO 4 2- will be spectator ions. E. No precipitate will form. Raymond Reactions... #19

9 15. The common constituent in all acid solutions is A. H 2. B. H +. C. OH -. D. H 2 SO 4. E. Cl Identify the major ions present in an aqueous LiOH solution. A. Li 2+, O -, H - B. Li +, OH - C. LiO -, H + D. Li +, O 2-, H + E. Li -, OH Identify the major ions present in an aqueous HNO 3 solution. A. HN +, O 2- B. OH -, NO - 3 C. OH -, NO D. H +, N 3-, O 2- E. H +, NO - 3 Raymond Reactions... #21 Raymond Reactions... #22 Raymond Reactions... # What is the correct formula of the salt formed in the neutralization reaction of hydrochloric acid with calcium hydroxide? A. CaO B. CaCl 2 C. CaH 2 D. CaCl E. CaClH Raymond Reactions... # What is the chemical formula of the salt produced by the neutralization of nitric acid with calcium hydroxide? A. CaNO 3 B. Ca 2 (NO 3 ) 3 C. Ca 3 (NO 3 ) 2 D. Ca 2 NO 3 E. Ca(NO 3 ) 2 Raymond Reactions... # What is the chemical formula of the salt produced by the neutralization of potassium hydroxide with sulfuric acid? A. KSO 3 B. K 2 (SO 4 ) 3 C. K 2 SO 4 D. K(SO 4 ) 2 E. KSO The oxidation number of N in NaNO 3 is A. +6. B. +5. C. +3. D. -3. E. none of these. 22. The oxidation number of S in K 2 SO 4 is A. +6. B. +4. C. +2. D. -1. E. none of these. Raymond Reactions... #28 Raymond Reactions... #29 Raymond Reactions... #30

10 23. The oxidation number of Mn in KMnO 4 is A. +8. B. +7. C. +5. D. -7. E The oxidation number of Cr in Cr 2 O 2-7 is A B. -7. C. -2. D. +6. E The oxidation number of Cl in ClO - 3 is A. -1. B. +7. C. +5. D. +3. E. none of these. 26. The oxidation number of N in N 2 H 4 is A. +4. B. -4. C. +2. D. -2. E. 0. Raymond Reactions... #31 Raymond Reactions... #33 Raymond Reactions... #34 Raymond Reactions... # Which choice gives the correct oxidation numbers for all three elements in Rb 2 SO 3 in the order that the elements are shown in the formula? A. -2, +6, -2 B. -1, +4, -3 C. +2, +4, -2 D. +1, +4, -2 E. +1, +6, Which one of these equations describes a redox reaction? A. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) B. 2KBr(aq) + Pb(NO3 ) 2 (aq) 2KNO 3 (aq) + PbBr 2 (s) Raymond Reactions... #40 C. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) D. H + (aq) + OH - (aq) H 2 O(l) E. CO3 2- (aq) + HSO 4 - (aq) HCO 3 - (aq) + SO 4 2- (aq) 29. Which of these equations does not represent an oxidation-reduction reaction? A. 3Al + 6HCl 3H2 + AlCl 3 Raymond Reactions... #41 B. 2H2 O 2H 2 + O 2 C. 2NaCl + Pb(NO3 ) 2 PbCl 2 + 3NaNO 3 D. 2NaI + Br2 2NaBr + I 2 E. Cu(NO3 ) 2 + Zn Zn(NO 3 ) 2 + Cu Raymond Reactions... #42

