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pH and Acid Rain
 

pH and Acid Rain

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    pH and Acid Rain pH and Acid Rain Presentation Transcript

    • pH and Acid Rain Mr. Wasley Earth Science
    • pH and Acid Rain
      • We use pH for many things
        • Health factors
        • Water quality of lakes, rivers, and the ocean
        • Acid rain affects wildlife and building structures
    •  
    •  
    • Clickers!!!!
      • Make sure you have the correct clicker
      • DO NOT press the channel button or the question mark button
    • Did you have breakfast this morning?
      • Yes
      • No
      0
    • You understand clickers now? Good! Now let’s see how well you know pH and acid rain!!! Keep score of how many questions you answers correctly.
    • 1. pH runs on a scale from…
      • 1-14
      • 0-14
      • 1-10
      • 0-100
      Mean = 1.4286 0
    • 2. Which of the following is NOT acidic?
      • Lemon juice
      • Milk
      • Rain
      • Blood
      • Soda
      Mean = 2.8095 0
    • 3. Which of the following describes how something basic tastes?
      • Chalky or bitter
      • Sweet and sour
      • Salty
      • Delicious
      0 Mean = 1.8095
    • 4. Something with a pH of 3 is…
      • Acidic
      • Basic
      • Neutral
      Mean = 2 0
    • 5. pH stands for…
      • Pride of Howard
      • Point of Helium
      • Power of Hydrogen
      • Pokemon Hunger
      0 Mean = 2.7143
    • 6. A solution with a pH of 3 is ____ times as acidic as a pH of 5.
      • 10
      • 20
      • 100
      • 1000
      0 Mean = 2.25
    • How did you do?
      • Figure out your score
      • Get ready to take notes
      • There will be another assessment at the end of this discussion that will count for a grade.
    • What’s pH?
      • Means “power of hydrogen”
      • pH range= 0-14
      • You can only find the pH of a solution- liquid only
      Acidic H+ Examples: HCl H 2 SO 4 Neutral H 2 O Basic OH - Examples: KOH NaOH 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
    • Acid Base HCl 0 NaOH 14 Drano ® 13 Mineral lime - Ca(OH) 2 12 Ammonia 11 Tums ® antacid 10 Baking Soda 9 Egg whites 8 Pure water 7 Milk 6 Rain water 5 Soda 4 Vinegar 3 Lemon Juice 2 Stomach acid 1 Example pH
    • pH Continued
      • pH indicates the acidity of a solution
      • pH= -log[H 3 O] +
      • Each numeric change in pH represents a factor of 10
      • Example: pH of 4 is 100 times more acidic as a pH of 6
      • Example: Stomach acid is 1000 times more acidic than soda
    • Ionization in water
      • Occasionally, a H+ is transferred between H 2 O molecules
      O O O O H H H H H H H H H 2 O OH - Hydroxide Ion (-) H 3 O + Hydronium ion (+) H 2 O Which ion is an acid? Which ion is a base? Donors Acceptors
    • Pure Water is Neutral
      • Pure water contains small, but equal amounts of H 3 O + and OH -
      H 3 O + OH -
    • Acids
      • Produce H + (as H 3 O + ) ions in water
      • Tastes sour
      • Corrode metals
      • More H 3 O + than H 2 O
      • As H 3 O + increase OH - decreases
      H 3 O + OH -
    • Bases
      • Produces OH- ions in water
      • Tastes bitter, chalky
      • Are electrolytes
      • Blood and salt water are basic
      • Feels soapy, slippery
      • More OH- than H2O
      • As OH - increases, H 3 O + decreases
      OH - H 3 O +
    • Neutralization
      • The neutralization reaction of an acid with a base will always produce water and a salt, as shown below:
      • Acid Base Water Salt
      • HCl + NaOH H 2 O + NaCl
      • HBr + KOH H 2 O + KBr
    • Buffer Solutions
      • Occurs when a buffer agent is dissolved in water
      • the resulting buffer solution includes both acid and base forms of the buffer
      • resists pH changes when exposed to other acids and bases
      • Very useful for keeping a solution balanced such as the ocean
    • Buffer Solution Continued
      • Example : In the human body, buffer agents play a vital role in both respiration and maintaining the body’s pH level. One of the most important buffer agents in humans is carbon dioxide . When carbon dioxide (CO 2 ) mixes with water (H 2 O) in the blood, carbonic acid is formed (H 2 CO 3 ), and bicarbonate (HCO 3 - ) (the base form) is also created. Carbonic acid and bicarbonate are in equilibrium in the blood, helping the body adjust to pH changes
    • Get those clickers ready!
      • Use your notes for these questions
      • Let’s see how we can improve as a class!
    • 1. pH runs on a scale from…
      • 1-14
      • 0-14
      • 1-10
      • 0-100
      Mean = 1.9048 0
    • 2. Which of the following is NOT acidic?
      • Lemon juice
      • Milk
      • Rain
      • Blood
      • Soda
      Mean = 3.85 0
    • 3. Which of the following describes how something basic tastes?
      • Chalky or bitter
      • Sweet and sour
      • Salty
      • Delicious
      0 Mean = 1
    • 4. Something with a pH of 3 is…
      • Acidic
      • Basic
      • Neutral
      Mean = 1.0476 0
    • 5. pH stands for…
      • Pride of Howard
      • Point of Helium
      • Power of Hydrogen
      • Pokemon Hunger
      0 Mean = 2.9524
    • 6. A solution with a pH of 3 is ____ times as acidic as a pH of 5.
      • 10
      • 20
      • 100
      • 1000
      5 Mean =
    • A pH of 2 is ___ times more acidic than a pH of 5
      • 10
      • 30
      • 100
      • 1000
    • Which of the following is not an acid?
      • HCl
      • H 2 SO 4
      • HNO 3
      • KOH
      • H 2 CO 3
    • Which of the following is a hydroxide ion
      • H 3 O
      • H 2 O
      • OH
      • H +