BIOMEDICAL SCIENCE MIN WAN

Size: px
Start display at page:

Download "BIOMEDICAL SCIENCE MIN WAN"

Transcription

1 ACID-BASE LECTURE BIOMEDICAL SCIENCE MIN WAN SEPT , /6/2016 1

2 Acid Base lecture September 2015 Min Wan 1. Introduction to ph 2. Acid base concept -calculations 3. Buffer -calculations 4. Titration 5. Physiologic ph regulation -calculations 6. How to measure ph -Read: Kemiboken från gymnasiet, Harvey & Ferrier, sid 6-9, Kompendiet Syra-Bas 9/6/2016 2

3 1. Introduction to ph 9/6/2016 3

4 1. Introduction to ph What does ph means? ph describes the concentration of H + or H 3 O + in water solution. ph value is lower, the hydronium ion concentration is greater. 9/6/2016 4

5 1. Introduction to ph How to calculate ph? ph = -log [H + ] Example : If the ph of a solution is 3.4, what is the hydronium ion concentration? [H 3 O + ] = 10 -ph = = M = M = mm 9/6/2016 5

6 1. Introduction to ph [H + ] (M = moles/liter) [H + ] (M) ph /6/

7 1. Introduction to ph Dissociation of H 2 O [H + ] = [H 3 O + ] Neutral water has a tendency to ionize H 2 O H + + OH - The free proton is associated with a water molecule to form the hydronium ion (H 3 O + ) H 2 O + H 2 O H 3 O + + OH - 9/6/2016 7

8 2. Acids and Bases Brønsted-Lowry definition Acid: a substance that can donate a proton Base: a substance that can accept a proton HCl + H 2 O H 3 O + + Cl - Acid Base Conjugate Acid Conjugate Base H 2 O + NH 3 NH OH - Acid Base Conjugate Acid Conjugate Base 9/6/2016 8

9 Ion Centrations (M) 2. Acids and Bases Acidic [H + ] > 10-7 M Neutral [H + ] = 10-7 M Basic [H + ] < 10-7 M [H + ] [OH - ] /6/ ph

10 2. Acids and Bases Relative strength of acids and bases strong and weak acids/bases The stronger acids are those that lose their hydrogen ions more easily than other acids. Similarly, the stronger bases are those that hold hydrogen ions more strongly than other bases. 9/6/

11 2. Acids and Bases Strong acid undergoes complete dissociation Ex. HCl HCl + H 2 O Cl - + H 3 O + HCl Cl - H 3 O + Relative strength of acids and bases Weak acid undergoes partial dissocation Ex. Acetic acid HAc + H 2 O Ac - + H 3 O + < 1% of HAc will react HAc HAc H + Ac - 9/6/

12 2. Acids and Bases Weak acids/bases HA + H 2 O H 3 O + + A - Acid Base Conjugate Acid Conjugate Base The relative stability of the acid form as compared to its conjugate base form determines if it is a weak or a strong acid. If the acid is stable = the proton is not lost easily= weak acid (ex HAc) If the conjugate base is stable = the proton will easily be lost = strong acid (ex HCl) 9/6/

13 2. Acids and Bases Neutralisation A solution of strong acids and bases HCl + NaOH HCl + NaOH H + + Cl - + Na + + OH - H 2 O + Na + + Cl - If we take same amount of HCl as NaOH, it becomes neutral neutralization otherwise it becomes acidic or basic. 9/6/

14 2. Acids and Bases ph calculation calculate ph in an acid solution Strong acid complete dissociation, equilibrium shifts to the right completely HCl + H 2 O Cl - + H 3 O + ph = -log [H + ] HCl Cl - H 3 O + Weak acid partial dissociation, at equilibrium there is still acid left HAc + H 2 O Ac - + H 3 O + HAc HAc 1 M 1 M 1 M 1 M? M H + Ac - 9/6/

15 2. Acids and Bases ph calculation Calculation of ph in a solution of a weak acid Law of mass action (the rate of a chemical reaction is proportional to the concentrations of the reacting substances.) Experimental values of K a (acid base constant) 9/6/

16 2. Acids and Bases Law of Mass action Two reactions: HAc + H 2 O Ac - + H 3 O + 1) HAc + H 2 O k 1 Ac - + H 3 O + V 1 = k 1 [HAc] [H 2 O] 2) Ac - + H 3 O + k 2 HAc + H 2 O V 2 = k 2 [Ac - ] [H 3 O + ] At equilibrium: V 1 = V 2 k 1 [HAc] [H 2 O] = k 2 [Ac - ] [H 3 O + ] k 1 = [Ac-] [H 3 O + ] [HAc] [H2O] = K a (acid constant) k 9/6/

17 2. Acids and Bases acid constant HAc + H 2 O Ac - + H 3 O + K a = [Ac - ] [H 3 O + ] [HAc] [H 2 O] K a = [Ac - ] [H 3 O + ] [HAc] K a is the acid constant and it has a specific value for each acid a large K a a strong acid a small K a a weak acid pka = -LogKa 9/6/

18 2. Acids and Bases Acid constant, Ka Acid K a pk a (-log K a ) strong weak HCl H 2 SO H 3 PO Lactic acid butyric acid Acetic acid K a describes acid strength 9/6/

19 2. Acids and Bases Base constant, Kb K b (base constant) H 2 O + NH 3 NH OH - K b = [NH 4 + ] [OH - ] [NH 3 ] pk b = -LogK b 9/6/

20 2. Acids and Bases Base constant, Kb Base K b pk b (-log K b ) strong weak OH CO NH HCO acetate K b describes base strength 9/6/

21 2. Acids and Bases Acid/Base constant Conjugated acid-base pair: pk a + pk b = 14 HAc / Ac - : = 14 H 2 O / OH - : (-1.74) = 14 H 3 O + / H 2 O : = 14 H 2 CO 3 /HCO - 3 : = 14 9/6/

