CEE 370 Environmental Engineering Principles

Transcription

1 Updated: 29 September 2015 Print version CEE 370 Environmental Engineering Principles Lecture #7 Environmental Chemistry V: Thermodynamics, Henry s Law, Acids-bases II Reading: Mihelcic & Zimmerman, Chapter 3 Davis & Masten, Chapter 2 Mihelcic, Chapt 3 David Reckhow CEE 370 L#7 1

2 Henry s Law Henry's Law states that the amount of a gas that dissolves into a liquid is proportional to the partial pressure that gas exerts on the surface of the liquid. In equation form, that is: C A = K H p A where, C A = concentration of A, [mol/l] or [mg/l] K H = equilibrium constant (often called Henry's Law constant), [mol/l-atm] or [mg/l-atm] p A = partial pressure of A, [atm] David Reckhow CEE 370 L#7 2

3 Henry s Law Constants Reaction Name K h, mol/l-atm pk h = -log K h CO 2 (g) _ CO 2 (aq) Carbon 3.41 x dioxide NH 3 (g) _ NH 3 (aq) Ammonia H 2 S(g) _ H 2 S(aq) Hydrogen 1.02 x sulfide CH 4 (g) _ CH 4 (aq) Methane 1.50 x O 2 (g) _ O 2 (aq) Oxygen 1.26 x David Reckhow CEE 370 L#7 3

4 Example: Solubility of O 2 in Water Background Although the atmosphere we breathe is comprised of approximately 20.9 percent oxygen, oxygen is only slightly soluble in water. In addition, the solubility decreases as the temperature increases. Thus, oxygen availability to aquatic life decreases during the summer months when the biological processes which consume oxygen are most active. Summer water temperatures of 25 to 30 C are typical for many surface waters in the U.S. Henry's Law constant for oxygen in water is 61.2 mg/l-atm at 5 C and 40.2 mg/l-atm at 25 C. What is the solubility of oxygen at 5 C and at 25 C? Example 4.1 from Ray David Reckhow CEE 370 L#7 4

5 Solution O 2 Solubility Ex. At 5 0 C the solubility is: C (5 C) = K P = 61.2 O H,O O C O 2 (5 C) = 12.8 mg L mg L- atm x atm At 25 0 C the solubility is: C (25 C) = K P = 40.2 O H,O O C O 2 mg L- atm (25 C) = 8.40 mg L x atm David Reckhow CEE 370 L#7 5

6 Air Stripping Tower Air out with Carbon Dioxide Water in with Carbon Water Out Air In David Reckhow CEE 370 L#7 6

7 Air Stripping Example An air stripping tower, similar to that shown in the previous slide, is to be used to remove dissolved carbon dioxide gas from a groundwater supply. If the tower lowers the level to twice the equilibrium concentration, what amount of dissolved gas will remain in the water after treatment? The partial pressure is about 350 ppm or The log of is about Therefore the partial pressure of carbon dioxide in the atmosphere is atm. Example 4.2 from Ray David Reckhow CEE 370 L#7 7

8 Solution to Air Stripping Ex. The first step is to determine Henry's Law constant for carbon dioxide. From the table it is The equilibrium solubility is then: = K mole L-atm CO H,CO p atm CO =10 10 = C 2 At equilibrium: After treatment: -5-5 C CO 2 = 10 M = 10 mole L x 44 g mole C CO 2 = 0.44 mg/ L C CO2 = 0.88 mg/l 3 10 mg x g mole L David Reckhow CEE 370 L#7 8

9 Ideal Gas Law The Ideal Gas Law states that the product of the absolute pressure and the volume is proportional to the product of the mass and the absolute temperature. In equation form this is usually written: PV = nrt where, P = absolute pressure, [atm] V = volume, [L] n = mass, [mol] T = absolute temperature, [K] R = proportionality constant or ideal gas constant, [ L-atm/K-mol] David Reckhow CEE 370 L#7 9

