1. Acids vs. Bases

2. What is pH? Parts of Hydrogen ions (H+)
More H+  lower the pH = very acidic
Few H+  higher the pH = very basic

3. The pH Scale 0 - 4 = strong acid 4.01 – 6.99 = weak acid 7 = neutral
7.01 – 10 = weak base
10.01 – 14 = strong base

4. Acids Release H+ into water pH 0 – 6.99 Taste Sour
Corrosive to Metals (eats them away)
Eat away at stones / buildings / statues

6. Examples pH of 1 -- Hydrochloric Acid / Battery acid
pH of Stomach Acid
pH of 3 – Lemon Juice
pH of 4 – Tomatoes / Acid rain
pH of 5 – Regular Rain
pH of 6 – Milk

7. Bases Release OH- into water pH 7.01 – 14 Taste Bitter
Slippery feeling
Corrosive to flesh (eats away skin)

8. Examples pH of 8 -- Ocean Water pH of 10 – antacids (tums, etc)
pH of 11 – Cleaners
pH of 12 – Baking soda
pH of 13 – Bleach
pH of 14 – Drain Cleaner / NaOH

9. Neutral pH of 7 Only pure H2O (distilled or de-ionized)
Tap water does not have neutral pH

10. To Bring solution to pH of 7
Neutralization
To Bring solution to pH of 7
What is needed to neutralize a basic solution?
What is needed to neutralize an acidic solution?

11. Example
John has a glass of orange juice. Which of the following would help raise its pH to 7?
Milk
Rain Water
Bleach
Sulfuric Acid

12. Real World Neutralization
Acid Rain lowers pH of a lake to 4.5
Most fish, plants and animals die at this pH
(all fish die at 4.2 or lower)
pH needs to be between 5 – 8 for
How do we do raise the pH of a lake to acceptable levels for life?

13. As rain water becomes more acidic what happens to its pH?
The pH increases
The pH decreases
The pH stays the same
It turns into lemonade!

14. Acid Rain Definition – rain with a pH below 5 Causes of Acid Rain
– Sulfur (SO2 , SO4, H2S) from pollution
dissolves into rain water
- burning fossil fuels (coal, oil, gasoline, diesel, etc.)
- volcanic activity
- Factory pollution
- More SO2 = lower pH = more damage
- Affects of CO2 can also lower pH