# Notes on Unit 4 Acids and Bases

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1 Ionization of Water DEMONSTRATION OF CONDUCTIVITY OF TAP WATER AND DISTILLED WATER Pure distilled water still has a small conductivity. Why? There are a few ions present. Almost all the pure water is H 2 O molecules. But every once in a while, this happens: H + H O + H H O + O H H O H H A proton is transferred Hydronium Hydroxide From one water molecule to another. An equilibrium is established Equation: Ionization of Water H 2 O + H 2 O H 3 O + + OH Or 2H 2 O (l) H 3 O + (aq) + OH (aq) Process is Endothermic 2H 2 O (l) + 59KJ H 3 O + (aq) + OH (aq) All water or aqueous solutions contain these. In neutral water [H 3 O + ] = [OH ] In acidic solutions [H 3 O + ] > [OH ] Know these!! In basic solutions [OH ] > [H 3 O + ] Write the Keq Expression for this equilibrium: Keq = 59KJ + 2H 2 O (l) H 3 O + (aq) + OH (aq) Keq = [H 3 O + ] [OH] (liquid water left out) Given a special name for ionization of water called Kw So Kw = [H 3 O + ] [OH ] Ionization constant for water Always true at any temp! Chemistry 12Notes of Unit 4 Acids and Bases Page 13

2 Since reaction is endothermic: 59KJ + 2H 2 O (l) H 3 O + (aq) + OH (aq) At higher temps are favoured and Kw is er. At lower temps are favoured and Kw is er. At 25 o C (only) Kw = 1.00 x Know this!! For comparison At 10 0 C Kw = x (smaller) At 60 0 C Kw = 9.55 x (larger) So Always: [H 3 O + ] [OH ] = Kw At 25 0 C only: [H 3 O + ] [OH ] = 1.00 x [H 3 O + ] & [OH ] in Neutral Water At 25 o C (NOTE: Assume Temp = 25 o C unless otherwise noted) [H 3 O + ] [OH ] = 1.00 x and [H 3 O + ] = [OH ] if water is neutral. (substitute. [H 3 O + ] for [OH ]) (If water is mentioned in a problem, it can be assumed to be NEUTRAL unless otherwise stated!) [H 3 O + ] [H 3 O + ] = 1.00 x [H 3 O + ] 2 = 1.00 x [H 3 O + ] = 1.00 x = 1.00 x 10 7 M Also [OH ] = [H 3 O + ] = 1.00 x 10 7 M At Higher Temp Given: Kw at 60 0 C = 9.55 x Calculate [H 3 O + ] & [OH ] at 60 0 C Chemistry 12Notes of Unit 4 Acids and Bases Page 14

3 [H 3 O + ] & [OH ] in Acids and Bases 2H 2 O (l) H 3 O + (aq) + OH (aq) Add acid, H 3 O + increases, so equilibrium shifts LEFT and [OH ] decreases All acids produce H 3 O + in water Add base, [OH ] increases, so the equilibrium shifts LEFT and [H 3 O + ] decreases. Finding [H 3 O + ] and [OH ] in Acids and Bases At 25 0 C Eg.) Find the [OH ] in M HCl In a Strong Acid ([H 3 O + ] = [acid]) [H 3 O + ] = M [H 3 O + ][OH ] = 1.00 x [OH ] = 1.00 x = 1.00 x = 1.00 x M [H 3 O + ] 1.00 x 10 2 Find [H 3 O + ] in M NaOH. [OH ] is less in an acid than in neutral water. [H 3 O + ][OH ] = 1.00 x [H 3 O + ] = 1.00 x = 1.00 x = 3.33 x [OH ] [H 3 O + ] is very low in a strong fairly concentrated base Find [H 3 O + ] in M Ba(OH) 2 In a STRONG BASE, [OH ] = [base] x # of OH s [OH ] =? ( ) M [H 3 O + ] = 1.00 x = M ( ) Chemistry 12Notes of Unit 4 Acids and Bases Page 15

