1.  Acid – a compound that produces ions when dissolved in  Examples:  Vinegar –  Lemon juice –  Tea –  Ant venom –

3.  taste   Turns litmus paper  Reacts with metals to form gas  solutions of acids are (must be mixed with water!)  Reacts with to form and

4.  Sugar, corn syrup, modified corn starch, citric acid, tartaric acid, natural and artificial flavors, yellow 5, yellow 6, red 40, blue 1  What ingredients make these… so sour?

5.  H + one other element  Begin with  Use the of the element name  Add the suffix  HCl

6.  HBr   HI   HF 

7.  H + polyatomic ion  Begin with ion without the  Add suffix if there was an  HNO 3 

8.  HClO 3   H 3 PO 3   H 2 CO 3 

9.  acids – completely in water (create a lot of )  3 binary acids  Ternary acids Strong if # of atoms - # of atoms ≥ H 2 SO 4 HNO 3

10.  acids – ionize only in solution  Binary acids – all others not listed above  Ternary acids Weak if # of atoms - # of atoms ≥ H 3 PO 3 HNO 2

11.  Base – a compound that produces ions when dissolved in  Examples:  Milk of Magnesia – neutralizes stomach acid  Drain cleaner–

12.  taste   Turns litmus paper  solutions of bases are (must be mixed with water!)  Reacts with to form and

13.  Use the same rules as for ions (name the cation, then name the anion)  NaOH   Ca(OH) 2   KOH 

14.  bases – completely in water (create a lot of ions).  All hydroxides with groups and metals (except ).  bases - only  All bases not listed above as strong.

15.  An acid must contain a and ionize in water to produce  An base must contain a and dissociates in water to produce

16.  Only compounds with can be classified as a base. What about ammonia, ?  Can only be applied to reactions that occur in  Would classify some compounds as acids, such as

17.  Classify each of the following as an Arrhenius acid (A – acid) or base (A – base).  Ca(OH) 2   HBr   H 2 SO 4   LiOH 

18.  A Bronsted – Lowry is any substance that can a  HCl + H 2 O  H 3 O + + Cl -

19.  Let’s look at the reverse reaction.  Cl - + H 3 O +  H 2 O + HCl

20.  acid – formed when a accepts a H + from an acid.  base – a that remains after an acid gives up a H +.  Conjugate acid – base pair – 2 substances related to each other by the of a single H +.

21.  Defined by how many H+ they can donate. Type# of H+ donated Example Monoprotic1HNO 3 Diprotic2H 2 SO 4 Triprotic3H 3 PO 3

22.  Identify the acid, base, conjugate acid, and conjugate base. HNO 3 + H 2 O  H 3 O + + NO 3 -

23.  Give the formula and name of the conjugate base of the following B-L acids. (After the B-L acid donates a H + )  HI   HCO 3 - 

24.  Give the formula and name of the conjugate acids of the following B-L bases. (After the B-L base accepts a H + )  H 2 PO 4 -   ClO 3 - 

25.  Water can sometimes act as a B-L acid and sometimes as a B-L base.  The of water:  H 2 O + H 2 O  H 3 O + + OH -

26.  This reaction occurs to a very small extent: = = 1 x 10 -7 M [ ] means [H+] x [OH-] = relationship

28. Neutral[H + ]=[OH - ] Acidic[H + ]>[OH - ] Basic[H + ]<[OH - ]

29.  [H + ] are often small, so the pH scale is easier to use to represent acidity and basicity.  pH range is from to  log 10 2 =  log 10 -3 =

30.  In water, a solution,= pH =

31. pH is < 7Solution is acidic pH is = 7Solution is neutral pH is > 7Solution is basic

32.  If [H 3 O + ] = 1.0 x 10 –5 M, what is the pH?  Is the solution basic, neutral, or acidic?

33.  If [H 3 O + ] = 1.0 x 10 –12 M, what is the pH?  Is the solution basic, neutral, or acidic?

34.  Given that a solution has a pH of 2.0, determine the [H 3 O + ].

35.  Similar to pH, there is also pOH.  Because [H + ] x [OH - ] =

36. [H + ] 1 pH 02 pOH 1410 [OH - ] 10 -14 10 -8 Ex. battery acid stomach acid tomatoesmilk

37. [H + ] 10 -12 pH 814 pOH 4 [OH - ] Ex. seawaterdetergentammoniaoven cleaner

38.  If [OH - ] = 1.0 x 10 –10 M, what is the pOH?  What is the pH?  Is the solution basic, neutral, or acidic?

39.  What is the pH and the pOH for 1.0 x 10 –6 M HF?  pH  pOH

40.  Given that a solution has a pH of 9.0, determine the [OH - ] and the pOH.  pOH  [OH - ]

41. AAcids LOSE H+ to become conjugate bases. TThis is a H atom. WWhen a H+ is lost from an acid, this (-) electron remains. TThe (+) proton is taken with the H. + + o o - -

42.  What is the conjugate base for the acid HBr?  HBr  H + + Br - H H Br H H + - Proton is kept by H. Electron is left by H. Conjugate base +

43. WWhat is the conjugate base for the acid HNO 2 ?  HNO 2  H + + NO 2 - H H NO 2 H H + - Proton is kept by H. Electron is left by H. Conjugate base NO 2 +

44.  What is the conjugate base for the acid HSO 3 - ?  HSO 3 -  H + + SO 3 2- H H SO 3 H H + 2- Proton is kept by H. Electron is left by H (added to the one that was there already). Conjugate base SO 3 + -

45.  Bases GAIN H+ to become conjugate bases.  What is the conjugate acid for CN - ?  CN - + H +  HCN H H CN + + - H H The + and the – cancel out in the final molecule.

46. WWhat is the conjugate acid for NH 3 ?  NH 3 + H +  NH 4 + H H NH 3 NH 3 + + H H There is no – on the NH 3 to cancel the + from H, so the final molecule is positive. NH 3 +

47.  Review:  pH = [H+] =  pOH = [OH-] =  pH + pOH =

48.  Example 1: Determine the pH of a 0.01 M HCl solution.  Example 2: Determine the pH of a 0.0010 M NaOH solution.

49.  Example 3: Determine the pH of a 0.150 M KOH solution.  Example 4: Find [H 3 O + ] for a solution that has a pH of 3.0.

50.  Example 5: Find [H 3 O + ] for a solution that has a pH of 8.2.  Example 6: Find [H 3 O + ] and pOH for a solution that has a pH of 4.85.

51.  Example 7: Find [OH - ] for a solution that has a pH of 11.2.

52.  What happens with you mix an acid with a base? A reaction  HCl + NaOH  +  Products are always a ( and ) and  This is called a reaction What happens with you mix an acid with a base? A ____________________________________________ reaction

53.  Write the balanced chemical equation for the neutralization reaction between: nitric acid and potassium hydroxide

54.  Write the balanced chemical equation for the neutralization reaction between: sulfuric acid and magnesium hydroxide

55.  Neutralization reaction:

56.  Titration – a process in which an acid-base neutralization reaction is used to determine the of a solution.

57.  1. How many mL of 0.45 M HCl acid must be added to 25.0 mL of 1.00 M KOH to make a neutral solution?

58.  2. What is the molarity of nitric acid if 15.0 mL of the solution is completely neutralized by 38.5 mL of 0.150 M NaOH?

59.  3. A 25.0 mL solution of sulfuric acid is completely neutralized by 18 mL of 1.0 M LiOH. What is the concentration of the H 2 SO 4 solution?