1. Indicators

2. Weak acids and bases can act as an indicator  can be forced the other way  So ammonia…  NH 3 + H 2 O NH 4 + +OH -  Ammonia is a gas with a distinct odor  Ammonium and hydroxide are both odorless.  If base is added to the solution you will smell ammonia, if hydroxide is removed you won’t.

3. Pet Stain Problem  Urine has ammonia in it.  Most cleansers are basic  NH 3 + H 2 O ⇌ NH 4 + +OH -  If I stress this equilibrium by adding a base…  It shifts to the left causing more ammonia to form. Animals sense of smell is better so they fine the same spot and mark it again.  That is why there are special cleansers (acidic) for pet stains

4. 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

5. 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 -

6. 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

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

8. 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 -

9. 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

10. What it does  adding H 3 O + should increase [H 3 O + ]  However, this forces the equation to the left, decreasing H 3 O + and increasing H 2 O  so the [H 3 O + ] remains constant  Removing H 3 O + (adding a base) should decrease [H 3 O + ]  However, this forces the equation to the right, increasing H 3 O + and decreasing H 2 O  So again, there is no change to [H 3 O + ]  There is a breaking point where the pH will change.

11. 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

12. Buffered Products  medications (Bufferin)  Shampoos, body soaps  All are buffered to be near your body pH so they won’t cause a major disruption.