1. The Acid Test Acids, Bases, and pH

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3. QOD How many neutrons are found in an atom of 42 Ca? What are the atoms of the same element with different masses called? What is the reason for this difference in mass?

4. 1. What is pH?  pH measures acidity and alkalinity (how basic) a liquid is*

5. 2. Describe the pH Scale The next few slides will illustrate this point. Be sure to write small and get it all!

6. Range of pH scale The pH scale ranges from 0 to 14. There are no units of measure for pH *

7. pH Range 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Neutral [H + ] > [OH - ] [H + ] = [OH - ] [OH - ] > [H + ] Acidic Basic

8. Learning Check pH7 Identify each solution as 1. acidic 2. basic3. neutral A. _____ HCl with a pH = 1.5 B. _____ Pancreatic fluid pH = 8 C. _____ Sprite soft drink pH = 3.0 D. _____ pH = 7.0 E. _____ pH = 3 F. _____ pH = 12

9. Solution pH7 Identify each solution as 1. acidic 2. basic3. neutral A. _1__ HCl with a pH = 1.5 B. _2__ Pancreatic fluid pH = 8 C. _1__ Sprite soft drink pH = 3.0 D. _3__ pH = 7.0 E. _1__ pH = 3 F. _2__ pH = 12

10. 3. What is a hydronium ion? Occasionally, in water, a H + is transferred between H 2 O molecules........ H : O : + : O : H H : O : H + + : O : H -........ H H H water molecules hydronium hydroxide ion (+) ion (-)

11. 4. How can the pH of a solution be determined? There will be several slides showing various ways to measure pH. Be sure to get them all!

12. Litmus paper Litmus paper cannot tell you the exact pH of a substance. It can only tell you if it is an acid or a base Blue litmus turns pink in the presence of an acid Red litmus turns blue in the presence of a base*

13. pH paper pH paper can tell you approximate pH values. By placing one end of the pH paper in the solution it will turn a color which can be matched to the color code key. *

14. Indicators Indicators: Weak organic acids and bases whose colors differ from the colors of their conjugate acids or bases. The color is best viewed from above against a white background

15. Table of Indicators Acid / Base Indicators IndicatorLower ColorpH RangeUpper Color methyl violetyellow-green0.0 - 2.5violet methyl orangered2.5 - 4.4yellow congo redblue3.0 - 5.0red bromocresol greenyellow4.5 - 5.5blue methyl redred4.8 - 6.0yellow bromocresol purpleyellow-green5.4 - 6.8violet bromothymol blueyellow6.0 - 7.6blue phenol redyellow6.4 - 8.2red-violet cresol redyellow7.1 - 8.8violet phenolphthaleincolorless8.3 - 10.0dark pink Phenolphthalein is a common indicator to use in neutralization titrations. The solution is considered neutral when the solution holds a very faint pink color for half a minute or more. alizarin yellow Ryellow9.9 - 11.8dark orange

16. pH Meter  The most precise and usually more accurate way to measure pH is using a pH meter which directly measures the amount of [H 3 O + ] in the solution

17.  Uses an electrode which specifically measures the pH of the solution.  This is a larger model. Some are small enough to be hand-held.*

18. WRITE THE QUESTION AND ANSWER. * Now Complete the HW--P. 263 #4, 5, & 6

19. 5. What are the properties of an acid? Acids Taste sour Donate a H + pH less than 7 Turn litmus paper red Turn bromothymol blue to yellow Turn phenolphthalein colorless Neutralize bases

20. 6. What are the properties of bases? Bases Taste bitter Usually ends in -OH pH greater than 7 Turn litmus paper blue Turn bromothymol blue to blue Turn phenolphthalein pink Feel slippery to touch Neutralize acids*

21. Learning Check AB2 Identify each as characteristic of an A) acid or B) base ____ 1. Sour taste ____ 2. Produces OH - in aqueous solutions ____ 3. Chalky taste ____ 4. Is an electrolyte ____ 5. Produces H + in aqueous solutions*

22. Solution AB2 Identify each as a characteristic of an A) acid or B) base A_ 1. Sour taste _B_ 2. Produces OH - in aqueous solutions _B_ 3. Chalky taste A, B 4. Is an electrolyte _A_ 5. Produces H + in aqueous solutions*

23. Question of the Day Describe the solution in each of the following as: 1) acid 2) base or 3)neutral. A. ___soda B. ___soap C. ___coffee D. ___ wine E. ___ water F. ___ grapefruit* G. ___ rain H. ___ vinegar I. ___ saliva J.___ salt water K.___ ketchup L.___ dishwashing detergent