4 At Other Temps you d be given Kw eg.) Kw at 60 0 C = 9.55 x Calculate [OH ] in M HNO 3 at 60 0 C. [H 3 O + ][OH ] = Kw SA [H 3 O + ][OH ] = 9.55 x [OH ] = 9.55 x = 1.59 x M Rd. pg Ex pg. 127 of SW. ph Shorthand method of showing acidity (or basicity, alkalinity) If [H 3 O + ] = 0.10 M (1.0 x 10 1 M) ph = 1.00 [H 3 O + ] = M (1.0 x10 4 M) ph = 4.00 Definition of ph ph= log 10 [H 3 O + ] (assume log = log 10 ) If [H 3 O + ] = 1.0 x 10 7 ph = log (1.0 x 10 7 ) Regular Scientific Calculator. Enter: 1 EXP 7 +/ LOG +/ and the answer should be 7 For DAL (Sharp) calc. Enter: +/ log 1 Exp +/ 7 = and the answer should be 7 For a TI 83 Enter () LOG 1 2 nd EE () 7 ENTER and the answer should be 7 Use the () button at the bottom right of the white pad. NOT the on the far right NOTE: If you are using a DAL or a TI 83 calculator and the number you want to find the ph of is the answer to a an ongoing calculation, leave the answer to your calculation in the calculator and press () or +/ log 2 nd ANS ENTER ( or =). Practice finding ph s on your own calculator. You will be doing many of these in the rest of this unit and it s important that you can do it quickly and easily and accurately! Chemistry 12Notes of Unit 4 Acids and Bases Page 16

5 Find the ph of M HCl 2 SD s SA. So [H 3 O + ] = [acid] [H 3 O + ] = M ph= log (0.030) = How to round off?? Sig. Digits in ph start at decimal point!!! so ph = 1.52 Start counting here. Find the ph of neutral water at 25 0 C [H 3 O + ] = 1.00 x 10 7 ph = Find the ph of M NaOH at 25 0 C [H 3 O + ] = 1.00 x = 1.00 x M No units for ph Basic solution [OH ] At 25 o C so ph = sig. digits In neutral water ph = 7.0 In acid solution ph < 7.0 In basic solution ph > 7.0 ph Scale 25 o C) More Acidic Neutral More Basic Chemistry 12Notes of Unit 4 Acids and Bases Page 17

6 Calculate ph of 12.0 M HCl Very concentrated Acid! Answer Another example: Calculate the ph of 15.0 M NaOH: [H 3 O + ] = 1.00 x = 6.67 x M 15.0 Very concentrated Base ph = log (6.67 x ) ph = ph = log [H 3 O + ] ph = log [H 3 O + ] antilog (ph) = [H 3 O + ] Converting ph to [H 3 O + ] or [H 3 O + ] = antilog (ph) 3 SD s eg.) If ph = , find [H 3 O + ] Put in () before you take the antilog [H 3 O + ] = antilog (11.612) For regular Scientific Calculator: Enter: / 2 nd log The calculator answer should be x The original ph had 3 SD s, so the answer must also have 3 SD s (Remember the answer is NOT a ph, so digits to the LEFT of the decimal point are also significant!). Remember that concentration also has a unit!. So the answer would be reported as: [H 3 O + ] = 2.44 x M 3 SD s unit For a DAL or TI 83 enter: 2 nd log () (or +/) ENTER (or =) If ph = calculate [H 3 O + ] Chemistry 12Notes of Unit 4 Acids and Bases Page 18

7 Logarithmic Nature of ph A change of 1 ph unit a factor of 10 in [H 3 O + ] or (acidity) eg.) ph = 3.0 [H 3 O + ] = 1 x 10 3 M ph goes down 1 unit 10 times more acidic ph = 2.0 [H 3 O + ] = 1 x 10 2 M How many times more acidic is ph 3 than ph 7? ph 7 [H 3 O + ] = 1 x 10 7 x 10 4 = 10,000x ph 3 [H 3 O + ] = 1 x 10 3 or taking antilog of difference in ph 7 3 = 4 antilog 4 = 10 4 = 10,000 times (remember lower ph more acidic) Natural rainwater ph ~ 6 Extremely acidic acid rain ph ~ 3 diff = 3 & antilog (3) = 10 3 (1,000) So, the acid rain is 1000 times more acidic than natural rain water! poh = log [OH ] poh And [OH ] = antilog (poh) Calculate the poh of M KOH [OH ] = 2.0 x 10 3 M poh = log (2.0 x 10 3 ) = 2.70 Find the ph of the same solution: [OH ] = 2.0 x 10 3 M [H 3 O + ] = 1.00 x = 5.0 x x 10 3 ph = Notice: ph + poh = From Math: If a x b = c Then: log a + log b = log c Eg.) 10 x 100 = 1000 Log(10) + log(100) = log(1000) = 3 Chemistry 12Notes of Unit 4 Acids and Bases Page 19