22 2. Acids and Bases Law of Mass action and experimental values of K a Now we can calculate ph in a solution of a weak acid! Ex: 0.1 mol acetic acid (CH 3 COOH) in 1 liter H 2 O, what is the ph? 9/6/

23 2. Acids and Bases Weak acids Ex. 0.1 mol acetic acid (CH 3 COOH) in 1 liter H 2 O HAc + H 2 O Ac - + H 3 O + Before equil After equil X X X K a = [Ac - ] [H 3 O + ] [HAc] 2:a grade equation... Make two approximations: 1) X << 0.1 2) X >> 10-7 K a = X (X ) X = X X 0.1 X 2 = 0.1 K a K a HAc = X 2 = /6/

24 2. Acids and Bases Weak acids Ex. 0.1 mol acetic acid (CH 3 COOH) in 1 liter H 2 O HAc + H 2 O Ac - + H 3 O + Before equil After equil X X X K a = K a = [Ac - ] [H 3 O + ] [HAc] X (X ) X K a HAc = X 2 = X = M [H 3 O + ] = X (X >> 10-7 ) X 2 = 0.1 K a [H 3 O + ] = M ph = -lg [H 3 O + ] = -lg ( ) = /6/

25 2. Acids and Bases Acid/Base constant Autoionization of water and Kw H 2 O as acid: a H + donor H 2 O H + + OH - H 2 O as base: a H+ acceptor H 2 O + H + H 3 O + H 2 O + H 2 O H 3 O + + OH - K = [products] [reactants] = [H 3 O + ] [OH - ] [H 2 O] [H 2 O] K is the dissociation constant K w = [H 3 O + ] [OH - ] = K becomes K w K w = ion product of water 9/6/

26 2. Acids and Bases Ion product of water K w = Ion product of water Neutral water [H 3 O + ] = [OH - ] = 10-7 Kw = [H 3 O + ] [OH - ] = (10-7 ) (10-7 ) = Therefore the ph of pure water = -log (10-14 ) = 7 pkw = -logkw = 14 = -log ([H 3 O + ] [OH - ] ) = -log [H 3 O + ] +(-log [OH - ]) = ph + poh pkw = ph + poh = 14 9/6/

27 2. Acids and Bases Amphoteric species An amphoteric species is a molecule or ion that can react as an acid as well as a base. H 2 O Ex. of other amphoteric species bisulfate monohydrogen phosphate dihydrogen phosphate a) HSO H 2 O SO H 3 O + b) HSO H 2 O H 2 SO 4 + OH - c) HPO H 2 O PO H 3 O + d) HPO H 2 O H 2 PO 4 + OH - e) H 2 PO 4- + H 2 O HPO H 3 O + f) H 2 PO 4- + H 2 O H 3 PO 4 + OH - bicarbonate g) HCO H 2 O CO H 3 O + h) HCO H 2 O H 2 CO OH - 9/6/

28 Acid Base lecture September 2015 Min Wan 1. Introduction to ph 2. Acid base concept -calculations 3. Buffer -calculations 4. Titration 5. Physiologic ph regulation -calculations 6. Measure ph? 9/6/

29 Observation If you add 0.01 ml of 1M HCl to 1000 ml of water ph 7, the ph of the water drops from 7 to 5!! i.e 100 fold increase in H + concentration: Log = 2 change. Problem: Large fluctuations in ph would disrupt the harmonious interactions of proteins and enzymes for efficiency in biochemical reactions in our body. Actually, biological properties change with small changes in ph, usually less than 1 ph unit. How does a system prevent fluctuations in ph? 9/6/

30 3. Buffer Buffer solutions A buffer consists of corresponding pairs of weak acids and weak bases HA H + + A - Weak acid proton conjugate base A buffer solution is keeping the ph relatively constant when strong acid or base is added. A buffer keeps the ph constant during dilution with water. 9/6/

31 3. Buffer Make a buffer How to make a buffer solution? 1) a weak acid with its corresponding weak base 2) a weak acid with a strong base 3) a weak base with a strong acid 9/6/

32 3. Buffer Buffer equation How can we determine the ph in a buffer? HA + H 2 O A - + H 3 O + K a = [A - ] [H 3 O + ] [HA] lg K a = lg [A - ] + lg [H 3 O + ] lg [HA] -lg [H 3 O + ] = -lg K a + lg [A - ] lg [HA] [A - ] ph = pk a + lg [HA] Buffer equation! (Hendelson-Hasselbach) 9/6/

33 3. Buffer Buffer equation ph = pk a + lg [A- ] [HA] -Can only be used to calculate ph in buffers. -Only valid if 1/30 < base/acid < 30 9/6/

34 3. Buffer Make a buffer Ex: To mix 1 L 0.1 M HAc and 1 L 0.2 M NaAc, what is the final ph of the solution? HAc H + + Ac - NaAc Na + + Ac - [HAc] [Ac - ] Before 0.1 M 0.2 M After 0.05 M 0.1 M [base] 0.1 = = 2 [acid] 0.05 buffer ph = pk a + lg [base] [acid] = lg 2 = = valid if 1/30 < base/acid < 30 9/6/

35 3. Buffer Make a buffer Example of different conjugate acid base pairs. 9/6/

36 3. Buffer Buffer equation How does ph change in a buffer upon dilution Ex: 0.2 mol acetate buffer in 1 liter H 2 O (0.1 mol HAc, 0.1 mol Ac - ) [acid] [base] [HAc] [Ac - ] ph = pk a + lg ph = pk a + lg 1 ph = pk a = 4.76 Add 1 liter H 2 O ph = pk a + lg 0.05 [acid] [base] 0.05 [HAc] [Ac - ] ph = pk a + lg ph = /6/

37 3. Buffer ph = pk a + lg [Ac- ] [HAc] pka = ph when [HA] = [A - ] (50% dissociated) The buffer capacity is largest when ph = pka. 9/6/

