1 Chapter 19: Acids, Bases, pH and pOHThey are everywhere.. In your food In your house EVEN IN YOU!!!!!

2 I Can … Explain the pH scale in terms of hydrogen ion concentrationExplain the pH scale in terms of hydroxide ion concentration Explain the pH scale in terms of acidity Explain the pH scale in terms of basicity

3 An acid is… An aqueous solution that has H+ ions.The more H+ ions, the more acidic the solution. Examples of acids: HCl (H+ and Cl-), HNO3 (H+ and NO3-)

4 Properties of an Acid Tastes Sour CorrosiveTurns blue litmus paper red Picture from BBC Revision Bites

5 Some Common Acids Vinegar Citrus fruits (lemons, limes, & orangesAscorbic acid = Vitamin C which your body needs to function. Car batteries

6 A Base is .. An aqueous solution that has OH- ions. Base = alkalineExamples of Bases: NaOH (Na+ and OH-), Ca(OH)2 (Ca+2 and OH-)

7 Properties of Bases Feel Slippery Taste Bitter CorrosiveTurns red litmus paper blue.

8 pH Scale pH is a measure of how acidic or basic a solution is.Ranges from 0 to 14. Acidic solutions - pH below 7 pH of 7 is neutral. Pure water has a pH of 7 Basic solutions - pH above 7.

9 pH Scale A change of 1 pH unit represents a tenfold (x10) change in the acidity of the solution. Tomato – pH 4 Lemon - pH 2 Lemons are 100 times more acidic than tomatoes

10 Acid – Base Reactions A reaction between an acid and a base is called neutralization. The result of a “perfect” neutralization reaction is a solution with a pH of 7

11 Acid – Base reactions HCl NaOH  NaCl H2O The products of an acid base reaction are a salt and water This is a type of double replacement reaction

12 Acid Nomenclature An easy way to remember which goes with which…No Oxygen In acid w/Oxygen An easy way to remember which goes with which… “You ATE something ICky, and you bITE something deliciOUS”

13 Examples: Memorize these four acids – names and chemical formulasHCl hydrochloric acid H2SO4 sulfuric HNO3 nitric H3PO4 phosphoric

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15 For simplicity you will use 3 significant figures for pH, pOH, [H+] and [OH-] calculations

16 Calculating the pH or pOHpH = - log [H+] pOH = - log [OH-] (The brackets [ ] mean concentration or Molarity) Example: If [H+] = 1.00 X M, what is the pH? pH = - log (1 X 10-10) pH = 10.0 Example: If [OH-] = 1.80 X 10-5 M ,what is the pOH? pOH = - log 1.80 X 10-5 pOH = 4.74

17 2) A 0.15 M solution of hydrochloric acid (acids have H+ ion)pH = - log [H+] Find the pH of these: [H+] = 1.25 x M pH = 2.90 2) A 0.15 M solution of hydrochloric acid (acids have H+ ion) pH = 0.824 3) A 3.00 X 10-7 M solution of nitric acid pH = 6.52

18 2) A 0.350 M solution of NaOH (bases have OH- ion)pOH = - log [OH-] Find the pOH of these: [OH-] = 2.15 x 10-3 pOH = 2.67 2) A M solution of NaOH (bases have OH- ion) pOH = 0.456 3) A 3.00 X 10-7 M solution of potassium hydroxide pOH = 6.52

19 Calculating the pOH or pH when you KNow the other OneSince acids and bases are opposites, pH and pOH are opposites! If pH = 1, then pOH = 13 Since pH and pOH are on opposite ends, pH + pOH = 14

20 pH and pOH calculations Solving for [H+] and [OH-]If the pH of Coke is 3.12, [H+] = ??? Because pH = - log [H+] then [H+] = antilog-pH [H+] = 10-pH [H+] = = 7.59 x 10-4 M

21 pOH calculations – Solving for [OH-]If the pOH of soap is 8.9, what is the [OH-]? [OH-] = 10-pOH [OH-] = = 1.26 x 10-9

22 [H+], [OH-] anD kw We can also use Kw (water constant)Kw = 1 x 10-14 Kw = [H+] [OH-] , so [H+] [OH-] = 1 x 10-14 What is the [H+] of a solution that has an [OH-] = 4.20 x 10-5 ? 2.38 x 10-10

23 Chapter 19 Acids and Bases Equation sheet - use this during exam[H+] to pH (-), then log, then number [OH-] to pOH Same as above pH to pOH or pOH to pH pH + pOH = 14 pH to [H+] 2nd, then log, then (-), then number pOH to [OH-] Same as above [H+] to [OH-] or [OH-] to [H+] [H+] [OH-] = 1.0 x 10-14

24 Examples: What is the pH of a 1.70 x 10-5 M solution of HCl? pH = 4.77 What is the pOH of a .0320M solution of NaOH? pH = 1.49 3. A solution has a pH of 6.40, what is the [H+]? 3.98 x 10-7 M What is the pOH of a solution with a pH of 4.50? pH = 9.50

25 Is this an acid, base, or neutral?5. What is the [H+] of a 1.6 x 10-9 M solution of NaOH? [OH-] = 1.6 x M 1.0 x 10-14 1.6 x = [H+] = 6.3 x 10-6 M 6. What is the [H+], [OH-], and pOH of a solution with pH = 3.67? pOH = 10.33 [H+] = 2.14 x 10-4 M [OH-] = 4.68 x M Is this an acid, base, or neutral?

26 pH testing There are several ways to test pHBlue litmus paper (red = acid) Red litmus paper (blue = basic) pH paper (multi-colored) pH meter (7 is neutral, <7 acid, >7 base) Indicators like phenolphthalein – we will use this

27 ACID-BASE Titrations REACTIONSHCl (aq) + NaOH (aq)  NaCl (aq) + H2O (l) acid base We can carry out this neutralization reaction using TITRATION. This will allow us to determine the unknown concentration of an acid or base ([H+] or [OH-])

28 ACID-BASE REACTIONS TitrationsAt the end of a titration reaction Moles of acid = moles of base

29 Titration is used to determine the Concentration of OH- (or H+) ion in the solution being analyzed Titration video 3:15 min

30 Titration CalculationsFor titrations using HCl and NaOH, we can simply use the dilution formula to do our calculations (because there is one H+ for every one OH-) M1V1 = M2V2

31 Titration CalculationsExample: Determine the volume of M NaOH needed to titrate 20.0mL of 0.400M HCl?

32 Titration CalculationsExample: What is the concentration of HCl if 34.5 mL of .0500M NaOH is required to titrate 50.0mL of the HCl solution?