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Water

Water. The chemical of life. Acids. Acids Sour taste, leaves burning sensation Increase hydrogen ions (H+) in solution. Acids. Acids Sour taste, leaves burning sensation Increase hydrogen ions (H+) in solution. Acids. Acids Sour taste, leaves burning sensation

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Water

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  1. Water The chemical of life

  2. Acids • Acids • Sour taste, leaves burningsensation • Increase hydrogen ions (H+) in solution

  3. Acids • Acids • Sour taste, leaves burningsensation • Increase hydrogen ions (H+) in solution

  4. Acids • Acids • Sour taste, leaves burningsensation • Increase hydrogen ions (H+) in solution

  5. Acids • Acids • Sour taste, leaves burningsensation • Increase hydrogen ions (H+) in solution

  6. Acids • Example: HClH+ + Cl- • Turns litmus (pH) paper to red

  7. Acids • Example: HClH+ + Cl- • Turns litmus (pH) paper to red

  8. Acids • Example: HClH+ + Cl- • Turns litmus (pH) paper to red

  9. Acids • Example: HClH+ + Cl- • Turns litmus (pH) paper to red

  10. Acids • Example: HClH+ + Cl- • Turns litmus (pH) paper to red

  11. Bases • Sharp bitter taste, feels slippery to touch • Decrease hydrogen ions (H+) in solution(Increase hydroxide ions (OH-) in solution

  12. Bases • Sharp bitter taste, feels slippery to touch • Decrease hydrogen ions (H+) in solution(Increase hydroxide ions (OH-) in solution

  13. Bases • Sharp bitter taste, feels slippery to touch • Decrease hydrogen ions (H+) in solution(Increase hydroxide ions (OH-) in solution

  14. Bases • Sharp bitter taste, feels slippery to touch • Decrease hydrogen ions (H+) in solution(Increase hydroxide ions (OH-) in solution

  15. Bases • Example: NaOHNa+ + OH- • Turns litmus (pH) paper to blue

  16. Bases • Example: NaOHNa+ + OH- • Turns litmus (pH) paper to blue

  17. Bases • Example: NaOHNa+ + OH- • Turns litmus (pH) paper to blue

  18. Bases • Example: NaOHNa+ + OH- • Turns litmus (pH) paper to blue

  19. The PH Scale • The pH Scale is a measurementof how acidic or how basic a solution is. • The scale goes from 0to 14.

  20. The PH Scale • The pH Scale is a measurementof how acidic or how basic a solution is. • The scale goes from 0to 14.

  21. The PH Scale • The pH Scale is a measurementof how acidic or how basic a solution is. • The scale goes from 0to 14.

  22. The PH Scale • The pH Scale is a measurementof how acidic or how basic a solution is. • The scale goes from 0to 14.

  23. The PH Scale • The pH Scale is a measurementof how acidic or how basic a solution is. • The scale goes from 0to 14.

  24. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  25. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  26. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  27. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  28. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  29. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  30. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  31. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  32. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  33. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  34. The PH Scale • Compounds are acidic if they have a pH lower than 7. • Compounds with a pH higher than 7 are basic or alkaline. • Compounds with a pH of 7, are neutral.

  35. Buffers • A buffer is a weakacidor base that prevents sudden changes in pH. • Maintains homeostasis

  36. Buffers • A buffer works by binding to H+ ions releasing H+ ions when the solution pH changes.

  37. Buffers • A buffer works by binding to H+ ions releasing H+ ions when the solution pH changes.

  38. Buffers • A buffer works by binding to H+ ions releasing H+ ions when the solution pH changes.

  39. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  40. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  41. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  42. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  43. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  44. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  45. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  46. Buffers • Buffers bind to H+ ions when the concentration of H= ions in solution increases. • NaOHNa+ + OH-(The OH- will bind to H+ ions to form H2O – neutralization)

  47. Buffers • Buffers release H+ ions when the concentration of H= ions in solution decreases.HClH+ + Cl-

  48. Buffers • Buffers release H+ ions when the concentration of H= ions in solution decreases.HClH+ + Cl-

  49. Buffers • Buffers release H+ ions when the concentration of H= ions in solution decreases.HClH+ + Cl-

  50. Buffers • Buffers release H+ ions when the concentration of H= ions in solution decreases.HClH+ + Cl-

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