10 Ideal Gas Law Example Anaerobic microorganisms metabolize organic matter to carbon dioxide and methane gas. Estimate the volume of gas produced (at atmospheric pressure and 25 C) from the anaerobic decomposition of one mole of glucose. The reaction is: C 6 H 12 O 6 3CH 4 + 3CO 2 Example 4.3 from Ray David Reckhow CEE 370 L#7 10

11 Solution to Ideal Gas Law Ex. Each mole of glucose produces three moles of methane and three moles of carbon dioxide gases, a total of six moles. The total volume is then: V = nrt P = L- atm (6 mol)( )(298 K) K- mol (1 atm) V = 147 L David Reckhow CEE 370 L#7 11

12 Dalton s Law of Partial Pressure Dalton's Law of partial pressures states that the total pressure of a mixture of several gases is the sum of the partial pressures of the individual gases. In equation form this is simply: n P t = Pi i=1 where, P t = total pressure of the gases, [atm] P i = pressure of the ith gas, [atm] David Reckhow CEE 370 L#7 12

13 Anaerobic Digester Example Anaerobic digesters are commonly used in wastewater treatment. The biological process produces both carbon dioxide and methane gases. A laboratory worker plans to make a "synthetic" digester gas. There is currently 2 L of methane gas at 1.5 atm and 1 L of carbon dioxide gas at 1 atm in the lab. If these two samples are mixed in a 4 L tank, what will be the partial pressures of the individual gases? The total pressure? Example 4.4 from Ray David Reckhow CEE 370 L#7 13

14 Solution to Anaerobic Digester Ex. First, we must find the partial pressures of the individual gases using the ideal gas law: 1 P = P V V 2 P1 V 1 = nrt = P2 V2 or 2 1 For methane gas For carbon dioxide gas: P 2 = 1.5 atm P 2 = 1 atm 2 L 4 L 1 L 4 L = 0.75 atm = 0.25 atm And the total is: P t = P CH + P CO = 1 atm 4 2 David Reckhow CEE 370 L#7 14

15 Equilibrium Reactions aa + bb pp + rr c d K eq = {C } {D } a b {A } {B } thermodynamics a, b, p, r = stoichiometric coefficients of the respective reactants {A}, {B}, {P}, {R} = activity of the reactants and products David Reckhow CEE 370 L#7 15

16 Chemical Activity {A} = γ A [A] {A} = activity of species A, [mol/liter] [A] = concentration of species A, [mol/liter] γ A = activity coefficient of A, unitless γ is dependent on ionic strength -- the concentration of ions in solution. For dilute aqueous solutions γ is near unity. Thus, the activity and concentration are approximately the same. For most freshwater systems, γ may be neglected. David Reckhow CEE 370 L#7 16

17 Activity conventions the activity of the solvent, water is set equal to unity the activity of a solid in equilibrium with a solution is unity the activity of a gas is the partial pressure the gas exerts on the liquid surface the activity of a solute is related to the concentration by {A} = γ A [A], where γ A is the activity coefficient of species A David Reckhow CEE 370 L#7 17

18 Auto-dissociation of Water H O 2 H + OH + - K = w + - [ H ][ OH ] [ H O] = [ H ][ OH ] At 25 C the value of K w is David Reckhow CEE 370 L#7 18

19 Example 4.12 Find the ph and poh of water at 25 C if the concentration of H + ions is 10-5 M. Solution + -5 ph = - log{h } = - log(10 ) = 5 {OH } = - w K {H } = = poh = - log{oh } = - log(10 ) = David Reckhow CEE 370 L#7 19

20 Acids & Bases Which is the strongest acid A. H 3 PO 4 B. H 2 CO 3 C. HNO 3 D. CH 3 COOH E. HF David Reckhow CEE 370 L#7 20

21 Acid:Base Equilibria Monoprotic Acid HA Diprotic Acid + - H + A H A = H + HA 2 HA + - H + A K A = { H }{ A } K 1 = A {HA} + - { H }{ HA } { H A} + 2- K A 2 = { H }{ A } - 2 { HA } David Reckhow CEE 370 L#7 21

