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Chapter Menu. Sec tio n 15.1 Acid and Base Reactions Section 15.2 Applications of Acid-Base Reactions. Click a hyperlink to view the corresponding slides. Chapter Menu. Acid and Base Reactions. Determine the overall, ionic, and net ionic equations for an acid-base reaction.

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  1. Chapter Menu Section 15.1Acid and Base Reactions Section 15.2 Applications of Acid-Base Reactions Click a hyperlink to view the corresponding slides. Chapter Menu

  2. Acid and Base Reactions Determine the overall, ionic, and net ionic equations for an acid-base reaction. Classify acids and bases using the hydrogen transfer definition. Predict and explain the final results of an acid-base reaction. Section 15.1

  3. Acid and Base Reactions pH: mathematical scale in which the concentration of hydrogen ions in a solution is expressed as number from 0 to 14. Section 15.1

  4. Acid and Base Reactions neutralization reaction salt ionic equation spectator ion net ionic equation Brønsted-Lowry model The concentrations of the acid and base determine the classification of an acid-base reaction. Section 15.1

  5. Types of Acid-Base Reactions A neutralization reaction is a reaction of an acid with a base in aqueous solution to produce water and a salt. acid + base → salt + water Section 15.1

  6. Types of Acid-Base Reactions (cont.) Salt is a general term used in chemistry to describe the ionic compound formed from the negative part of the acid and the positive part of the base. Because both acids and bases may be either strong or weak, four possible combinations of acid-base reactions occur. Section 15.1

  7. Types of Acid-Base Reactions (cont.) Section 15.1

  8. Strong Acid + Strong Base An ionic equation is an equation in which substances that primarily exist as ions in solutions are shown as ions. Spectator ions are ions that are present in a solution but do not participate in the reaction. Section 15.1

  9. Strong Acid + Strong Base (cont.) A net ionic equation is an equation that results when ions common to both sides of the equation are removed, usually from an ionic equation. Section 15.1

  10. Strong Acid + Weak Base The submicroscopic interactions between a strong acid-weak base reaction are between hydrogen ions and the bases. The reaction of a strong acid and a weak base is not quite a neutralization. Section 15.1

  11. Strong Acid + Weak Base (cont.) Section 15.1

  12. A Broader Definition of Acids and Bases In the Brønsted-Lowry model, an acid is defined as a substance that donates a hydrogen ion in a chemical reaction. A base is defined as a substance that accepts a hydrogen ion in a chemical reaction. Section 15.1

  13. A Broader Definition of Acids and Bases (cont.) Section 15.1

  14. A Broader Definition of Acids and Bases (cont.) Water can act as an acid or a base, depending upon what else is in the solution. Reactions that result in the transfer of a hydrogen ion do not require water to be present. Section 15.1

  15. Weak Acid + Strong Base The reaction of a weak acid and a strong base does not result in a neutral solution. In the reaction of a weak acid and a strong base, the hydrogen ion transfers from the weak acid to the hydroxide ion. Section 15.1

  16. Weak and Weak: It’s Uncertain The strong-strong reaction plus the two types of weak-strong reactions are the predominant acid-base reactions. Neither a weak acid nor a weak base has a strong tendency to transfer a hydrogen ion. Section 15.1

  17. Section Assessment In a neutralization reaction, an acid and a base react to form: A.saltwater B.salt and ammonia C.salt and water D.salt and oxygen gas Section 15.1

  18. Section Assessment Salt forms from the ___ part of an acid and the ___ part of a base. A.negative; positive B.positive; negative C.negative: negative D.positive; positive Section 15.1

  19. End of Section 15.1

  20. Applications of Acid-Base Reactions Evaluate the importance of a buffer in controlling pH. Perform acid-base titrations. Calculate results from titration data. Section 15.2

  21. Applications of Acid-Base Reactions spectator ions: ions that are present in a solution but do not participate in a reaction. Section 15.2

  22. Applications of Acid-Base Reactions buffer titration standard solution Acid-base reactions play an important role in the human body. Section 15.2

  23. Buffers to Regulate pH A buffer is a solution that resists changes in pH when moderate amounts of acids or bases are added. A buffer contains ions or molecules that react with OH– or H+ if one of these ions is introduced into a solution. Section 15.2

  24. Buffers to Regulate pH (cont.) The ability of blood to maintain a constant pH of 7.4 is due to several buffer systems, including one that involves dissolved carbon dioxide. Section 15.2

