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Comprehensive Overview of Acid-Base Chemistry: Concepts, Properties, and Titration Techniques

This guide serves as a thorough review of acid-base chemistry, focusing on the characteristics and naming of acids and bases, their properties, and the neutralization reactions that occur between them. It covers the pH scale, calculation methods, and the use of titration to determine the molarity of unknown solutions. Key concepts, including ionization, strong acids and bases, and various methods for measuring pH, are presented, alongside practical tips for conducting experiments. Perfect for students seeking to deepen their understanding of acid-base interactions.

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Comprehensive Overview of Acid-Base Chemistry: Concepts, Properties, and Titration Techniques

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Presentation Transcript

  1. Day 1 Acid-Base

  2. Review of naming acids

  3. Characteristics of Acids & Bases

  4. Acids are Characterized by: • Sour taste •  color of indicator • Release of H2 gas • Reacts with bases  salt( ionic compound) & H2O

  5. Bases are Characterized by: • Bitter taste • Feels slippery •  color of indicator • Reacts with acid  salt( ionic compound) & H2O • Conducts electric current ( its an ionic compound)

  6. What does ionization mean?

  7. Ionization • Adding or removing electrons (e-) • Making a cation or anion

  8. Strong Acids • Ionizes completely = breaks up completely • Conducts electric current (remember electrolyte demo & PhET)

  9. Strong Acids Examples: • Hydrochloric Acid (HCl) • Sulfuric Acid (H2SO4) • Nitric Acid (HNO3)

  10. Strong Base • Ionizes completely = breaks up completely • Examples: group 1 hydroxides – sodium hydroxide, potassium hydroxide, etc.

  11. Neutralization Reaction HCl + NaOH NaCl + HOH Strong + Strong  Salt + Water Acid Base HNO3 + KOH  KNO3 + HOH

  12. Neutralization Reaction Is a double replacement rxn b/w … strong acid + strong base a salt (ionic compound) + water

  13. pH Scale Determining strength of an Acid or Base

  14. pH scale 0-14 • neutral pH = 7.0 • acidic pH <7.0 • basic pH > 7.0

  15. pH Scale

  16. Calculating pH & [H+] pH = -log[H+] Inverse of log10 is 10^( ) [H+] = 10^(-pH)

  17. Calculating pOH & [OH-] pH = -log[OH-] Inverse of log10 is 10^( ) [OH-] = 10^(-pOH)

  18. Relationship between pH & pOH pH + pOH = 14

  19. Now you try…

  20. Answer

  21. Try on your own…

  22. Try on your own…

  23. Practice

  24. Now you try

  25. Answer

  26. Try on your own..

  27. Answers

  28. Other methods of determining pH

  29. If molarity is not known, pH can be determined by… • Acid-Base Indicators • pH meter • Titration

  30. Indicator Solutions • Change color depending on pH of test solution

  31. Indicators

  32. Indicators

  33. Indicators

  34. Problems with indicator solutions: • If you have a colored solution • Approx pH value not exact • Temperature affects color 

  35. pH meter

  36. pH meter • consists of a measuring probe • electronic meter: measures & displays the pH reading • have to calibrate probe

  37. Titration • Use Buret, Erlenmeyer flask, indicator • Use M1V1 = M2V2 to determine molarity of unknown

  38. Titration

  39. Titration

  40. Answer the following questions while watching the video clips: • Where do you read/How do you read a burette? • What hand do you use to swirl the Erlenmeyer flask? • What hand do use to adjust the burette? • When do you know you are getting close to the endpoint? • How is the standard solution added as you get close to the endpoint? • When do you know you have achieved the endpoint?

  41. Titration Video Clip #1 (3:15) • Titration Video Clip # 2 ( 6:07)

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