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ACID- BASE EQUILIBRIA

ACID- BASE EQUILIBRIA. ACID- BASE EQUILIBRIA. ACID- BASE EQUILIBRIA. ACID- BASE EQUILIBRIA. +. H H N H H. Al 3+ + 6 H 2 O Al(H 2 O) 6. H + +. H N H H. H + + NH 3 NH 4 1+.

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ACID- BASE EQUILIBRIA

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  1. ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA ACID- BASE EQUILIBRIA

  2. + H H N H H Al3+ + 6 H2O Al(H2O)6 H+ + H N H H H+ + NH3 NH41+ H2O + SO3 H2SO4 : BF3 + NH3 BF3 - NH3 LEWIS ACIDS & BASES ACID = ELECTRON PAIR ACCEPTOR BASE = ELECTRON PAIR DONOR MUST HAVE AN UNSHARED PAIR OF ELECTRONS TO DONATE TO THE COVALENT BOND BETWEEN THE ACID AND BASE

  3. + + O THAT IS, MUST BE A LEWIS BASE O O NH3 - oo C C o o o o O H oo H3C H3C o o o o ACID - BASE REACTION NEUTRALIZATION BRONSTED - LOWRY BRONSTED ACIDS AND BASES H+ SPECIAL CASE OF THE LEWIS ACID-BASE THEORY ACID IS A PROTON DONOR BASE IS A PROTON ACCEPTOR MUST HAVE UNSHARED PAIR OF ELECTRONS PROTON BOUND TO A VERY ELECTRONEGATIVE ATOM NOT AN ACID PROTON

  4. ARRHENIUS: PRODUCES H1+ IN WATER BRONSTED: PROTON DONOR ACID: LEWIS: HAS EMPTY ORBITAL + DIFFERENCE: BRONSTED ACID HAS A PROTON! ARRHENIUS: PRODUCES OH1- IN WATER BASE: BRONSTED: PROTON ACCEPTOR LEWIS: HAS e- PAIR AVAILABLE TO SHARE SALT + WATER NEUTRALIZATION

  5. NAMING ACIDS UNLESS DISSOLVED IN WATER -- COVALENT HBr BINARY: HYDROBROMIC ACID HYDROGEN HYDRO BROMIDE BROMIC HF HI HYDROFLUORIC ACID HYDROIODIC ACID POLYATOMIC ANIONS -ITE = OUS OR -ATE = IC EXCEPTING S OR P CO3 2- CARBON ATE ION H2 CO3 IC ACID H2 SO4 = SULFURIC ACID SO42- = SULFATE ION H2 SO3 = SULFUROUS ACID SO32- = SULFITE ION

  6. HCOOH (aq) + H2 O (l) HCOO1- (aq) + H3 O1+ (aq) + + CONJUGATE CONJUGATE CONJUGATE CONJUGATE CONJUGATE O HOBr (aq) + H2 O (l) OBr1- (aq) + H3 O1+ (aq) O O NH3 - oo C C o o o o O H oo H3C H3C o o o o CONJUGATE BRONSTED ACID-BASECONJUGATE PAIRS BASE ACID ACID BASE CONJUGATE PAIRS DIFFER BY A SINGLE PROTON!!!

  7. CH3COOH (aq) + NH3 (aq) CH3COO1- (aq) + (aq) a IF K >> 1, REACTION IS EXTENSIVE DISSOCIATION IS EXTENSIVE IF K << 1, DISSOCIATION IS NOT EXTENSIVE THE LARGER THE VALUE OF K, THE MORE EXTENSIVE IS THE REACTION

  8. [HS1-] [H3O1+] [ H2S] H2S (aq) + H2O (l)  HS1- (aq) + H3O1+ (aq) K = a THE LARGER THE VALUE OF K, THE STRONGER IS THE ACID OR THE BASE Kb = 1 X 10-14 / Ka FOR ACID: THE MORE H3O1+ ION IS PRODUCED HIGH Ka + HIGH Kb = EXTENSIVE REACTION FROM ACID - BASE CHART: RESULT: K>1 IF PRODUCT IS THE WEAKER ACID OR BASE OF THE CONJUGATE PAIR

  9. ACID-BASE STRENGTH STRENGTH OF THE HA BOND BINARY HA USUALLY: STRONGER BOND = WEAKER ACID ELECTRONEGATIVITY OF A OXOACID (OXYANION) X-O- H OXIDATION STATE OF X ELECTRONEGATIVITY OF X RESULT: K>1 IF PRODUCT IS THE WEAKER ACID OR BASE OF THE CONJUGATE PAIR

  10. H2O (l) + H301+ H2O (l) + H301+ Ka < Ka FOR H3O1+ Ka << 1 WEAK ACID: Kb < Ka FOR H3O1+ Kb << 1 WEAK BASE: HX WHERE X = Cl, Br, I STRONG ACIDS: HNO3, HClO4, H2SO4 STRONG BASE: SOLUBLE METAL HYDROXIDE

  11. H2O (l) + H2O (l) H3O1+ (aq) + OH1- (aq) [H3O1+] > [OH1-] ACIDIC SOLUTION [H301+] = [OH1-] NEUTRAL SOLUTION [H3O1+] < [OH1-] BASIC SOLUTION K = Kw = [H3O1+][OH1-] = 1.0 x 10-14 AT 25 oC <7 = 7 >7 [H3O1+] = [OH1-] = 1.0x10-7 M -log [H3O1+] -log[1.0x10-7 ] pH = pK = -logKa pH + pOH = 14 pKa + pKb = 14 Ka x Kb = 1.0 x 10-14

  12. Scales to determine Acidity or Alkalinity Base Acid pH 0 2 4 6 7 8 10 12 14 14 12 10 8 7 6 4 2 0 pOH Acid Base

  13. 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14 GASTRIC JUICE, 0.1 M HCl ACIDIC ORANGE JUICE COKE, VINEGAR WINE TOMATO, BEER BLACK COFFEE RAIN SALIVA URINE HUMAN MILK NEUTRAL BLOOD, TEARS SEAWATER, EGG WHITE BILE BAKING SODA BORAX BASIC NAIR HOUSEHOLD AMMONIA DRAIN CLEANER, 0.1 M NaOH

  14. pH = -log[H3O1+] Kw = [H3O1+][OH1-] = 1.0 x 10-14 C. [H3O1+] A. SOLUTION WHERE [H3O1+] = 3.6x10-6 M B. 0.25 M HCl C. SOLUTION WHERE [OH1-] = 2.5x10-3 M WHAT IS THE pH of: WHAT IS THE [OH1-] CONC. OF A pH = 4.5 SOLUTION? A. pH = - LOG[3.6x10-6] = 5.4 (AN ACIDIC SOLUTION) B. pH = -LOG[0.25] = 0.60 [2.5x10-3] = 1.0x10-14 = 4.0x10-12 pH = -LOG[4.0x10-12] = 11.4 (A BASIC SOLUTION) [H3O1+] = 10-pH = 10-4.5 = 3.2x10-5 [3.2x10-5][OH1-] = 1.0 x 10-14 = 3.1x10-10 M

  15. Titration Sample problem • What volume of 1.0 M HCl is needed to neutralize 30.0 mL of 2.5 M NaOH?

  16. Try These: • What is the molarity of 5.0 mL of acid used to neutralize 10.0 mL of 2.5 M base? • What volume of 1.0 M base is needed to neutralize 20.0 mL of 2.3 M acid?

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