11 30. In the chemical reaction 5H 2 O 2 + 2MnO H + 2Mn H 2 O + 5O 2, the oxidizing agent is A. H 2 O 2. B. MnO 4 -. C. H +. D. Mn 2+. E. O 2. Difficulty: Difficult Raymond Reactions... # In the chemical reaction 5S + 6KNO 3 + 2CaCO 3 3K 2 SO 4 + 2CaSO 4 + CO 2 + 3N 2, the oxidizing agent is A. S. B. N 2. C. KNO 3. D. CaSO 4. E. CaCO Identify the reducing agent in the chemical reaction 5Fe 2+ (aq) + MnO 4 - (aq) + 8H + (aq) 5Fe 3+ (aq) + Mn 2+ (aq) + 4H 2 O(l). A. Fe 2+ B. MnO 4 - C. H + D. Mn 2+ E. Fe Identify the reducing agent in the chemical reaction Cd + NiO 2 + 2H 2 O Cd(OH) 2 + Ni(OH) 2. A. Cd B. NiO 2 C. H 2 O D. Cd(OH) 2 E. Ni(OH) What element is oxidized in the chemical reaction 3Cu + 8HNO 3 3Cu(NO 3 ) 2 + 2NO + 4H 2 O? A. Cu B. H C. N D. O E. H 2 O 35. What element is oxidized in the chemical reaction NiO 2 + Cd + 2H 2 O Ni(OH) 2 + Cd(OH) 2? A. Ni B. Cd C. O D. H E. This is not a redox reaction. 36. What element is reduced in the chemical reaction Cu + 2H 2 SO 4 CuSO 4 + SO 2 + 2H 2 O? A. Cu B. H C. S D. O E. H 2 O Difficulty: Difficult Raymond Reactions... #44 Difficulty: Difficult Raymond Reactions... #46 Difficulty: Difficult Raymond Reactions... #47 Raymond Reactions... #48 Raymond Reactions... #49 Raymond Reactions... #51

12 37. Predict the products of the single replacement reaction Fe(s) + CuSO 4 (aq)? A. Cu(s) + FeSO 4 (aq) B. Fe(s) + Cu(s) + SO 4 (aq) C. CuS(s) + Fe 2 SO 4 (aq) D. FeCuSO 4 (aq) E. FeO(s) + CuSO 3 (aq) 38. Which of these chemical equations describes a precipitation reaction? A. 2H2 (g) + O 2 (g) 2H 2 O(l) Raymond Reactions... #52 B. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) C. 2KNO3 (s) 2KNO 2 (s) + O 2 (g) D. 2KBr(aq) + Cl2 (g) 2KCl(aq) + Br 2 (l) E. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) 39. Which of these chemical equations describes an acid-base neutralization reaction? A. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) Raymond Reactions... #56 B. SO2 (g) + H 2 O(l) H 2 SO 3 (g) C. LiOH(aq) + HNO3 (aq) LiNO 3 (aq) + H 2 O(l) D. 2KBr(aq) + Cl2 (g) 2KCl(aq) + Br 2 (l) E. CaBr2 (aq) + H 2 SO 4 (aq) CaSO 4 (s) + 2HBr(g) 40. Which of these chemical equations describes a combustion reaction? A. 2C2 H 6 (g) + 7O 2 (g) 4CO 2 (g) + 6H 2 O(l) B. LiOH(aq) + HNO3 (aq) LiNO 3 (aq) + H 2 O(l) Raymond Reactions... #57 C. N2 (g) + 3H 2 (g) 2NH 3 (g) D. 2Na(s) + 2H2 O(l) 2NaOH(aq) + H 2 (g) E. 2Al(s) + 3H2 SO 4 (aq) Al 2 (SO 4 ) 3 (aq) + 3H 2 (g) 41. What are three characteristics of a base? Raymond Reactions... #59 a. A base has a bitter taste. b. A base feels slippery. c. A base changes red litmus paper to blue. 42. What are three characteristics of an acid? Raymond Reactions... #100 a. An acid has a sour taste. b. An acid changes blue litmus paper to red. c. An acid reacts with certain metals to produce hydrogen gas. 43. Give an example of a diprotic acid. Raymond Reactions... #101 H 2 CO 3 Raymond Reactions... #103