38 ph 3. Buffer A buffer pair is usually considered to be a useful buffer within one ph unit on either side of its pka Buffer range pka of Tris buffer is 8.1, the buffering range is More acid added pka More base added 9/6/

39 3. Buffer Ex:1 L 0.1 M acetate buffer ph = 5, what is the ph value after adding 3 ml 6 M HCl? 1) To calculate the concentration of acid and base in acetate buffer ph = pk a + lg [Ac- ] [HAc] 5 = lg [Ac- ] [HAc] 0.24 = lg [Ac- ] [HAc] [HAc] + [Ac - ] = 0.1 M [Ac - ] = [HAc] 0.1- [HAc] = 1.74 [HAc] [HAc] = M [Ac - ] [HAc] [Ac - ] = [HAc] = M = = /6/

40 3. Buffer Ex:1 L 0.1 M acetate buffer ph = 5, what is the ph value after adding 3 ml 6 M HCl? 2) To calculate the amount of acid and base in acetate buffer V = 1L n (HAc) = [HAc] V = M 1 L = mol n (Ac - ) = [Ac - ] V = M 1 L = mol 3) To calculate the amount of acid and base after adding HCl n (HCl) = [HCl] V = 6 M L = mol H 3 O + + Ac - HAc + H 2 O Before: /6/ After:

41 3. Buffer Ex:1 L 0.1 M acetate buffer ph = 5, what is the ph value after adding 3 ml 6 M HCl? 3) To calculate the amount of acid and base after adding HCl n (HCl) = [HCl] V = 6 M L = mol H 3 O + + Ac - HAc + H 2 O Before: After: ) To calculate the concentrations of acid and base after reaction ph = pk a + lg [Ac- ] [HAc] = lg = /6/

42 3. Buffer When the buffer is buffering, the equilibrium is changed Buffer range 9/6/

43 Acid Base lecture September 2015 Min Wan 1. Introduction to ph 2. Acid base concept -calculations 3. Buffer -calculations 4. Titration -calculations 5. Physiologic ph regulation -calculations 6. Measure ph? 9/6/

44 4. Titration Titration is a common laboratory method to determine the unknown concentration of an acid or base. Ex: a strong acid HCl (unknown concentration) a strong base NaOH (known concentration) How can we use NaOH to know the concentration of HCl? 9/6/

45 4. Titration Titration is a common laboratory method to determine the unknown concentration of an acid or base. Add NaOH into HCl to get neutrolization equivalent point ph indicator (phenolphthalein) ph probe equivalent point: colorness to pink amount base added = amount acid at start 9/6/

46 4. Titration Ex: 20 ml HCl is titrated with 16 ml of 0.1 M NaOH to the equivalent point. What is the concentration of HCl? C a V a = C b V b C a 20 ml = 0.1 M 16 ml C a = 0.1 M 16 ml / 20 ml = 0.08 M = 80 mm Answer: The concentration of the HCl solution is 80 mm. 9/6/

47 ph 4. Titration Titration of a weak acid (HAc) with a strong base [HAc] = [Ac - ] CH 3 COO - equivalent point amount base added = amount acid at start CH 3 COOH ph = pk a = 4.76 best buffer capacity Percent titration

48 4. Titration Ex: 1 L phosphoric acid of unknown concentration is titrated with 0.1 M KOH. The approximate ph range of ph indicator for color change is When the ph indicator changes the color, 35 ml KOH is added. What is the concentration of phosphoric acid? 1) To calculate the amount of KOH added for titration n (KOH) = [KOH] V = 0.1 M L = mol = 3.5 mmol 9/6/

49 4. Titration Ex: 1 L phosphoric acid of unknown concentration is titrated with 0.1 M KOH. The approximate ph range of ph indicator for color change is When the ph indicator changes the color, 35 ml KOH is added. What is the concentration of phosphoric acid? 2) To calculate the amount of H 3 PO 4 H 3 PO 4 + KOH H 2 PO K + + H 2 O H 2 PO KOH HPO K + + 2H 2 O HPO KOH PO K + + 3H 2 O n (KOH) = 2 n (H 3 PO 4 ) n (KOH) = 3.5 mmol n (H 3 PO 4 ) = 1.75 mmol 9/6/

50 4. Titration Ex: 1 L phosphoric acid of unknown concentration is titrated with 0.1 M KOH. The approximate ph range of ph indicator for color change is When the ph indicator changes the color, 35 ml KOH is added. What is the concentration of phosphoric acid? 2) To calculate the amount of H 3 PO 4 H 3 PO 4 + 2KOH HPO K + + 2H 2 O n (KOH) = 2 n (H 3 PO 4 ) n (KOH) = 3.5 mmol n (H 3 PO 4 ) = 1.75 mmol 3) To calculate the con. of H 3 PO 4 C (H 3 PO 4 ) = n (H 3 PO 4 ) / V = 1.75 mmol / 1 L 9/6/2016 = 1.75 mm 50

51 4. Titration Titration curve for the amino acid alanine + H 3 N H C COOH [OH - ] + H 3 N H C COO - [OH - ] H 2 N H C COO - CH 3 CH 3 CH 3 Form I (alanine in acid solution) Form II (alanine in neutral solution) Form III (alanine in base solution) Two groups on alanine that can donate proton Two pka -COOH / -COO - pk a1 = 2.3 -NH 3 + / -NH 2 pk a2 = 9.2 9/6/

52 4. Titration 9/6/

53 Acid Base lecture September 2014 Min Wan 1. Introduction to ph 2. Acid base concept -calculations 3. Buffert -calculations 4. Titration 5. Physiological ph regulation -calculations 6. Measure ph? 9/6/

54 5. Physiological ph regulation Life [H 3 O + ]: Blood ph value 10-6 M 10-7 M 10-8 M [OH - ]: 10-8 M 10-7 M 10-6 M Normal ph value of blood 7.4 Blood (venous) Blood (arteriell) How can we keep the ph so constant in our body? 9/6/

