1. 1 Dr. Marwa Eid

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5.  An acid is a solution that has an excess of H + (hydrogen ion).  The more H + ions, the more acidic the solution.

6. Vinegar (acetic or ethanoic acid) Citric Acid 6

7. 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” 7

8. LecturePLUS Timberlake 8 HCl hydrochloric acid HNO 3 nitric acid H 3 PO 4 phosphor ic acid H 2 SO 4 sulfur ic acid CH 3 COOH acet ic acid

9.  Acetic Acid = Vinegar  Citric Acid = lemons, limes, & oranges.  It is in many sour candies such as lemonhead & sour patch.  Ascorbic acid = Vitamin C which your body needs to function.  Sulfuric acid is used in the production of fertilizers, steel, paints, plastics & Car batteries

10.  -A base is a solution that has an excess of OH - ions.  -Another word for base is alkali.  -Your blood is a basic solution.

11. Ammonia 11

12.  Produce OH - ions in water  Taste bitter, chalky  Electrolytes  Feel soapy  React with acids to form salts and water  pH greater than 7  Turns red litmus paper to blue “Basic Blue” 12

13.  Sodium Hydroxide NaOH  Potassium HydroxideKOH  Magnesium HydroxideMg(OH) 2  AmmoniaNH 3 13

14.  -Bases give soaps, ammonia, and many other cleaning products some of their useful properties.

15. LecturePLUS Timberlake 15 Acid, Base Name or Salt CaCl 2 _______________________ KOH_______________________ Ba(OH) 2 ______ _________________ HBr_______________________ H 2 SO 4 ________________________

16. LecturePLUS Timberlake 16 cid, Base Name or CaCl 2 saltcalcium chloride KOHbasepotassiuim hydroxide Ba(OH) 2 basebarium hydroxide HBracidhydrobromic acid H 2 SO 4 acidsulfuric acid

17.  pH is a measure of how acidic or basic a solution is. The pH scale ranges from 0 to 14.  Acidic solutions have pH values below 7  A solution with a pH of 0 is very acidic.  A solution with a pH of 7 is neutral. Pure water has a pH of 7. Basic solutions have pH values above 7.

18. pH Scale

19.  A reaction between an acid and a base is called neutralization.  An acid-base mixture is not as acidic or basic as the individual starting solutions.

20. Acids:  Arrhenius acid  Arrhenius acid: Any substance that, when dissolved in water, increases the concentration of hydronium ion (H 3 O + )  Bronsted-Lowry acid  Bronsted-Lowry acid: A proton donor  Lewis acid  Lewis acid: An electron acceptor Bases:  Arrhenius base  Arrhenius base: Any substance that, when dissolved in water, increases the concentration of hydroxide ion (OH - )  Bronsted-Lowery base  Bronsted-Lowery base: A proton acceptor  Lewis base  Lewis base: An electron donor 20

21. Arrhenius acid Arrhenius acid: Any substance that, when dissolved in water, increases the concentration of hydronium ion (H 3 O + )  Acids produce hydrogen ions (H + ) in an aqueous solution, while bases produce hydroxide ion (OH - ). Acid: HCl (aq)  Cl - (aq) + H + (aq) Base: NaOH(aq)  Na + (aq) + OH - (aq) 21

22. Arrhenius acid is a substance that produces H + (H 3 O + ) in water Arrhenius base is a substance that produces OH - in water 4.3 Acid/Base definitions Definition 1: Arrhenius 22

23. Number of Ionizable Hydrogens Monoprotic1 Diprotic2 Triprotic3 23

24.  One ionizable proton: HCl → H + + Cl -  Two ionizable protons: H 2 SO 4 → H + + HSO 4 - HSO 4 - → H + + SO 4 2-  Three ionizable protons: H 3 PO 4 → H + + H 2 PO 4 – H 2 PO 4 - → H + + HPO 4 2- HPO 4 2- → H + + PO 4 -3 Combined: H 2 SO 4 → 2H + + SO 4 2- Combined: H 3 PO 4 → 3H + + PO 4 3- 24

25. Bronsted Theory of Acids & Bases Conjugate Acid-Base Pairs General Equation An acid is a proton (H + ) donor. A base is a proton (H + ) acceptor. 25

26.  Example: HF + H 2 O  H 3 O + + F - AcidBase H 3 O + : hydronium ion 26

27. Lone Hydrogen ions do not exist by themselves in solution. H+ is always bound to a water molecule to form a hydronium ion 27

28.  General expression: HA (aq) + H 2 O (l)  H 3 O + (aq) + A - (aq) Acid Base Conjugate Conjugate AcidBase 28

29.  Conjugate acid is the particle formed that has received the proton. (ex: H 3 O + )  Conjugate base is the particle left from the acid once it has donated the proton. 29 Note: Water acts as an acid and as a base. It is amphoteric.

30. NH 3 (aq) + H 2 O (l)  NH 4 + (aq) + OH - (aq) Base Acid Conjugate Conjugate Acid Base 30

31.  An acid accepts a pair of electrons.  A base donates a pair of electrons.  This is a more general definition than the previous two. 31

32. :NH 3 + H +  NH 4 + 32

33. ModelDefinition of Acid Definition of Base ArrheniusH + producerOH - producer Bronsted-LowryH + donorH + acceptor LewisElectron-pair acceptor Electron-pair donor 33

34. ELECTROLYTES Electrolytes are species which conducts electricity when dissolved in water. Acids, Bases, and Salts are all electrolytes. Salts and strong Acids or Bases form Strong Electrolytes. They are fully dissociated, available to conduct electricity. HCl (s) + H 2 O  H 3 O + + Cl - Weak Acids and Weak Bases form Weak Electrolytes. Weak electrolytes have less ions available to conduct electricity. NH 3 + H 2 O  NH 4 + + OH - 34

35. 35 Strong and Weak Acids/Bases STRONG ACID: HNO 3 (aq) + H 2 O (l)  H 3 O + (aq) + NO 3 - (aq)

36.  Weak acids are much less than 100% ionized in water. *One of the best known is acetic acid = CH 3 CO 2 H and ammonia *One of the best known is acetic acid = CH 3 CO 2 H and ammonia NH 3 (aq) + H 2 O (l) ↔ NH 4 + (aq) + OH - (aq) NH 3 (aq) + H 2 O (l) ↔ NH 4 + (aq) + OH - (aq) Strong and Weak Acids/Bases 36

37.  Strong Base: 100% dissociated in water. NaOH (aq)  Na + (aq) + OH - (aq) NaOH (aq)  Na + (aq) + OH - (aq) Other common strong bases include KOH and Ca(OH)2. CaO (lime) + H 2 O --> Ca(OH) 2 (slaked lime) Ca(OH) 2 (slaked lime) CaO Strong and Weak Acids/Bases Strong bases are the group I hydroxides Calcium, strontium, and barium hydroxides are strong, but only soluble in water to 0.01 M 37

38. WEAK BASES 38

39. ACIDS & BASES STRONG vs WEAK STRONG vs WEAK _ completely ionized_ partially ionized _ strong electrolyte_ weak electrolyte _ ionic/very polar bonds_ some covalent bonds Strong Acids : Strong Bases: HClO 4 LiOH H 2 SO 4 NaOH HIKOH HBrCa(OH) 2 HClSr(OH) 2 HNO 3 Ba(OH) 2 39

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