8 So since [H 3 O + ] [OH ] = Kw log[h 3 O + ] + log[oh ] = log (Kw) or make everything negative log[h 3 O + ] + log [OH ] = log Kw ph + poh = pkw (relation) True at all temperatures where pkw = log Kw (definition of pkw) Specifically at 25 0 C Kw = 1.00 x pkw = log (1.00 x ) pkw = Only at 25 0 C so at 25 0 C ph + poh = At 25 0 C If ph = 4.00 poh = Or: If ph = poh= eg.) Find the ph of 5.00 x 10 4 M LiOH (25 0 C) plan: [OH ] poh ph [OH ] = 5.00 x 10 4 poh = ph = = eg.) Find the poh of M HBr (25 0 C) [H 3 O + ] = M (HBr is a strong acid) ph = poh = poh = See poh scale & ph scale. Pg. 140 S.W. Chemistry 12Notes of Unit 4 Acids and Bases Page 20

9 When not at 25 0 C Eg.) At 60 0 C Kw = 9.55 x Find the ph of neutral water at 60 0 C. One way: Calculate pkw pkw = log Kw = log (9.55 x ) At 60 0 C pkw = For neutral water ph = poh ([H 3 O + ] = [OH ]) ph + poh = pkw (substitute ph for poh) ph + ph = pH = so ph = = Is ph always 7.00 in neutral water? At higher temp: 2H 2 O + heat H 3 O + + OH Summary: [H 3 O + ] > 1.0 x 10 7 so ph < 7 [OH ] > 1.0 x 10 7 so poh < 7 In neutral water ph = poh at any temp. ph & poh = 7.00 at 25 0 C only. At lower temps ph and poh are > 7 At higher temps ph and poh are < 7 These are very important? Make sure you study these! At any temp: ph + poh = pkw At 25 0 C: ph + poh = Read p in SW. Do ex (p S.W.) Do Worksheet 43 ph and poh Calculations K a & K b for Weak acids and Bases Reminder: ph of SA s [H 3 O + ]=[acid] strong means 100% ionized so, to find ph of M HCl [H 3 O + ] = M ph = Chemistry 12Notes of Unit 4 Acids and Bases Page 21

10 For weak acids [H 3 O + ] << [acid] Eg.) What is ph of 0.10 M HF? Look at equilibrium for Weak Acid HF HF (aq) + H 2 O (l) H 3 O + (aq) + F (aq) Dissolved but not ionized Pure liquid not included in Keq expression. Keq = [H 3 O + ][F ] [ HF] for WA s Keq is called K a (acid ionization constant) see acid table for list of Ka s. higher Ka stronger acid lower Ka weaker acid For SA s (eg. HCl) Ka = [H 3 O + ] [Cl ] = called very large! [HCl] Essentially zero molecular HCl Discuss Relative Strengths of Oxyacids Calculations Using Ka (Used for Weak Acids ) [H 3 O + ] from Ka (ph from Ka) 1. [H 3 O + ] from Ka and Original concentration (Co) eg.) Find the [H 3 O + ] in 0.10 M HF WA 1. Write out equilibrium equation for ionization HF + H 2 O H 3 O + + F Chemistry 12Notes of Unit 4 Acids and Bases Page 22

11 2. Ice table 3. Ka expression: Ka = [H 3 O + ][F ] [HF] Ka = (x) (x) 0.10 x 4. Substitute Ka = x 2 5. Solve for x ([H 3 O + ]) Ka = x HF + H 2 O H 3 O + + F [I] [C] x +x +x [E] 0.10 x x x 0.10 ( Assume 0.10 x 0.10 ) So x 2 = 0.10 Ka [H 3 O + ] = x = = [H 3 O + ] = 5.9 x 10 3 M ~ Check assumption (we see that this is quite small compared to 0.10) Do ex. 74 & 75 Pg. 152 To avoid quadratic assume x is insignificant compared to 0.10 This can be confirmed later Ka 0.10 (3.5 x 10 4 ) After Questions 74 & 75 You must state this assumption here! Ka from Acid Table In Chem. 12 with weak acids, always use this assumption Make sure you state it! Short cut for multiple choice Only!! For WA [H 3 O + ] = C o Ka NOTE: In W.R. questions, full solution must be shown including the assumption! root a coka (beer) (cola) C o is Original Acid Concentration Eg.) Find ph of 2.0 M acetic acid (Multiple Choice Question) 1. First [H 3 O + ] = C o Ka = 2.0 (1.8 x 10 5 ) [H 3 O + ] = 6.0 x 10 3 M Ka from Acid Table 2. Find ph = log (6.0 x 10 3 ) ph = SD s. The 2.0 M was 2 SD s and the Ka was 2 SD s Try using this for a SA!! Chemistry 12Notes of Unit 4 Acids and Bases Page 23