22 Similar to Table 3.5 in M&Z Acidity Constants Reaction Name K a pk a = log K a HCl = H + + Cl Hydrochloric H 2 SO 4 = H + + HSO 4 - HNO 3 = H + + NO 3 - HSO 4 - = H + + SO 4 - H 3 PO 4 = H + + H 2 PO 4 - Sulfuric, H Nitric ~1 ~0 Sulfuric, H2 1 x Phosphoric, H x HAc = H + + Ac - Acetic 2.00 x H 2 CO 3 = H + + HCO 3 - Carbonic, H x H 2 S = H + + HS - Hydrosulfuric, H x H 2 PO 4 - = H + + HPO 4 2 Phosphoric, H x HOCl = H + + OCl - Hypochlorous 3.16 x NH 4 + = H + + NH 3 Ammonium 5.01 x HCO 3 - = H + + CO 3 2 HPO 4 2 = H + + PO 4 3 Carbonic, H x Phosphoric, H x David Reckhow CEE 370 L#7 22

23 NAME EQUILIBRIA pka Perchloric acid HClO4 = H+ + ClO STRONG Hydrochloric acid HCl = H+ + Cl- -3 Sulfuric acid H2SO4= H+ + HSO (& 2) ACIDS Nitric acid HNO3 = H + + NO Hydronium ion H3O+ = H+ + H2O 0 Trichloroacetic acid CCl3COOH = H + + CCl3COO Iodic acid HIO3 = H+ + IO3-0.8 Dichloroacetic acid CHCl2COOH = H + + CHCl2COO Bisulfate ion HSO4 - = H+ + SO4-2 2 Phosphoric acid H3PO4 = H+ + H2PO (& 7.2,12.3) Ferric ion Fe(H2O)6 +3 = H+ + Fe(OH)(H2O) (& 4.6) Chloroacetic acid CH2ClCOOH = H+ + CH2ClCOO o-phthalic acid C6H4(COOH)2 = H+ + C6H4(COOH)COO (& 5.51) Citric acid C3H5O(COOH)3= H + + C3H5O(COOH)2COO (& 4.77,6.4) Hydrofluoric acid HF = H+ + F- 3.2 Formic Acid HCOOH = H + + HCOO Aspartic acid C2H6N(COOH)2= H+ + C2H6N(COOH)COO (& 9.82) m-hydroxybenzoic acid C6H4(OH)COOH = H+ + C6H4(OH)COO (& 9.92) Succinic acid C2H4(COOH)2 = H + + C2H4(COOH)COO (& 5.61) p-hydroxybenzoic acid C6H4(OH)COOH = H+ + C6H4(OH)COO (& 9.32) Nitrous acid HNO2 = H+ + NO2-4.5 Ferric Monohydroxide FeOH(H2O) H+ + Fe(OH)2(H2O) Acetic acid CH3COOH = H + + CH3COO Aluminum ion Al(H2O)6 +3 = H + + Al(OH)(H2O) David Reckhow CEE 370 L#7 23