13 44. Write the net ionic equation for the following reaction. Aqueous iron(iii) sulfate is added to aqueous sodium sulfide to produce solid iron(iii) sulfide and aqueous sodium sulfate. 2Fe 3+ (aq) + 3S 2- (aq) Fe 2 S 3 (s) Raymond Reactions... #105

14 Category # of Questions Difficulty: Difficult Raymond Reactions Chapter 4 Part 1 Practice Summary

Steps for balancing a chemical equation

Steps for balancing a chemical equation The Chemical Equation: A Chemical Recipe Dr. Gergens - SD Mesa College A. Learn the meaning of these arrows. B. The chemical equation is the shorthand notation for a chemical reaction. A chemical equation

More information

Experiment 1 Chemical Reactions and Net Ionic Equations

Experiment 1 Chemical Reactions and Net Ionic Equations Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is:

NET IONIC EQUATIONS. A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NET IONIC EQUATIONS A balanced chemical equation can describe all chemical reactions, an example of such an equation is: NaCl + AgNO 3 AgCl + NaNO 3 In this case, the simple formulas of the various reactants

More information

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s)

Potassium + Chlorine. K(s) + Cl 2 (g) 2 KCl(s) Types of Reactions Consider for a moment the number of possible chemical reactions. Because there are millions of chemical compounds, it is logical to expect that there are millions of possible chemical

More information

Reactions in Aqueous Solution

Reactions in Aqueous Solution CHAPTER 7 1. Water is the most universal of all liquids. Water has a relatively large heat capacity and a relatively large liquid range, which means it can absorb the heat liberated by many reactions while

More information

Lecture 6. Classes of Chemical Reactions

Lecture 6. Classes of Chemical Reactions Lecture 6 Classes of Chemical Reactions Lecture 6 Outline 6.1 The Role of Water as a Solvent 6.2 Precipitation Reactions 6.3 Acid-Base Reactions 1 Electron distribution in molecules of H 2 and H 2 O The

More information

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction

Chapter 5. Chemical Reactions and Equations. Introduction. Chapter 5 Topics. 5.1 What is a Chemical Reaction Introduction Chapter 5 Chemical Reactions and Equations Chemical reactions occur all around us. How do we make sense of these changes? What patterns can we find? 1 2 Copyright The McGraw-Hill Companies,

More information

Experiment 9 - Double Displacement Reactions

Experiment 9 - Double Displacement Reactions Experiment 9 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

stoichiometry = the numerical relationships between chemical amounts in a reaction.

stoichiometry = the numerical relationships between chemical amounts in a reaction. 1 REACTIONS AND YIELD ANSWERS stoichiometry = the numerical relationships between chemical amounts in a reaction. 2C 8 H 18 (l) + 25O 2 16CO 2 (g) + 18H 2 O(g) From the equation, 16 moles of CO 2 (a greenhouse

More information

Tutorial 5 NET IONIC EQUATIONS

Tutorial 5 NET IONIC EQUATIONS T-33 Tutorial 5 NET IONIC EQUATIONS The efficiency and extent of a chemical reaction is very much dependent upon the physical state (solid, liquid, gas, or solution) of reactants and products. Not surprisingly,

More information

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent

Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:

More information

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change

Chemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure

More information

Test 12: Review questions

Test 12: Review questions Name: Wednesday, April 16, 2008 Test 12: Review questions 1. Which reaction represents the process of neutralization? 1. Mg(s) + 2HCl(aq) MgCl 2(aq) + H 2(g) 2. HCl(aq) + KOH(aq) KCl(aq) + H2O(l) 3. Pb(NO

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry

Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry AP Chemistry A. Allan Chapter 4 Notes - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent A. Structure of water 1. Oxygen's electronegativity is high (3.5) and hydrogen's

More information

Chapter 7: Chemical Reactions

Chapter 7: Chemical Reactions Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that