12 NOTE: Ions which act as acids can come from compounds. Eg.) See table ~ ammonium ion NH 4 + can be found in NH 4 NO 3, NH 4 Cl, NH 4 Br, etc. ferric ( hexaaquoiron) Fe 3+ ( Fe(H 2 O) 6 3+ ) could be found in Fe(H 2 O) 6 Br 3 (also called FeBr 3 ) or Fe(H 2 O) 6 (NO 3 ) 3 (also called Fe(NO 3 ) 3 ) Aluminum (hexaaquoaluminum) Al 3+ (Al(H 2 O) 6 3+ ) could be found in Al(H 2 O) 6 Cl 3 ( also called AlCl 3 ) Do ex. 79 & 81, Pg. 152 More Ka Calculations: Ka from ph NOTE: the ph is to 3 SD s so your final answer cannot have more than 3 SD s. Eg.) a M Solution of the weak acid HA has a ph of Find the Ka of HA. 1. First convert ph to [H 3 O + ] [H 3 O + ] = antilog (ph) = antilog (1.620) [H 3 O + ] = x 10 2 M This is the [H 3 O + ] at equilibrium 2. Write out equilibrium equation for ionization. Make an ICE table: HA + H 2 O H 3 O + + A [I] [C] [E] x 10 2 Now, you can see that the change in concentration [C] of [H 3 O + ] is x 10 2 M and using the mole ratios (mole bridges) in the balanced equation, you can figure out the [C] s for the A and the HA: x 10 2 M x 10 2 M x 10 2 M HA + H 2 O H 3 O + + A [I] [C] x x x 10 2 [E] x 10 2 Now, we can figure out the equilibrium concentrations of HA and A. There are no x s in the table so we don t need to make any assumptions. It is best to use your calculator to figure out the equilibrium [HA], because the [C] may or MAY NOT be insignificant. Using a calculator x 10 2 = Don t round it off too much here. I would keep it in a memory in my calculator. BUT BECAUSE THE IS 3 DECIMAL PLACES AND YOU ARE SUBTRACTING, THE [E] OF HA CANNOT HAVE MORE THAN 3 DECIMAL PLACES (although you should use in your calculator) JUST REMEMBER THAT IN THE NEXT CALCULATION, THE 3 DECIMAL PLACES IN THE ICE TABLE TRANSLATES TO 3 SD S, SO YOUR FINAL ANSWER CANNOT HAVE MORE THAN 3 SD S. Chemistry 12Notes of Unit 4 Acids and Bases Page 24

13 2.399 x 10 2 M x 10 2 M x 10 2 M HA + H 2 O H 3 O + + A [I] [C] x x x 10 2 [E] x x Write Ka expression & substitute values. Ka = [H 3 O + ][A ] = (2.399 x 10 2 ) 2 [HA] = x 10 3 and expressing in 3SD s, the answer is: Ka = 1.77 x 10 3 For those that want a shortcut for multiple choice: Ka from [H 3 O + ] : Ka = [H 3 O + ] 2 ( Co [H 3 O + ] ) OK for multiple choice ONLY! Don t forget this Don t rearrange [H 3 O + ] = C o Ka Was derived using an assumption which may NOT be valid! Do Ex. 77 & 80 on p. 152 SW To Calculate Co ( conc. of acid needed) form ph & Ka Eg. Find the concentration of HCOOH needed to form a solution with ph = First change ph to [H 3 O + ] [H 3 O + ] = antilog (ph) = antilog (2.69) [H 3 O + ] = x 10 3 M (notice that the given ph limits us to 2SD s, but keep more in your calculations.) 2. Write out ionization equilibrium with an ICE TABLE. You can insert x 10 3 for equilibrium [H 3 O + ]. And since our unknown is the initial [HCOOH], we put in an C o for the [I] of HCOOH: HCOOH + H 2 O H 3 O + + HCOO [I] C o 0 0 [C] [E] x 10 3 Chemistry 12Notes of Unit 4 Acids and Bases Page 25

