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5. Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce hydrogen gas. React with carbonates and bicarbonates to produce carbon dioxide gas Have a bitter taste. Feel slippery. Many soaps contain bases. Bases 5

6. þ Produce H + (as H 3 O + ) ions in water (the hydronium ion is a hydrogen ion attached to a water molecule) þ Taste sour þ Corrode metals þ Electrolytes þ React with bases to form a salt and water þ pH is less than 7 þ Turns blue litmus paper to red “Blue to Red A-CID” 6

7.  HNO 3 - nitric acid  HCl - hydrochloric acid  H 2 SO 4 - sulfuric acid  citric acid H 3 (C 6 H 5 O 7 )  acetic acid H(C 2 H 3 O 2 )  lactic acid H(C 3 H 5 O 3 ) 7

8.  Produce OH - ions in water  Taste bitter, chalky  Are electrolytes  Feel soapy, slippery  React with acids to form salts and water  pH greater than 7  Turns red litmus paper to blue “Basic Blue” 8

9. NaOHsodium hydroxidelye KOHpotassium hydroxideliquid soap Ba(OH) 2 barium hydroxidestabilizer for plastics Mg(OH) 2 magnesium hydroxide Milk of magnesia Al(OH) 3 aluminum hydroxideMaalox (antacid) Al(OH) 3 aluminum hydroxideMaalox (antacid) 9

10.  What did all of the acids on the previous screen have in common?  What did all of the bases on the previous screen have in common?  Definition #1: Arrhenius (traditional) Acids – produce H + ions (or hydronium ions H 3 O + ) Bases – produce OH - ions (problem: some bases don’t have hydroxide ions!) 10

11. Arrhenius acid is a substance that produces H + (H 3 O + ) in water Arrhenius base is a substance that produces OH - in water But: some bases don’t have hydroxide ions! Now what????? 11

12.  Definition #2:  Brønsted – Lowry Acids – proton donor Bases – proton acceptor A “proton” is really just a hydrogen atom that has lost it’s electron!

13. A Brønsted-Lowry acid is a proton donor A Brønsted-Lowry base is a proton acceptor acid conjugate base base conjugate acid 13

14. The Brønsted definition means NH 3 is a BASE in water — and water is itself an ACID

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16. Label the acid, base, conjugate acid, and conjugate base in each reaction: HCl + OH -  Cl - + H 2 O H 2 O + H 2 SO 4  HSO 4 - + H 3 O + 16

17. Lewis acid - a substance that accepts an electron pair Lewis base - a substance that donates an electron pair Definition #3 – Lewis

18. Formation of hydronium ion is also an excellent example. Electron pair of the new O-H bond originates on the Lewis base.Electron pair of the new O-H bond originates on the Lewis base. 18

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20. Example: If [H + ] = 1 X 10 -10 pH = - log 1 X 10 -10 pH = - (- 10) pH = 10 Example: If [H + ] = 1.8 X 10 -5 pH = - log 1.8 X 10 -5 pH = - (- 4.74) pH = 4.74 pH = - log [H+] [H] is the hydrogen ion concentration 20

21. 0 7 14 21

22. Find the pH of these: 1) A 0.15 M solution of Hydrochloric acid 2) A 3.00 X 10 -7 M solution of Nitric acid 22

23.  There are several ways to test pH  Blue litmus paper (red = acid)  Red litmus paper (blue = basic)  pH paper (multi-colored)  pH meter (7 is neutral, 7 base)  Universal indicator (multi-colored)  Indicators like phenolphthalein  Natural indicators like red cabbage, radishes 23

24. Use litmus paper or pH paper  Put a stirring rod into the solution and stir.  Take the stirring rod out, and place a drop of the solution from the end of the stirring rod onto a piece of the paper  Read and record the color change. Note what the color indicates.  You should only use a small portion of the paper. You can use one piece of paper for several tests.

25.  Tests the voltage of the electrolyte  Converts the voltage to pH  Very cheap, accurate  Must be calibrated with a buffer solution

26.  Indicators are dyes that can be added that will change color in the presence of an acid or base.  Some indicators only work in a specific range of pH

27. H 2 C 2 O 4 (aq) + 2 NaOH(aq) ---> acid base Na 2 C 2 O 4 (aq) + 2 H 2 O(liq) Carry out this reaction using a TITRATION. Oxalic acid, H 2 C 2 O 4 27

28. Setup for titrating an acid with a base 28

29. 1. 1. Add solution from the buret. 2. Reagent (base) reacts with compound (acid) in solution in the flask. 3. Indicator shows when exact stoichiometric reaction has occurred. (Acid = Base) This is called NEUTRALIZATION.

30. But how much water do we add? 30

31. How much water is added? The important point is that ---> moles of NaOH in ORIGINAL solution = moles of NaOH in FINAL solution moles of NaOH in FINAL solution 31

32. Amount of NaOH in original solution = M V = (3.0 mol/L)(0.050 L) = 0.15 mol NaOH Amount of NaOH in final solution must also = 0.15 mol NaOH Volume of final solution = (0.15 mol NaOH)(1 L/0.50 mol) = 0.30 L or 300 mL 32

33. Conclusion:. add 250 mL of water to 50.0 mL of 3.0 M NaOH to make 300 mL of 0.50 M NaOH. 33

34. A shortcut M 1 V 1 = M 2 V 2 34

35.  You have a stock bottle of hydrochloric acid, which is 12.1 M. You need 400 mL of 0.10 M HCl. How much of the acid and how much water will you need? 35