  25. Buffers to Regulate pH (cont.) The ability of lakewater to resist the pH-lowering effects of acid rain is in their local geology • The combination of water, CO2, and the calcium carbonate of limestone neutralize acid rain in an acid-base reaction. Section 15.2

  26. The Acid-Base Chemistry of Antacids The acidic environment in the stomach is extremely important for good digestion. If stomach contents become too acidic, it can break down the basic membrane that protects the stomach and eventually lead to gastric ulcers. Section 15.2

  27. The Acid-Base Chemistry of Antacids (cont.) Antacids are substances used to counteract stomach acidity. Hydroxide-containing bases and carbonate-containing bases are two different compounds used in antacids. Section 15.2

  28. The Acid-Base Chemistry of Antacids (cont.) Section 15.2

  29. Stoichiometry Revisited: Acid-Base Titrations Titration is the process of determining the molarity of an acid or base by using an acid-base reaction where one reactant is of known molarity. Solutions of known molarity that are used in titration are called standard solutions. Section 15.2

  30. Stoichiometry Revisited: Acid-Base Titrations (cont.) The endpoint is the point when the indicator used in a titration changes color, indicating that neutrality has been reached. Section 15.2

  31. Stoichiometry Revisited: Acid-Base Titrations (cont.) The volume of the standard used, the molarity of the standard, and the volume of the unknown help calculate the molarity of the unknown in a titration. Acid-base reactions are usually double displacement reactions. Section 15.2

  32. Section Assessment What qualities help calculate the molarity of the unknown in a titration? A.the volume of the standard used B.the molarity of the standard C.the volume of the unknown D.all of the above Section 15.2

  33. Section Assessment Acid-base reactions are usually what kind of reactions? A.ionic B.double displacement C.buffer D.double replacement Section 15.2

  34. End of Section 15.2

  35. Chemistry Online Study Guide Chapter Assessment Standardized Test Practice Image Bank Concepts in Motion Resources Menu

  36. Key Concepts Acid-base reactions are classified by the strength of the acid and base. Strong acid–strong base, weak acid–strong base, and weak base–strong acid are the predominant types of acid–base reactions. Acids and bases in reactions can be identified using a hydrogen-ion transfer definition. An acid is an H+ donor; a base is an H+acceptor. When acids and bases react, the pH of the final solution is dependent upon the nature of the reactants. Strong acid–strong base reactions yield neutral solutions. Weak acid–strong base reactions yield more basic solutions, whereas strong acid–weak base reactions produce acidic solutions. Study Guide 1

  37. Key Concepts A buffer is a solution that maintains a relatively constant pH when H+ions or OH– ions are added. Antacids are bases that react with stomach acid. An acid-base titration uses an acid-base reaction to determine the molarity of an unknown acid or base. Study Guide 2

  38. What type of acid-base reaction does a solution of hydrochloric acid and sodium hydroxide result in? A.strong acid + strong base B.strong acid + weak base C.weak acid + strong base D.weak acid + weak base Chapter Assessment 1

  39. An example of an ionic equation is: A.NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) B.NaOH + HCl → NaCl + H2O C.H+(aq) + OH–(aq) → H2O(l) D.H+(aq) + Cl–(aq) + Na+(aq) + OH–(aq) → Na+(aq) + Cl–(aq) + H2O(l) Chapter Assessment 2

  40. An example of a net ionic equation is: A.H+(aq) + OH–(aq) → H2O(l) B.NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l) C.NaOH + HCl → NaCl + H2O D.H+(aq) + Cl–(aq) + Na+(aq) + OH–(aq) → Na+(aq) + Cl–(aq) + H2O(l) Chapter Assessment 3

  41. Depending upon what else is present in a solution, what has the ability of acting as either an acid or a base? A.ammonia B.oxygen C.water D.salt Chapter Assessment 4

  42. Reactions that result in the transfer of a hydrogen ion require water to be present. A.true B.false Chapter Assessment 5

  43. Which reaction is not considered a predominant acid-base reaction? A.strong acid + strong base B.strong acid + weak base C.weak acid + strong base D.weak acid + weak base STP 1

  44. An acid is an H+ ___. A.donor B.acceptor C. reactor STP 2

  45. On average, the pH of human blood is: A.slightly acidic B.slightly basic C.neutral STP 3

  46. Solutions that resist changes in pH are called: A.standard solutions B.donors C.acceptors D.buffers STP 4

  47. What substance helps neutralize acid rain in lakewater? A.magnesium carbonate B.calcium carbonate C.magnesium hydroxide D.aluminum hydroxide STP 5

  48. Click on an image to enlarge. IB Menu

  49. IB 1

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