24 NAME FORMULA pka Propionic acid C2H5COOH = H + + C2H5COO Carbonic acid H2CO3 = H + + HCO (& 10.33) Hydrogen sulfide H2S = H + + HS (& 13.9) Dihydrogen phosphate H2PO4 - = H + + HPO Hypochlorous acid HOCl = H + + OCl Copper ion Cu(H2O)6 +2 = H + + CuOH(H2O) Zinc ion Zn(H2O)6 +2 = H + + ZnOH(H2O) Boric acid B(OH)3 + H2O = H + + B(OH)4-9.2 (& 12.7,13.8) Ammonium ion NH4 + = H + + NH Hydrocyanic acid HCN = H + + CN p-hydroxybenzoic acid C6H4(OH)COO - = H + + C6H4(O)COO Orthosilicic acid H4SiO4 = H + + H3SiO (& 13.1) Phenol C6H5OH = H + + C6H5O m-hydroxybenzoic acid C6H4(OH)COO - = H + + C6H4(O)COO Cadmium ion Cd(H2O)6 +2 = H + + CdOH(H2O) Bicarbonate ion HCO3 - = H + + CO Magnesium ion Mg(H2O)6 +2 = H + + MgOH(H2O) Monohydrogen phosphate HPO4-2 = H + + PO Calcium ion Ca(H2O)6 +2 = H + + CaOH(H2O) Trihydrogen silicate H3SiO4 - = H + + H2SiO Bisulfide ion HS - = H + + S Water H2O = H + + OH Ammonia NH3 = H + + NH2-23 Hydroxide OH - = H + + O M ethane CH4 = H + + CH3-34 David Reckhow CEE 370 L#7 24

25 Acidity Constants, #1 Reaction Name K a pk a HCl = H + +Cl - Hydrochloric H2SO4 = H + +HSO4 - Sulfuric, H HNO3 = H + +NO3 - Nitric ~1 ~0 HSO4 - = H + + SO4-2 Sulfuric, H2 1x H3PO4 = H + + H2PO4 - Phosphoric, H1 7.9x HAc = H + + Ac - Acetic 2.0x H2CO3 = H + + HCO3 - Carbonic, H1 5.0x David Reckhow CEE 370 L#7 25

26 Acidity Constants, #2 Reaction Name K a pk a H2S = H + +HS - Hydrosulfuric, H1 7.9x H2PO4 - = H + +HPO4-2 Phosphoric, H2 6.3x HOCl = H + +OCl - Hypochlorous 2.5x NH4 + = H + + NH3 Ammonium 5x HCO3 - = H + + CO3-2 Carbonic, H2 5x HPO4-2 = H + + PO4-3 Phosphoric, H3 5x David Reckhow CEE 370 L#7 26

27 Example What fraction of the following acids are ionized at ph 7? a) Nitric b) Hydrochloric c) Sulfuric d) Hypochlorous David Reckhow CEE 370 L#7 27

28 Solution to Example a) K = a + - [H ][NO 3] [HNO ] 3 [HNO 3] - [NO ] 3 = [H + ] K = 10 1 a -7 = 10-7 F = - [NO 3] [HNO ] + [NO ] = - [NO ] [NO ] + [NO ] David Reckhow CEE 370 L#7 28

29 Solution to Example d) K = a + - [H ][OCl ] [HOCl] [HOCl] - [OCl ] = [H + ] K = = a F = - [OCl ] - [HOCl] + [OCl ] = - [OCl ] - - 4[OCl ] + [OCl ] = 0.20 David Reckhow CEE 370 L#7 29

30 Log C vs ph Diagram for Hypochlorous Acid -2 C T = 10-3 M Log C (Molar) HOCl OCl ph David Reckhow CEE 370 L#7 30

31 Log C (Molar) Log C vs ph Diagram for Hypochlorous Acid [HOCl] - [OCl ] ph C T = 10-3 M HOCl OCl- = [H + ] K = [H + ] 10 a -7.6 David Reckhow CEE 370 L#7 31

32 Definitions Bronsted-Lowry (1923) Acids: (proton donor) any substance that can donate a proton to any other substance Bases: (proton acceptor) any substance that accepts a proton from any other substance Acid 1 + Base 2 = Acid 2 + Base 1 HNO 3 + H 2 O = H 3 O NO 3 HOCl + H 2 O = H 3 O + + OCl - NH H 2 O = H 3 O + + NH 3 Acid strength of a conjugate acid-base pair is measured relative to the other pair the stronger the acid, the weaker the conjugate base, and vice versa H 2 O + H 2 O = H 3 O + + OH - David Reckhow CEE 370 L#7 32

33 To next lecture David Reckhow CEE 370 L#7 33