55 5. Physiological ph regulation Buffers in body fluids Our body uses 3 different systems to keep the ph constant: 1) Buffers in body fluids (the first minutes) a) Phosphate buffer inside the cells b) Proteins (albumin,hemoglobin) inside the cells c) Bicarbonate buffer in blood or plasma 2) Regulate breathing via lung (adjust CO 2 ) 3) Long term regulation via kidneys 9/6/

56 5. Physiological ph regulation Buffers in body fluids 1) Buffers in body fluids a) Phosphate buffer inside the cells b) Proteins (albumin,hemoglobin) inside the cells c) Bicarbonate buffer in blood or plasma Inside the cells: haemoglobin 35% other proteins 7% phosphate 5% 47% Blood or plasma: bicarbonate 53% 9/6/

57 5. Physiological ph regulation Phosphate buffer 1) Buffer-phosphate buffer H 3 PO 4 + H 2 O H 2 PO H 3 O + H 2 PO H 2 O HPO H 3 O + HPO H 2 O PO H 3 O + Two of the ions are amphoteric species! 9/6/

58 5. Physiological ph regulation Phosphate buffer The phosphate buffer system mainly works in the internal fluid of cells What kind of phosphate ions do we have in the cells? (H 2 PO 4- ) (HPO 4 2- ) Many molecules contain phosphate groups, such as adenosine triphosphate (ATP) adenosine diphosphate (ADP) 9/6/ adenosine monophosphate (AMP)

59 5. Physiological ph regulation Protein as a buffer 1) Buffer-proteins When a protein acts as a buffer, only a few amino acids are responsible 9/6/

60 5. Physiological ph regulation Proteins as a buffer Amino acids that can buffer: + Histidine acid conjugate base - Cysteine acid conjugate base When the amino acid is buffering, the charge will change! 9/6/

61 5. Physiological ph regulation Proteins as a buffer The protein structure can change due to ph When histidin-side chain buffer, it will take up a proton. H 3 O + It becomes positively charged. The new + gives a new electrostatic interaction with a neighbouring - Structure will change. Maybe even the function of the protein? 9/6/

62 5. Physiological ph regulation Bicarbonate buffer 1) Buffer-bicarbonate buffer H 2 CO 3 + H 2 O HCO H 3 O + Conjugate acid. Conjugate base HCO H 2 O CO H 3 O + Conjugate acid Conjugate base First proteolytic step important. 9/6/

63 5. Physiological ph regulation Bicarbonate buffer In body fluids H 2 CO 3 + H 2 O HCO H 3 O + Conj. Acid conj.. base Dihydrogen carbonate (H 2 CO 3 ) can exist in water, but will quickly become CO 2 bubbles. CO 2 (d) + 2H 2 O H 2 CO 3 + H 2 O HCO H 3 O + conj. acid conj. base The acid in bicarbonate buffer consists of H 2 CO 3 and CO 2 (d) together. 9/6/

64 5. Physiological ph regulation Bicarbonate buffer CO 2 is dissolved in water CO 2 CO 2 Water with dissolved H 2 CO 3 and CO 2 H 2 CO 3 H 2 CO 3 CO 2 CO 2 The concentration of dissolved CO 2 is proportional to the partial pressure of CO 2 (p CO2 ) outside. H 2 CO 3 H 2 CO 3 CO 2 CO 2 (d) + 2H 2 O H 2 CO 3 + H 2 O HCO H 3 O + [CO 2 ] + [H 2 CO 3 ] = 0.23 p CO2 9/6/

65 5. Physiological ph regulation Bicarbonate buffer Buffer formula for bicarbonate buffer CO 2 + 2H 2 O H 2 CO 3 + H 2 O HCO H 3 O + conjugate acid Conjugate base ph = pk a + lg [base] [acid] ph = pk a + lg [HCO 3- ] 0.23 p CO2 [HCO ph = pk a + lg 3- ] [CO 2 ] + [H 2 CO 3 ] Henderson Hasselbalch s formula [CO 2 ] + [H 2 CO 3 ] = 0.23 p CO2 [HCO 3- ]: mm, p CO2 : kpa 9/6/

66 5. Physiological ph regulation Bicarbonate buffer Buffer formula for bicarbonate buffer [HCO 3- ] ph = pk a + lg 0.23 p CO2 Henderson Hasselbalch s formula ph depends on the ratio of [HCO 3- ] and P CO2 Normal human arterial blood: Pco 2 = 5.3 kpa (40 mmhg) [HCO 3- ] = 24 mm [HCO 3- ] ph = pk a + lg 0.23 p CO2 24 = lg = lg 20 9/6/ = = 7.4

67 5. Physiological ph regulation Bicarbonate buffer CO 2 + 2H 2 O H 2 CO 3 + H 2 O HCO H 3 O + CO 2 /HCO 3 - has a far higher buffering power in an open system than in a close system Ex. How does ph change if we add 5 mmol HCl in a closed bicarbonate buffer system (1L, ph = 7.4, [HCO 3- ] = 24 mm, Pco 2 = 5.3 kpa)? 1) Add 5 mmol HCl H 3 O + + HCO 3 - H 2 O +H 2 CO 3 CO 2 + 2H 2 O Before = 1.2 After = 6.2 [HCO ph = pk a +log 3- ] = log 19 = 6.59 [CO 2 ] + [H 2 CO 3 ] Pco 2 = [CO 2 ] + [H 2 CO 3 ] = 6.2 Pco 2 = 27 kpa 9/6/

68 5. Physiological ph regulation Bicarbonate buffer CO 2 + 2H 2 O H 2 CO 3 + H 2 O HCO H 3 O + CO 2 /HCO 3 - has a far higher buffering power in an open system than in a close system Ex. How does ph change if we add 5 mmol HCl in an open bicarbonate buffer system (1L, ph = 7.4, [HCO 3- ] = 24 mm, Pco 2 = 5.3 kpa)? 1) Add 5 mmol HCl H 3 O + + HCO - 3 H 2 O +H 2 CO 3 CO 2 + 2H 2 O Before = 1.2 After (Pco 2 constant) [HCO ph = pk a +log 3- ] = log 19 = 7.3 [CO 2 ] + [H 2 CO 3 ] 1.2 9/6/

