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Acids and Bases

Acids and Bases. http://www.emsb.qc.ca/laurenhill/science/bronsted_cartoon.gif. Why are they important?. They are found on the Earth you walk, the foods you eat and the products that you, not to mention who important your amino acids are

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Acids and Bases

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  1. Acids and Bases http://www.emsb.qc.ca/laurenhill/science/bronsted_cartoon.gif

  2. Why are they important? • They are found on the Earth you walk, the foods you eat and the products that you, not to mention who important your amino acids are • These two flowers are the same species. Why are the different colors? • Their color depends on the acidity of the soil that they are grown in http://www.profizahrada.cz/images_data/3170-hydrangea-macrophylla-bailmer-1.jpg

  3. Taste

  4. The pH Scale • The measurement of H+ (acid) • pOH = measure of OH-(base) ions. • Lots of H+ = Acid • Lots of OH- = Base

  5. pH + pOH = 14 • What is the pH of a solution that has a pOH of 9? • Substute in • pH + 9 = 14 • pH = 5

  6. Think you’ve got it?

  7. The Basic Formula • Acid + Base  Salt + Water HA + BOH  BA + H2O • What is a salt again? • General way to describe an ionic bond • Acid and base reactions can happen forward and backwards

  8. Acids • contain H+ (proton) • Sour in taste • Strong Vs. Weak • Strong = pH 1-4 (molecule will break apart) • Weak = pH 3-6 ( only some molecule will) • Example: • HCl  H+ + Cl-

  9. Bases • Contain OH- • Alkaline • Strong Vs. Weak • Strong = pH 10-14 • Weak = pH 8-10 (only some break apart)

  10. Neutral • pH = 7 • Neutraization • When acids and bases are mixed • Antacid • Stomach acid + antacid = neutralized stomach • Let’s visit The Alien Juice Bar

  11. BAAD Acronym • Bases Accept protons (H+) • Acids Donate protons(H+)

  12. Progress Check

  13. Solution stoichiometry • Concentration • [ } = concentration in moles/ literpH = -log [H+] pH scale • Reactions with solutionNeutralization reaction

  14. 10.0 ml of 1.5 M HCl solution neutralizes a 30.0 ml sample Ca(OH)2. What is the concentration (M) of the Ca(OH)2 solution? • First step = Balance the Equation • 2 HCl + Ca(OH)2  CaCl2 + 2H2O • Next start w/ given and follow units until unknown  .01 L x 1.5 M HCl x 1 moles Ca(OH)2 1 L 2 moles HCl = .0075M Ca(OH)2 *  .0075 M Ca(OH)2= .25M  .03L

  15.  15.9 ml of 2.50M Al(OH)3 solution is used to neutralized a 25.0 ml sample of H2SO4 . Calculate the molarity of H2SO4 Solution. • First, balance the equation • 2Al(OH)3 + 3H2SO4 Al2(SO4)3 + 6H2O • Next, start w/ given and follow units until unknown •  .159L x 2.50moles Al(OH)2 x 3 moles H2SO4 1L 2moles Al(OH)2 = .6M H2SO4 • .6 M H2SO4 = 24M .025L

  16. Indicators • Indicates pH • Change colors at different pH Levels • Types • Universal • Phenolphthalein   Clear  Pink  Magenta  * For our lab we went to stop at pink

  17. Cabbage Indicator

  18. pH calculations • pH = measure of H

  19. Buffers • Resist change to pH • Example • Holding your breath will build up the concentration of CO2 in your body. • That changes the pH in your blood • Exhaling the CO2 changes the pH back to normal

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