More information

Practise Exam Chapter 4

Practise Exam Chapter 4 Practise Exam Chapter 4 1. Which one of the following is a nonelectrolyte? A) aqueous barium nitrate solution B) aqueous calcium chloride solution C) aqueous lithium phosphate solution D) aqueous methyl

More information

Chapter 4 Chemical Reactions

Chapter 4 Chemical Reactions Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser

More information

1. Balancing a chemical equation so that it obeys the law of conservation of matter requires:

1. Balancing a chemical equation so that it obeys the law of conservation of matter requires: General Chemistry I Exam 2 Review 1 1. Balancing a chemical equation so that it obeys the law of conservation of matter requires: a. Adjusting the coefficients in front of the d. Changing the formulas

More information

Experiment 8 - Double Displacement Reactions

Experiment 8 - Double Displacement Reactions Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are

More information

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation.

H 2 + O 2 H 2 O. - Note there is not enough hydrogen to react with oxygen - It is necessary to balance equation. CEMICAL REACTIONS 1 ydrogen + Oxygen Water 2 + O 2 2 O reactants product(s) reactant substance before chemical change product substance after chemical change Conservation of Mass During a chemical reaction,

More information

David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College

David A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,

More information

Aqueous Ions and Reactions

Aqueous Ions and Reactions Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for

More information

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate

More information

6 Reactions in Aqueous Solutions

6 Reactions in Aqueous Solutions 6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface

More information

Molarity of Ions in Solution

Molarity of Ions in Solution APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.

More information

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes

4.1 Aqueous Solutions. Chapter 4. Reactions in Aqueous Solution. Electrolytes. Strong Electrolytes. Weak Electrolytes Chapter 4 Reactions in Aqueous Solution 4.1 Aqueous Solutions Solution homogeneous mixture of 2 or more substances Solute the substance present in a smaller amount (usually solid in Chap. 4) Solvent the

More information

Chemical Equations and Chemical Reactions. Chapter 8.1

Chemical Equations and Chemical Reactions. Chapter 8.1 Chemical Equations and Chemical Reactions Chapter 8.1 Objectives List observations that suggest that a chemical reaction has taken place List the requirements for a correctly written chemical equation.

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up )

2. DECOMPOSITION REACTION ( A couple have a heated argument and break up ) TYPES OF CHEMICAL REACTIONS Most reactions can be classified into one of five categories by examining the types of reactants and products involved in the reaction. Knowing the types of reactions can help

More information

SOLUBILITY CURVES WORKSHEET

SOLUBILITY CURVES WORKSHEET SOLUBILITY CURVES WORKSHEET 1.) Which compound is least soluble at 20 o C? At 80 o C? 2.) Which substance is the most soluble at 10 o C? At 50 o C? At 90 o C? 3.) The solubility of which substance is most

More information

4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine.

4. Balanced chemical equations tell us in what molar ratios substances combine to form products, not in what mass proportions they combine. CHAPTER 9 1. The coefficients of the balanced chemical equation for a reaction give the relative numbers of molecules of reactants and products that are involved in the reaction.. The coefficients of the

More information

GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing

GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing GHW#9. Louisiana Tech University, Chemistry 100. POGIL Exercise on Chapter 4. Quantities of Reactants and Products: Equations, Patterns and Balancing Why? In chemistry, chemical equations represent changes

More information

CHAPTER 4. AQUEOUS REACTION CHEMISTRY

CHAPTER 4. AQUEOUS REACTION CHEMISTRY CAPTER. AQUEOUS REACTION CEMISTRY solution - homogeneous mixture of or more substances; uniform distribution of particles and same properties throughout. A solution is composed of a solute dissolved in

More information

Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions

Chapter 11. Electrochemistry Oxidation and Reduction Reactions. Oxidation-Reduction Reactions. Oxidation-Reduction Reactions Oxidation-Reduction Reactions Chapter 11 Electrochemistry Oxidation and Reduction Reactions An oxidation and reduction reaction occurs in both aqueous solutions and in reactions where substances are burned