69 5. Physiological ph regulation a closed system an open system 9/6/

70 5. Physiological ph regulation Regulate ph by lung and kidney 2) ph regulation via lung 3) ph regulation via kidneys [HCO 3- ] ph = pk a + lg 0.23 p CO2 kidney lung 9/6/

71 5. Physiological ph regulation Regulate ph by lung and kidney 2) Regulate ph via breath [HCO 3- ] ph = pk a + lg 0.23 p CO2 lung Lung: to keep Pco 2 constant by carefully matching the rates of CO 2 production and excretion. CO 2 production varies with physical activity, the lung alters ventilatory rate to keep the balance between CO 2 production and excretion. 9/6/

72 5. Physiological ph regulation Regulate ph by lung Gas transport O 2 is transported from the lung to the tissues and CO 2 formed in tissues is transported back to the lung, and the transport of these gases is coupled to ph. Hemoglobin transport O 2, and it has four Heme groups O 2 O 2 O 2 O 2 9/6/

73 5. Physiological ph regulation Lungs: High ph, Low CO 2 and O 2 affinity increases, Shift left Bohr effect: An increase of CO 2 and a decrease in ph results in reduced affinity of Hb for O 2. Tissue= Low ph, High CO 2 O 2 affinity decrease and is released to tissues Shift right 9/6/

74 5. Physiological ph regulation 3) ph regulation via kidneys [HCO 3- ] ph = pk a + lg 0.23 p CO2 kidney Kidney: to keep stable bicarbonate concentration. Kidney filters bicarbonate from blood, these ions are reabsorbs by kidney and return to blood. Kidney also can produce new bicarbonate to replace consumed bicarbonate. 9/6/

75 5. Physiological ph regulation ph 7.4 Pco 2 L H HCO - 3 Normal Acidosis and alkalosis: the processes that cause ph to change. acidosis: any disease process or condition that acts to lower ph alkalosis: any disease process or condition that acts to raise ph 9/6/

76 5. Physiological ph regulation CO 2 + H 2 O HCO H 3 O + Two ways to change [H+] or ph: change Pco 2 or change [HCO 3- ] respiratory: indicate an acidosis or alkalosis caused by a pathologic change in Pco 2 metabolic: indicate an acidosis or alkalosis caused by a pathologic change in [HCO 3- ] 9/6/

77 Metabolic Respiratory 5. Physiological ph regulation Chronic COPD L Acidosis ph 7.4 H L Alkalosis ph 7.4 H asthma diarrea renal failure L ph 7.4 H L ph 7.4 H vomiting 9/6/

78 Acid Base lecture September 2014 Min Wan 1. Introduction to ph 2. Acid base concept -calculations 3. Buffert -calculations 4. Titration 5. Physiologic ph regulation -calculations 6. Measure ph? 9/6/

79 6. Measureing ph ph paper: acid base form have different light absorbance ph meter: Measures the voltage produced by the solution, compares it with the voltage of a known standard solution, and uses the difference in voltage to calculate the ph. In vivo: measure ph value in plasma or urine. Difficult to measure inside the cell, microelectrodes and fluorescent ph indicator dyes 9/6/

80 6. Measureing ph Approximate ph values of various body fluids Boron W.F. & Boulpaep E.L. Medical Physiology 2 nd edition Compartment ph Gastric secretions 0.7 Lysosome 5.5 Cytosol of a typical cell 7.2 Arterial blood plasma Mitochondrial inner matrix 7.5 Secreted pancreas fluid 8.1 9/6/

81 END of lecture 9/6/

2. Acid base concept -calculations. 3. Buffert -calculations. 5. Physiologic ph regulation -calculations

2. Acid base concept -calculations. 3. Buffert -calculations. 5. Physiologic ph regulation -calculations Acid Base lecture 15-16 September 2014 Agnes Rinaldo-Matthis 1. Introduction to ph 2. Acid base concept -calculations 3. Buffert -calculations 4. Titration 5. Physiologic ph regulation -calculations 6.

More information

Acids and bases, ph and buffers. Dr. Mamoun Ahram Lecture 2

Acids and bases, ph and buffers. Dr. Mamoun Ahram Lecture 2 Acids and bases, ph and buffers Dr. Mamoun Ahram Lecture 2 ACIDS AND BASES Acids versus bases Acid: a substance that produces H+ when dissolved in water (e.g., HCl, H2SO4) Base: a substance that produces

More information

10/16/17 ACIDS AND BASES, DEFINED WATER IS AMPHOTERIC OUTLINE. 9.1 Properties of Acids and Bases. 9.2 ph. 9.3 Buffers

10/16/17 ACIDS AND BASES, DEFINED WATER IS AMPHOTERIC OUTLINE. 9.1 Properties of Acids and Bases. 9.2 ph. 9.3 Buffers ACIDS AND BASES, DEFINED A hydrogen atom contains a proton and an electron, thus a hydrogen ion (H + ) is a proton: Acids: Proton (H + ) transfer between molecules is the basis of acid/base chemistry Ø

More information

ph and buffers Dr. Mamoun Ahram Summer, 2018

ph and buffers Dr. Mamoun Ahram Summer, 2018 ph and buffers Dr. Mamoun Ahram Summer, 2018 Kw Kw is called the ion product for water What is ph? Example: Find the K a of a 0.04 M weak acid HA whose [H + ] is 1 x 10-4? HA H + + A - K a = [A - ] [H

More information

Principles Of Acid-Base Balance

Principles Of Acid-Base Balance Principles Of Acid-Base Balance I. Introduction A. For normal body function the free H+ concentration [H+] or ph must be kept within a narrow normal range. Some reasons why: 1. The proton "pump" within

More information

K w. Acids and bases 8/24/2009. Acids and Bases 9 / 03 / Ionization of water. Proton Jumping Large proton and hydroxide mobility

K w. Acids and bases 8/24/2009. Acids and Bases 9 / 03 / Ionization of water. Proton Jumping Large proton and hydroxide mobility Chapter 2 Water Acids and Bases 9 / 03 / 2009 1. How is the molecular structure of water related to physical and chemical behavior? 2. What is a Hydrogen Bond? 3Wh 3. What are Acids Aid and db Bases? 4.