24. Answers of the Day Describe each solution as: 1) acid 2) base or 3) neutral. A. _1_ soda B. _2_ soap C. _1_ coffee D. _1_ wine E. _3_ water F. _1_ grapefruit* G. _1__ rain H. _1__ vinegar I. __1_ saliva (depends on what you ate recently) J._3__ salt water K.__1_ ketchup L._2__ dishwashing detergent

25. 7. What compounds are formed when an acid reacts with a base? When acid and bases with equal amounts of hydrogen ion H + and hydroxide ions OH - are mixed, the resulting solution is neutral. NaOH (aq) + HCl(aq) NaCl + H 2 O base acid salt water Ca(OH) 2 + 2 HCl CaCl 2 + 2H 2 O base acid salt water*

26. Learning Check N2 Select the correct group of coefficients for the following neutralization equations A. __ HCl + __ Al(OH) 3 __AlCl 3 + __ H 2 O 1) 1, 3, 3, 12) 3, 1, 1, 1 3) 3, 1, 1 3 B.__ Ba(OH) 2 + __H 3 PO 4 __Ba 3 (PO 4 ) 2 + __ H 2 O 1) 3, 2, 2, 22) 3, 2, 1, 6 3) 2, 3, 1, 6

27. Solution N2 A. 3HCl + 1Al(OH) 3 1AlCl 3 + 3H 2 O B. 3Ba(OH) 2 + 2H 3 PO 4 1Ba 3 (PO 4 ) 2 + 6H 2 O*

28. 8. Antacids A practical use of the neutralization process

29. Antacids Used to neutralize stomach acid (HCl) Many contain one or more weak bases Alka-Seltzer: NaHCO 3, citric acid, and aspirin Di-gel: CaCO 3 and Mg(OH) 2 Gelusil: Al(OH) 3 and Mg(OH) 2 Maalox: Al(OH) 3 and Mg(OH) 2 Mylanta: Al(OH) 3 and Mg(OH) 2*

30. More Antacids Milk of Magnesia: Mg(OH) 2 Rolaids: AlNa(OH) 2 CO 3 aluminum sodium dihydroxy carbonate Tums: CaCO 3 Tempo: CaCO 3, Al(OH) 3, Mg(OH) 2*

31. How much more acidic is a solution of pH 2 than a solution of pH 6? A)3 times more acidic B)10 times more acidic C)100 times more acidic D)1,000 times more acidic E)10,000 times more acidic

32. Answer E) 10,000 times more acidic Every one pH value that a solution decreases, it is 10 times more acidic Example, normal rain is about 5.5. If its pH falls to 4.5 it is now 10 times more acidic. Some industrialized areas have had pH values measured to be as low as 2.5 or 1,000 times more acidic

33. pH measures the concentration of hydrogen ion [H + ] in a solution So every time you increase one number on the pH scale the acidity (or alkalinity) increases by a power of 10! The concentration of pH = 2 solution is 4 pH values from a pH = 6 solution or The pH = 2 solution is 10,000 times more acidic than the pH = 6 solution

34. What does this mean for the environment? An in-depth look at acid rain

35. Sources of Acid Rain Power stations Oil refineries Coal with high S content Car and truck emissions Bacterial decomposition, and lighting hitting N 2*

36. Acid Rain 2. Reactions in the atmosphere form SO 3 2SO 2 + O 2  2 SO 3*

37. Acid Rain 3. Reactions with atmosphere water form acids SO 3 + H 2 O  H 2 SO 4 sulfuric acid NO + H 2 O  HNO 2 nitrous acid HNO 2 + H 2 O  HNO 3 nitric acid*

38. Acid Rain 4. Effects of Acid Rain  Decline in fish populations in rivers and lasts due to toxic effect of Al leached from soil by acid rain  Extensive fish kills in spring from runoff due to accumulation of large amounts of acid on the snow  Dissolves minerals Mg, Ca, and K from the soil and waxy coatings that protect leaves from bacteria  Corrodes metals, textiles, paper and leather*

39. Acid Rain Formation of acid rain: 1. Emission of sulfur and nitrogen oxides from the burning of fuels especially coal with high S content, power stations, oil refineries, vehicles as well as bacterial decomposition, and lighting hitting N 2 SO 2 26 million tons in 1980 NO and NO 2 22 million tons in 1980 Mt. St Helens (1980) 400,000 tons SO 2*