More information

Chapter 8: Chemical Equations and Reactions

Chapter 8: Chemical Equations and Reactions Chapter 8: Chemical Equations and Reactions I. Describing Chemical Reactions A. A chemical reaction is the process by which one or more substances are changed into one or more different substances. A chemical

More information

Chapter 8 - Chemical Equations and Reactions

Chapter 8 - Chemical Equations and Reactions Chapter 8 - Chemical Equations and Reactions 8-1 Describing Chemical Reactions I. Introduction A. Reactants 1. Original substances entering into a chemical rxn B. Products 1. The resulting substances from

More information

1/7/2013. Chapter 9. Chemical Reactions in Aqueous Solutions. Chemistry: Atoms First Julia Burdge & Jason Overby. Reactions in Aqueous Solutions 9.

1/7/2013. Chapter 9. Chemical Reactions in Aqueous Solutions. Chemistry: Atoms First Julia Burdge & Jason Overby. Reactions in Aqueous Solutions 9. Chemistry: Atoms First Julia Burdge & Jason Overby 9 Reactions in Aqueous s Chapter 9 Chemical Reactions in Aqueous s Kent L. McCorkle Cosumnes River College Sacramento, CA Copyright (c) The McGraw-Hill

More information

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS

UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS UNIT (4) CALCULATIONS AND CHEMICAL REACTIONS 4.1 Formula Masses Recall that the decimal number written under the symbol of the element in the periodic table is the atomic mass of the element. 1 7 8 12

More information

Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction

Worksheet # 11. 4. When heated, nickel (II) carbonate undergoes a decomposition reaction. Write a balanced equation to describe this reaction Worksheet # 11 1. A solution of sodium chloride is mixed with a solution of lead (II) nitrate. A precipitate of lead (II) chloride results, leaving a solution of sodium nitrated. Determine the class of

More information

Oxidation-Reduction Reactions

Oxidation-Reduction Reactions CHAPTER 19 REVIEW Oxidation-Reduction Reactions SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. All the following equations involve redox reactions except (a) CaO H 2 O

More information

Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources

Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Department of Chemical Engineering Review Sheet Chemical Reactions Prepared by Dr. Timothy D. Placek from various sources Introduction This document is intended to help you review the basics of writing

More information

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ

Experiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical

More information

REVIEW QUESTIONS Chapter 8

REVIEW QUESTIONS Chapter 8 Chemistry 51 ANSWER KEY REVIEW QUESTIONS Chapter 8 1. Identify each of the diagrams below as strong electrolyte, weak electrolyte or non-electrolyte: (a) Non-electrolyte (no ions present) (b) Weak electrolyte

More information

Writing, Balancing and Predicting Products of Chemical Reactions.

Writing, Balancing and Predicting Products of Chemical Reactions. Writing, Balancing and Predicting Products of Chemical Reactions. A chemical equation is a concise shorthand expression which represents the relative amount of reactants and products involved in a chemical

More information

Chem 111 Evening Exam #3

Chem 111 Evening Exam #3 * Enter your answers on the bubble sheet. Turn in all sheets. * This exam is composed of 25 questions on 7 pages total. Go initially through the exam and answer the questions you can answer quickly. Then

More information

Chapter 6 Notes Science 10 Name:

Chapter 6 Notes Science 10 Name: 6.1 Types of Chemical Reactions a) Synthesis (A + B AB) Synthesis reactions are also known as reactions. When this occurs two or more reactants (usually elements) join to form a. A + B AB, where A and

More information

Decomposition. Composition

Decomposition. Composition Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus

More information

EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS

EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS PURPOSE EXPERIMENT 5: CHEMICAL REACTIONS AND EQUATIONS To perform and observe simple chemical reactions. To identify the products of chemical reactions and write balanced equations for those reactions.