More information

General Phenomena: Law of mass action, dissociation of water, ph, buffers

General Phenomena: Law of mass action, dissociation of water, ph, buffers General Phenomena: Law of mass action, dissociation of water, ph, buffers Ionization of Water, Weak Acids and Weak Bases Many properties of water can be explained in terms of uncharged H 2 O molecule Small

More information

Alkalosis or alkalemia arterial blood ph rises above Acidosis or acidemia arterial ph drops below 7.35 (physiological acidosis)

Alkalosis or alkalemia arterial blood ph rises above Acidosis or acidemia arterial ph drops below 7.35 (physiological acidosis) Acid-Base Balance Normal ph of body fluids Arterial blood is 7.4 Venous blood and interstitial fluid is 7.35 Intracellular fluid is 7.0 Alkalosis or alkalemia arterial blood ph rises above 7.45 Acidosis

More information

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor

ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor ph calculations MUDr. Jan Pláteník, PhD Brønsted-Lowry concept of acids and bases Acid is a proton donor Base is a proton acceptor HCl(aq) + H 2 O(l) H 3 O + (aq) + Cl - (aq) Acid Base Conjugate acid Conjugate

More information

battery acid the most widely used industrial chemical Hydrochloric acid, HCl muriatic acid stomach acid Nitric acid, HNO 3

battery acid the most widely used industrial chemical Hydrochloric acid, HCl muriatic acid stomach acid Nitric acid, HNO 3 BRCC CHM 101 Chapter 9 Notes (Chapter 8 in older text versions) Page 1 of 9 Chapter 9: Acids and Bases Arrhenius Definitions more than 100 years old Acid a substance that produces H + in water (H + is

More information

BIOC 460 General Chemistry Review: Chemical Equilibrium, Ionization of H 2 O, ph, pk a

BIOC 460 General Chemistry Review: Chemical Equilibrium, Ionization of H 2 O, ph, pk a BIOC 460 General Chemistry Review: Chemical Equilibrium, Ionization of H 2 O, ph, pk a General Equilibrium: What are the UNITS of K eq? Example reactions: A --> B units of K eq? A --> B + C units of K

More information

Chem 150, Spring Unit 4 - Acids & Bases. Introduction

Chem 150, Spring Unit 4 - Acids & Bases. Introduction Chem 150, Spring 2015 Unit 4 - Acids & Bases Introduction Patients with emphysema cannot expel CO2 from their lungs rapidly enough. This can lead to an increase of carbonic (H2CO3) levels in the blood

More information

Physiology Lecture 2 and 27 Chapter 2: Acids, Bases and Salts REVIEW:

Physiology Lecture 2 and 27 Chapter 2: Acids, Bases and Salts REVIEW: Physiology Lecture 2 and 27 Chapter 2: Acids, Bases and Salts REVIEW: 1. Salts an ionic compounds containing other than H + or OH - ; can dissociate in water to form electrolytes. Electrolytes can conduct

More information

Dr. Diala Abu-Hassan, DDS, PhD Lecture 3 MD summer 2014

Dr. Diala Abu-Hassan, DDS, PhD Lecture 3 MD summer 2014 ph, DDS, PhD Dr.abuhassand@gmail.com Lecture 3 MD summer 2014 www.chem4kids.com 1 Outline ph Henderson-Hasselbalch Equation Monoprotic and polyprotic acids Titration 2 Measuring the acidity of solutions,

More information

Acids, Bases, Salts, Buffers

Acids, Bases, Salts, Buffers Acids, Bases, Salts, Buffers Acids, Bases, Salts, Buffers An acid is any solute that dissociates in a solution and releases hydrogen ions, thereby lowering ph Since a hydrogen ion consist solely of a proton,

More information

Acid-Base Balance. Lecture # 5 Second class/ 2015

Acid-Base Balance. Lecture # 5 Second class/ 2015 Acid-Base Balance Lecture # 5 Second class/ 2015 Terms Acid Any substance that can yield a hydrogen ion (H + ) or hydronium ion when dissolved in water Release of proton or H + Base Substance that can

More information

A 95 g/mol B 102 /mol C 117 g/mol D 126 g/mol E 152 g/mol

A 95 g/mol B 102 /mol C 117 g/mol D 126 g/mol E 152 g/mol Titrations In a titration a solution of accurately known concentration is added gradually added to another solution of unknown concentration until the chemical reaction between the two solutions is complete.

More information

Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017

Acids, Bases and ph Preliminary Course. Steffi Thomas 14/09/2017 Acids, Bases and ph Preliminary Course Steffi Thomas ssthomas@tcd.ie 14/09/2017 Outline What are acids and bases? Can we provide a general definition of acid and base? How can we quantify acidity and basicity?

More information

Chapter 10 - Acids & Bases

Chapter 10 - Acids & Bases Chapter 10 - Acids & Bases 10.1-Acids & Bases: Definitions Arrhenius Definitions Acids: substances that produce hydrogen ions when dissolved in H 2 O Common Strong Acids: Common Weak acids: Organic carboxylic

More information

Where does Physical Chemistry fit into your course in Dentistry?