14 Now we can see that the change in concentration [C] of [H 3 O + ] is x 10 3 and the [C] of HCOO will be the same. The [C] of HCOOH will be x 10 3 HCOOH + H 2 O H 3 O + + HCOO [I] C o 0 0 [C] x x x 10 3 [E] x 10 3 We can now calculate the equilibrium concentrations [E] of HCOOH and HCOO. HCOOH + H 2 O H 3 O + + HCOO [I] C o 0 0 [C] x x x 10 3 [E] C o x x x 10 3 The next step will be to write the K a expression and substitute the equilibrium concentrations in: 3. Write Ka expression. Substitute equilibrium concentrations in. Find Ka for HCOOH on the acid table: Ka = [H 3 O + ] [HCOO ] [ HCOOH] Find Ka on Acid Table 1.8 x 10 4 = ( x 10 3 ) 2 ( Co x 10 3 ) Now we can solve for Co (the original concentration of the acid): Co x 10 3 = ( x 10 3 ) x 10 4 Co x 10 3 = x 10 2 Co = x x 10 3 Co = 2.52 x 10 2 M Co = 2.5 x 10 2 M or M (remember, we are restricted to 2 SD s) Do Ex. 76 & 78 on p. 152 of SW. Now For Bases Base ionization NH 3 very common weak base. It partially ionizes in water to form NH 4 + and OH : NH 3(aq) + H 2 O (l) NH 4 + (aq) + OH (aq) Equilibrium constant called base ionization constant (Kb) Chemistry 12Notes of Unit 4 Acids and Bases Page 26

15 NH 3(aq) + H 2 O (l) NH 4 + (aq) + OH (aq) Kb expression: Kb = [NH 4 + ] [OH ] [NH 3 ] NOTE: Ions can also act as a weak bases. The reaction of an ion with water to form OH is called base hydrolysis. Equilibrium constant is still called Kb. Eg.) Hydrolysis of CN CN (aq) + H 2 O (l) HCN (aq) + OH (aq) Already an ion Kb = [HCN][OH ] [CN ] Kb expression Ionization of N 2 H 4 (weak base) N 2 H 4 (aq) + H 2 O (l) N 2 H 5 + (aq) + OH (aq) A neutral molecule Kb = [N 2 H 5 + ] [OH ] [N 2 H 4 ] Kb expression Do Ex 32 on p. 128 of SW. How to Find Kb using Acid Table (not shown directly) Derivation Look at hydrolysis of base F : F + H 2 O HF + OH Kb (F) = [HF] [OH ] [F ] Look at ionization the weak acid HF: HF + H 2 O H 3 O + + F Ka (HF) = [H 3 O + ] [F ] [HF] Multiply Ka [HF] x Kb [F ] Conj. Acid Conj. base Ka [HF] x Kb [F ] = [H 3 O + ] [F ] x [HF] [OH ] = [H 3 O + ] [OH ] (notice that [HF] and [F ] will cancel.) [HF] [F ] or Ka (HF) x Kb (F ) = Kw Chemistry 12Notes of Unit 4 Acids and Bases Page 27

16 Ka (HF) x Kb (F ) = Kw Or Kb (F ) = Kw Ka (HF) In general: Kb (weak base) = Kw Ka (it s conj. acid) Using Acid Table: 1. Find base on right side ( if amphiprotic locate base on right side only) 2. It s conjugate acid will be across from it on the left side. 3. The Ka of it s conjugate acid is on the far right of the same line. 4. Use equation: Kb (base) = Kw Ka(conj. acid) Eg.) Calculate the Kb for HCO 3 : ( find HCO 3 on RIGHT SIDE) Line: H 2 CO 3 H + + HCO x 10 7 It s conj. acid Base Ka (it s conj. acid) Kb(HCO 3 ) = Kw = 1.0 x = 2.3 x 10 8 Ka(H 2 CO 3 ) 4.3 x 10 7 Find Kb of SO 3 2 Similarly : If Kb (base) given Ka (weak acid) = Kw Kb(it s conj. Base) Eg.) The Kb for base B is 2.73 x 10 9 Find the Ka for the acid HB 3 sig. Digs. Ka (HB) = Kw = 1.00 x = 3.66 x 10 6 Kb (B ) 2.73 x 10 9 Chemistry 12Notes of Unit 4 Acids and Bases Page 28