More information

Balancing Chemical Equations

Balancing Chemical Equations Balancing Chemical Equations 1. sodium carbonate + calcium hydroxide sodium hydroxide + calcium carbonate Na 2 CO 3 + Ca(OH) 2 2 NaOH + CaCO 3 2. carbon dioxide + water carbonic acid CO 2 + H 2 O H 2 CO

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Chem 101 Reactions in Aqueous Solutions Lectures 15 and 16 Predicting Whether a Reaction Will Occur Forces that drive a reaction Formation of a solid Formation of water Transfer of electrons Formation

More information

Chemistry Themed. Types of Reactions

Chemistry Themed. Types of Reactions Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start

More information

Balancing Chemical Equations Worksheet Intermediate Level

Balancing Chemical Equations Worksheet Intermediate Level Balancing Chemical Equations Worksheet Intermediate Level Neutralization Reactions Salts are produced by the action of acids. Salts are written metal first, then non-metal. Eg. NaCl not ClNa Acid + Base

More information

Chapter 4 An Introduction to Chemical Reactions

Chapter 4 An Introduction to Chemical Reactions 37 Chapter 4 An Introduction to Chemical Reactions Review Skills 4.1 Chemical Reactions and Chemical Equations Interpreting a Chemical Equation Balancing Chemical Equations Internet: Balancing Equations

More information

EXPERIMENT 8: Activity Series (Single Displacement Reactions)

EXPERIMENT 8: Activity Series (Single Displacement Reactions) EPERIMENT 8: Activity Series (Single Displacement Reactions) PURPOSE a) Reactions of metals with acids and salt solutions b) Determine the activity of metals c) Write a balanced molecular equation, complete

More information

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction?

Chapter 6 Oxidation-Reduction Reactions. Section 6.1 2. Which one of the statements below is true concerning an oxidation-reduction reaction? Chapter 6 Oxidation-Reduction Reactions 1. Oxidation is defined as a. gain of a proton b. loss of a proton c. gain of an electron! d. loss of an electron e. capture of an electron by a neutron 2. Which

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent.

Chemistry 51 Chapter 8 TYPES OF SOLUTIONS. A solution is a homogeneous mixture of two substances: a solute and a solvent. TYPES OF SOLUTIONS A solution is a homogeneous mixture of two substances: a solute and a solvent. Solute: substance being dissolved; present in lesser amount. Solvent: substance doing the dissolving; present

More information

Writing and Balancing Chemical Equations

Writing and Balancing Chemical Equations Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

More information

38. Consider the following reaction that occurs in a breathalyzer: 2Cr 2 O 7

38. Consider the following reaction that occurs in a breathalyzer: 2Cr 2 O 7 Electrochemistry Multiple Choice January 1999 37. Consider the following redox reaction: 2MnO 4 - + 3ClO 3 - + H 2 O 3ClO 4 - + 2MnO 2 + 2OH - The reducing agent is A. H 2 O B. ClO 3 - C. MnO 2 D. MnO

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

Redox and Electrochemistry

Redox and Electrochemistry Name: Thursday, May 08, 2008 Redox and Electrochemistry 1. A diagram of a chemical cell and an equation are shown below. When the switch is closed, electrons will flow from 1. the Pb(s) to the Cu(s) 2+

More information

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens.

V. POLYPROTIC ACID IONIZATION. NOTICE: K a1 > K a2 > K a3 EQUILIBRIUM PART 2. A. Polyprotic acids are acids with two or more acidic hydrogens. EQUILIBRIUM PART 2 V. POLYPROTIC ACID IONIZATION A. Polyprotic acids are acids with two or more acidic hydrogens. monoprotic: HC 2 H 3 O 2, HCN, HNO 2, HNO 3 diprotic: H 2 SO 4, H 2 SO 3, H 2 S triprotic:

More information

Common Ion Effects. CH 3 CO 2 (aq) + Na + (aq)

Common Ion Effects. CH 3 CO 2 (aq) + Na + (aq) Common Ion Effects If two reactions both involve the same ion, then one reaction can effect the equilibrium position of the other reaction. The ion that appears in both reactions is the common ion. Buffers