Where does Physical Chemistry fit into your course in Dentistry? Where does Physical Chemistry fit into your course in Dentistry? Acidogenic bacteria in dental plaque can rapidly metabolise certain carbohydrates to acid endproducts. In the mouth, the resultant change

More information

CHAPTER 8: ACID/BASE EQUILIBRIUM

CHAPTER 8: ACID/BASE EQUILIBRIUM CHAPTER 8: ACID/BASE EQUILIBRIUM Already mentioned acid-base reactions in Chapter 6 when discussing reaction types. One way to define acids and bases is using the Brønsted-Lowry definitions. A Brønsted-Lowry

More information

Unless otherwise stated, all images in this file have been reproduced from:

Unless otherwise stated, all images in this file have been reproduced from: Unless otherwise stated, all images in this file have been reproduced from: Blackman, Bottle, Schmid, Mocerino and Wille, Chemistry, 3 rd Edition 2016 (John Wiley & Sons) The University of Sydney Page

More information

Grace King High School Chemistry Test Review

Grace King High School Chemistry Test Review CHAPTER 19 Acids, Bases & Salts 1. ACIDS Grace King High School Chemistry Test Review UNITS 7 SOLUTIONS &ACIDS & BASES Arrhenius definition of Acid: Contain Hydrogen and produce Hydrogen ion (aka proton),

More information

CHAPTER 7 Acid Base Equilibria

CHAPTER 7 Acid Base Equilibria 1 CHAPTER 7 Acid Base Equilibria Learning Objectives Acid base theories Acid base equilibria in water Weak acids and bases Salts of weak acids and bases Buffers Logarithmic concentration diagrams 2 ACID

More information

Strong and Weak. Acids and Bases

Strong and Weak. Acids and Bases Strong and Weak Acids and Bases Strength of Acids H2SO4 HSO4 - + H + HNO3 NO3 - + H + Strong Acids HCl Cl - + H + H3PO4 H2PO4 - + H + Phosphoric acid Moderate Acid CH3COOH CH3COO - + H + Acetic acid HF

More information

HW #10: 10.38, 10.40, 10.46, 10.52, 10.58, 10.66, 10.68, 10.74, 10.78, 10.84, 10.88, 10.90, ,

HW #10: 10.38, 10.40, 10.46, 10.52, 10.58, 10.66, 10.68, 10.74, 10.78, 10.84, 10.88, 10.90, , Chemistry 121 Lectures 20 & 21: Brønstead-Lowry Acid/Base Theory Revisited; Acid & Base Strength - Acids & Bases in Aqueous Solution; Acid Dissociation Constants and the Autoionization of Water; ph or

More information

-log [H+][OH-] = - log [1 x ] Left hand side ( log H + ) + ( log OH - ) = ph + poh Right hand side = ( log 1) + ( log ) = 14 ph + poh = 14

-log [H+][OH-] = - log [1 x ] Left hand side ( log H + ) + ( log OH - ) = ph + poh Right hand side = ( log 1) + ( log ) = 14 ph + poh = 14 Autoionization of Water H 2 O H + + OH - K = [H + ][OH - ]/[H 2 O] = 1.802 x 10-16 Concentration of [H 2 O] is so HIGH autoionization is just a drop in the bucket, so [H 2 O] stays constant at 55.5 M,

More information

Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33

Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Acid-Base Equilibria (Chapter 10.) Problems: 2,3,6,13,16,18,21,30,31,33 Review acid-base theory and titrations. For all titrations, at the equivalence point, the two reactants have completely reacted with

More information

Acid-Base Equilibria. And the beat goes on Buffer solutions Titrations

Acid-Base Equilibria. And the beat goes on Buffer solutions Titrations Acid-Base Equilibria And the beat goes on Buffer solutions Titrations 1 Common Ion Effect The shift in equilibrium due to addition of a compound having an ion in common with the dissolved substance. 2

More information

Studying the properties of substances and the reactions that transform substances into other substances.

Studying the properties of substances and the reactions that transform substances into other substances. 3 CHEMISTRY Studying the properties of substances and the reactions that transform substances into other substances. Improving agricultural production, curing many diseases, increasing the efficiency of

More information

Water, water everywhere,; not a drop to drink. Consumption resulting from how environment inhabited Deforestation disrupts water cycle

Water, water everywhere,; not a drop to drink. Consumption resulting from how environment inhabited Deforestation disrupts water cycle Chapter 3 Water: The Matrix of Life Overview n n n Water, water everywhere,; not a drop to drink Only 3% of world s water is fresh How has this happened Consumption resulting from how environment inhabited

More information

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water.

IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. IB Chemistry ABS Introduction An acid was initially considered a substance that would produce H + ions in water. The Brønsted-Lowry definition of an acid is a species that can donate an H + ion to any

More information

Lecture #11-Buffers and Titrations The Common Ion Effect

Lecture #11-Buffers and Titrations The Common Ion Effect Lecture #11-Buffers and Titrations The Common Ion Effect The Common Ion Effect Shift in position of an equilibrium caused by the addition of an ion taking part in the reaction HA(aq) + H2O(l) A - (aq)

More information

Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride

Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride Acids and Bases Acids and bases, as we use them in the lab, are usually aqueous solutions. Ex: when we talk about hydrochloric acid, it is actually hydrogen chloride gas dissolved in water HCl (aq) Concentrated

More information

{Take note: Why is water liquid at room temperature, but Ammonia is gas at room temperature? What is Hydrogen bond?}

{Take note: Why is water liquid at room temperature, but Ammonia is gas at room temperature? What is Hydrogen bond?} 1 Structure of Water (H 2 O) UNIVERSITY OF PNG SCHOOL OF MEDICINE AND HEALTH SCIENCES DIVISION OF BASIC MEDICAL SCIENCES BIOCHEMISTRY AND MOLECULAR BIOLOGY PBL Seminar WATER, ph and BUFFER SOLUTIONS: Overview

More information

Practical: Acid-base balance

Practical: Acid-base balance Practical: Acid-base balance Definition All the processes inside the body which keep the H+ concentration within normal values. It is a result of the hydro-electrolytic balance and a sum of mechanisms