17 NOTES: Table only states Ka values. For questions like this Kb will have to be calculated if not given. All Ka s on table are 2 SD s limits any calculation using them to 2 SD s maximum. The larger the Kb, the stronger the weak base the more OH produced. The smaller the Ka of an acid, the larger the Kb of its conjugate Base. (Weaker acids have stronger conjugate bases) Calculations Involving Kb Given: Find or find or find [Base] & Kb [OH ] poh ph eg.) Find [OH ] in a 0.20 M solution of KNO 2 (this is a salt, so it must be dissociated into it s ions first) Dissociation of KNO 2 K + + NO 2 Neutral spectator (discard) Weak base 1. Find Kb of NO 2 K b (NO 2 ) = Kw K a (HNO 2 ) = 1.0 x x 10 4 K b (NO 2 ) = x Hydrolysis ( if ion) or ionization ( if molecule) equation followed by an ICE table: NO 2 + H 2 O HNO 2 + OH [I] [C] [E] We can let x equal the moles/l of NO 2 which hydrolyze as the reaction reaches equilibrium. Using the mole ratios in the equation and calculating [E] s we get: NO 2 + H 2 O HNO 2 + OH [I] [C] x +x +x [E] 0.20 x x x 3. K b Expression: K b = [HNO 2 ] [OH ] [NO 2 ] at equilibrium On the next page, we substitute the [E] s into the Kb expression (Don t forget, we are in baseland not acidland now!) Chemistry 12Notes of Unit 4 Acids and Bases Page 29

18 Substitute: Kb = [HNO 2 ] [OH ] or Kb = x 2 [NO 2 ] (0.20 x) Approximation: Kb x Original conc. of NO 2 (Co) Assume that 0.20 x 0.20 x 2 = 0.20 K b [OH ] = [OH ] = 0.20 Kb 0.20 (2.174 x ) [OH ] = x 10 6 M [OH ] = 2.1 x 10 6 M Both the 0.20 M and the Ka used in calculating Kb limit us to 2 SD s. NOTE: In many problems, finding [OH ] is only the first step. Often you have to find the ph. Then you would use the process [OH ] poh ph Kb From ph and Concentration Eg.) At a certain temp, a 0.20 M solution of K 2 SO 3 has a ph of Calculate the Kb of SO 3 2 at this temp. 1. Identify SO 3 2 as a weak base (When K 2 SO 3 is dissociated, it yields K + (a spectator) and SO 3 2 ) 2. [OH ] can be obtained from ph (ph poh [OH ] ) ph = so poh = = 3.75 [OH ] = antilog (poh) = antilog (3.75) = x 10 4 M 3. Write hydrolysis equation and an ICE table. (It is called hydrolysis this time because SO 3 2 is an ion.) We know the initial [SO 3 2 ] is 0.20M and the equilibrium [OH ] is x 10 4 M: 2 SO 3 + H 2 O HSO 3 + OH [I] [C] [E] x 10 4 So, from this, the change in conc. [C] of OH is x 10 4 and using the coefficient ratios we can insert the [C] s for the other species and calculate the equilibrium concentrations [E] s: 2 SO 3 + H 2 O HSO 3 + OH [I] [C] x x x 10 4 [E] x x 10 4 Chemistry 12Notes of Unit 4 Acids and Bases Page 30

19 4. Now we write the Kb expression and substitute the values from the [E] s in our ICE table: K b = [HSO 3 ] [OH ] = ( x 10 4 ) 2 = x 10 7 [SO 3 2 ] ( ) We round it to 1.6 x 10 7 because the 0.20M and the ph given both had 2 SD s So: Kb of SO 3 2 at the temperature given is = 1.6 x 10 7 Rd. pg & Do Ex. 84, 87, 88,& 89 on p. 153 of SW Short Cut for Multiple Choice: Kb = [OH ] 2 (C O [OH ]) Like Weak acids: Ka = [H 3 O + ] 2 (Co [H 3 O + ]) Do worksheet on Ka, Kb calculations Chemistry 12Notes of Unit 4 Acids and Bases Page 31

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