More information

Types of Reactions. CHM 130LL: Chemical Reactions. Introduction. General Information

Types of Reactions. CHM 130LL: Chemical Reactions. Introduction. General Information Introduction CHM 130LL: Chemical Reactions We often study chemistry to understand how and why chemicals (reactants) can be transformed into different chemicals (products) via a chemical reaction: Reactants

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces

More information

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases

Chapter 17. How are acids different from bases? Acid Physical properties. Base. Explaining the difference in properties of acids and bases Chapter 17 Acids and Bases How are acids different from bases? Acid Physical properties Base Physical properties Tastes sour Tastes bitter Feels slippery or slimy Chemical properties Chemical properties

More information

CHAPTER 5: MOLECULES AND COMPOUNDS

CHAPTER 5: MOLECULES AND COMPOUNDS CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting

More information

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l)

3. Which of the following describes a conjugate acid-base pair for the following equilibrium? CN - (aq) + CH 3 NH 3 + (aq) H 2 CO 3 (aq) + H 2 O (l) Acids, Bases & Redox 1 Practice Problems for Assignment 8 1. A substance which produces OH ions in solution is a definition for which of the following? (a) an Arrhenius acid (b) an Arrhenius base (c) a

More information

SAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK

SAMPLE PROBLEM 8.1. Solutions of Electrolytes and Nonelectrolytes SOLUTION STUDY CHECK Solutions of Electrolytes and Nonelectrolytes SAMPLE PROBLEM 8.1 Indicate whether solutions of each of the following contain only ions, only molecules, or mostly molecules and a few ions: a. Na 2 SO 4,

More information

2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions.

2. Write the chemical formula(s) of the product(s) and balance the following spontaneous reactions. 1. Using the Activity Series on the Useful Information pages of the exam write the chemical formula(s) of the product(s) and balance the following reactions. Identify all products phases as either (g)as,

More information

Appendix D. Reaction Stoichiometry D.1 INTRODUCTION

Appendix D. Reaction Stoichiometry D.1 INTRODUCTION Appendix D Reaction Stoichiometry D.1 INTRODUCTION In Appendix A, the stoichiometry of elements and compounds was presented. There, the relationships among grams, moles and number of atoms and molecules

More information

Chemistry. Zumdahl, 7th edition

Chemistry. Zumdahl, 7th edition Chemistry Zumdahl, 7th edition CH4 Types of Chemical Reactions and Solution Stoichiometry Yellow lead(ii) iodide is produced when lead(ii) nitrate is mixed with potassium iodide. P.126 Contents 4.1 Water,

More information

Experiment 17-Chemical Reactions Lab

Experiment 17-Chemical Reactions Lab Since the Middle Ages, when ancient physicians attempted to find a magical substance that would cure all diseases, humans have been fascinated with chemical reactions. In order to effectively describe

More information

Chapter 7: Chemical Equations. Name: Date: Period:

Chapter 7: Chemical Equations. Name: Date: Period: Chapter 7: Chemical Equations Name: Date: Period: 7-1 What is a chemical reaction? Read pages 232-237 a) Explain what a chemical reaction is. b) Distinguish between evidence that suggests a chemical reaction

More information

Summer 2003 CHEMISTRY 115 EXAM 3(A)

Summer 2003 CHEMISTRY 115 EXAM 3(A) Summer 2003 CHEMISTRY 115 EXAM 3(A) 1. In which of the following solutions would you expect AgCl to have the lowest solubility? A. 0.02 M BaCl 2 B. pure water C. 0.02 M NaCl D. 0.02 M KCl 2. Calculate

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

CHM-101-A Exam 2 Version 1 October 10, 2006

CHM-101-A Exam 2 Version 1 October 10, 2006 CHM-101-A Exam 2 Version 1 1. Which of the following statements is incorrect? A. SF 4 has ¼ as many sulfur atoms as fluorine atoms. B. Ca(NO 3 ) 2 has six times as many oxygen atoms as calcium ions. C.

