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Understanding pH and Indicators in Chemistry

Learn about pH scale, neutral, acidic, and basic solutions, ionization of water, calculation of pH, Soren Sorensen's pH concept, and the role of indicators in indicating acidity or basicity.

derek-cohen
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Understanding pH and Indicators in Chemistry

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  1. pH and Indicators Chemistry Mrs. Coyle

  2. Basic14>ph>7 Neutral ph=7 Acidic 1<pH<7

  3. Self Ionization of H2O H2O  H+ (aq) + OH- (aq) Ion Product ConstantK wfor Water: Kw= [H+ ] x [OH-] =1.0 x 10 -14

  4. For pure H2O [H+ ] = [OH-] = 1.0 x 10-7M

  5. pH • 1909 Soren Sorensen (Danish) pH=-log[H+] What is the pH of pure water?

  6. Ex 1: Find the pH for [H+]=10-3M • Answer: pH=3

  7. Ex 2: Find the pH for [H+]=5x10-3M • Answer: pH=2.3

  8. Finding [H+] from pH • [H+]= 10-pH

  9. Ex 3: Find the [H+] for pH=5 • Answer: [H+] = 10-5 M

  10. Ex 4: Find the [H+] for pH=5.8 • [H+]= 10-pH • Answer: [H+] = 1.6x10-6 M

  11. pOH pH=-log[H+] pH + pOH=14

  12. Basic(Alkaline)Solutions Neutral Solutions Acidic Solutions

  13. Acids Change phenolphthalein to colorless.

  14. Acids • Turn litmus paper from blue to red.

  15. Bases Change phenolphthalein to pink.

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