1. Indicators and Buffers

2. Indicators  Indicators are a substance that change color in the presence of (whatever they check for)  They do this because of Le Châtelier’s principle. All you need an equilibrium reaction with different colored products and reactants.  The pen used to check for counterfeit money is a starch indicator

3. How an acid base indicator works  A generic indicator will follow this reaction, HId is the reactant indicator, and Id - is its product  HId + H 2 O H 3 O + + Id -  The color differences are important  in an acidic solution (high H 3 O + ) you see reactant  HId + H 2 O H 3 O + + Id -  in a basic solution (low H 3 O + ) you see product  HId + H 2 O H 3 O + + Id -

4. Acid Base indicators  Acid base indicators change color at certain pH levels  They don’t have to change at 7 (most don’t)  Universal indicator solution (phenolphthalein, bromthymol blue and methyl red dissolved in ethanol and water) changes color at each integral pH value

5. Other pH indicators  Litmus and phenolphthalein are indicators  Red cabbage has a pigment that changes colors at different pH values

6. Buffers  Buffers are solutions that don’t change in pH when acids or bases are added.  They use weak acids/bases and Le Châtelier’s principle.  WA = weak acid  HWA + H 2 O  H 3 O + + WA -

7. How?  pH is determined by the concentration of H 3 O +  Concentration is measured by mol /L  Moles of H 3 O + / L (primarily of) H 2 O

8. What it does  adding H 3 O + forces the equation to the left  so the [H 3 O + ] remains constant  removing H 3 O + (adding OH - ) forces the equation to the right  so the [H 3 O + ] remains constant  There is a breaking point where the pH will change.

9. What does this have to do with my life?  Your blood is a buffered solution  The pH must remain between 7.35-7.45  Outside of that range can kill you  below this range is called acidosis  above is called alkalosis

10. homework  Read section 10.5  Pg 354-358  Questions 26-30; 97-100