More information

= 11.0 g (assuming 100 washers is exact).

= 11.0 g (assuming 100 washers is exact). CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula

More information

Unit 8: Chemical Reactions and Equations

Unit 8: Chemical Reactions and Equations 1 Chemical Reactions Unit 8: Chemical Reactions and Equations What are chemical reactions and how do they occur? How are chemical reactions classified? How are products of chemical reactions predicted?

More information

Chemistry: Chemical Equations

Chemistry: Chemical Equations Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

More information

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS

I N V E S T I C E D O R O Z V O J E V Z D Ě L Á V Á N Í CHEMICAL REACTIONS Chemical reaction = process during which original substances change to new substances, reactants turn to... The bonds of reactants... and new bonds are... The classification of reactions: 1. Classification

More information

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11

1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11 SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436

More information

TOPIC 11: Acids and Bases

TOPIC 11: Acids and Bases TOPIC 11: Acids and Bases ELECTROLYTES are substances that when dissolves in water conduct electricity. They conduct electricity because they will break apart into Ex. NaCl(s)! Na + (aq) + Cl - (aq), and

More information

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

Naming Compounds Handout

Naming Compounds Handout Naming Compounds Handout IONIC COMPOUNDS versus MOLECULAR COMPOUNDS ionic compound: consist of cations (positive ions) and anions (negative ions) held together by electrostatic attraction usually metal

More information

Chemical Reactions in Water Ron Robertson

Chemical Reactions in Water Ron Robertson Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Properties of Compounds in Water Electrolytes and nonelectrolytes Water soluble compounds

More information

Chemical Reactions in Water

Chemical Reactions in Water Chemical Reactions in Water Ron Robertson r2 f:\files\courses\1110-20\2010 possible slides for web\waterchemtrans.doc Acids, Bases and Salts Acids dissolve in water to give H + ions. These ions attach

More information

Stoichiometry and Aqueous Reactions (Chapter 4)

Stoichiometry and Aqueous Reactions (Chapter 4) Stoichiometry and Aqueous Reactions (Chapter 4) Chemical Equations 1. Balancing Chemical Equations (from Chapter 3) Adjust coefficients to get equal numbers of each kind of element on both sides of arrow.

More information

CHEM 102: Sample Test 5

CHEM 102: Sample Test 5 CHEM 102: Sample Test 5 CHAPTER 17 1. When H 2 SO 4 is dissolved in water, which species would be found in the water at equilibrium in measurable amounts? a. H 2 SO 4 b. H 3 SO + 4 c. HSO 4 d. SO 2 4 e.

More information

Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells

Atomic Structure. Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells Atomic Structure called nucleons Name Mass Charge Location Protons 1 +1 Nucleus Neutrons 1 0 Nucleus Electrons 1/1837-1 Orbit nucleus in outer shells The number of protons equals the atomic number This

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

Aqueous Chemical Reactions

Aqueous Chemical Reactions Name: Date: Lab Partners: Lab section: Aqueous Chemical Reactions The purpose of this lab is to introduce you to three major categories of reactions that occur in aqueous solutions: precipitation reactions,

More information

Nomenclature of Ionic Compounds

Nomenclature of Ionic Compounds Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.

More information

Answers and Solutions to Text Problems

Answers and Solutions to Text Problems Chapter 7 Answers and Solutions 7 Answers and Solutions to Text Problems 7.1 A mole is the amount of a substance that contains 6.02 x 10 23 items. For example, one mole of water contains 6.02 10 23 molecules

More information

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe: Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

More information

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical?

6) Which compound is manufactured in larger quantities in the U.S. than any other industrial chemical? MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which statement concerning Arrhenius acid-base theory is not correct? A) Acid-base reactions must

More information