More information

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Acid-Ionization Equilibria. Acid-Ionization Equilibria Acid-Ionization Equilibria Acid-Base Equilibria Acid ionization (or acid dissociation) is the reaction of an acid with water to produce hydronium ion (hydrogen ion) and the conjugate base anion. (See Animation:

More information

Chapter 8 Lecture Notes: Acids, Bases, and ph

Chapter 8 Lecture Notes: Acids, Bases, and ph Educational Goals Chapter 8 Lecture Notes: Acids, Bases, and ph 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether the

More information

Chapter 10. Acids, Bases, and Salts

Chapter 10. Acids, Bases, and Salts Chapter 10 Acids, Bases, and Salts Topics we ll be looking at in this chapter Arrhenius theory of acids and bases Bronsted-Lowry acid-base theory Mono-, di- and tri-protic acids Strengths of acids and

More information

Physiology lecture (8): Acid Base regulation

Physiology lecture (8): Acid Base regulation Physiology lecture (8): Acid Base regulation If we add hydrogen, we have three lines of defense against a mild change in ph: 1) Buffers, instantaneous, within a fraction of milliseconds. 2) The lung, takes

More information

Chemical Equilibria Part 2

Chemical Equilibria Part 2 Unit 1 - Inorganic & Physical Chemistry 1.4 Chemical Equilibria Part 2 Acid / Base Equilibria Indicators ph Curves Buffer Solutions Pupil Notes Learning Outcomes Questions & Answers KHS ChemistrySept 2015

More information

Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations

Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations Ch. 17 Applications of Aqueous Equilibria: Buffers and Titrations Sec 1 The Common-Ion Effect: The dissociation of a weak electrolyte decreases when a strong electrolyte that has an ion in common with

More information

BIOB111_CHBIO - Tutorial activity for Session 6:

BIOB111_CHBIO - Tutorial activity for Session 6: BIOB111_CHBIO - Tutorial activity for Session 6: General topics for the week: Acids and Bases ph and buffer Interactive animations are used to reinforce the understanding Instructions- interactive animations:

More information

Acid-Base balance. Acid : is the substance that donates H+, base : is the substance which receives or removes that H+.

Acid-Base balance. Acid : is the substance that donates H+, base : is the substance which receives or removes that H+. Acid-Base balance Introduction : We usually suffer from metabolic acidosis more than alkalosis, acidosis means that there is an increase in H+ concentration in plasma and thus interstial fluid ;because

More information

Chapter 8 Acid-Base Equilibria

Chapter 8 Acid-Base Equilibria Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6

More information

10.1 Acids and Bases in Aqueous Solution

10.1 Acids and Bases in Aqueous Solution 10.1 Acids and Bases in Aqueous Solution Arrhenius Definition of Acids and Bases An acid is a substance that gives hydrogen ions, H +, when dissolved in water. In fact, H + reacts with water and produces

More information

A strong acid is completely protolysed

A strong acid is completely protolysed Strong acid A strong acid is completely protolysed Ex. 0.16 mol HCl to 1 liter H 2 O (=0.16 M) [H 2 O] = 55,6 M 1. Set up the reaction. HCl is a strong acid. 2. Amount acid resp. base before and after

More information

Chapter 8 Educational Goals

Chapter 8 Educational Goals Chapter 8 Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether the reactants or products are predominant.

More information

Full file at Chapter 2 Water: The Solvent for Biochemical Reactions

Full file at   Chapter 2 Water: The Solvent for Biochemical Reactions Chapter 2 Water: The Solvent for Biochemical Reactions SUMMARY Section 2.1 Summary Water is a polar molecule, with a partial negative charge on the oxygen and partial positive charges on the hydrogens.

More information

Water. Water participates in H-bonding with biomolecules.

Water. Water participates in H-bonding with biomolecules. Water Most biochemical reactions occur in an aqueous environment. Water is highly polar because of its bent geometry. Water is highly cohesive because of intermolecular hydrogen bonding. Water participates

More information

Chapter 8 Acid-Base Equilibria

Chapter 8 Acid-Base Equilibria Chapter 8 Acid-Base Equilibria 8-1 Brønsted-Lowry Acids and Bases 8-2 Water and the ph Scale 8-3 The Strengths of Acids and Bases 8-4 Equilibria Involving Weak Acids and Bases 8-5 Buffer Solutions 8-6

More information

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base

Acid-Base Equilibria. 1.NH 4 Cl 2.NaCl 3.KC 2 H 3 O 2 4.NaNO 2. Solutions of a Weak Acid or Base Acid-Base Equilibria 1 Will the following salts be acidic, basic or neutral in aqueous solution? 1.NH 4 Cl.NaCl.KC H O 4.NaNO A = acidic B = basic C = neutral Solutions of a Weak Acid or Base The simplest

More information

Acids, Bases and the Common Ion Effect. More quantitative. Continued [F - ] = M. Consider the following acid equilibrium of a weak acid:

Acids, Bases and the Common Ion Effect. More quantitative. Continued [F - ] = M. Consider the following acid equilibrium of a weak acid: Acids, Bases and the Common Ion Effect Consider the following acid equilibrium of a weak acid: HF + H O H 3 O + + F - K a = [H 3 O + ][F - ] [HF] By LeChatelier s principle, we predict the HF dissociation

More information

Chemistry. Friday, April 27 th Monday, April 30 th, 2018

Chemistry. Friday, April 27 th Monday, April 30 th, 2018 Chemistry Friday, April 27 th Monday, April 30 th, 2018 Do-Now: BrainPOP: Acids & Bases 1. Write down today s FLT 2. The ph scale ranges from to. 3. Which is more acidic: ph 3 or ph 6? 4. Which is more

More information

Introduction to Acids & Bases II. Packet #26

Introduction to Acids & Bases II. Packet #26 Introduction to Acids & Bases II Packet #26 1 Review I Svante Arrhenius was the first person to recognize the essential nature of acids and bases. 2 Review II Arrhenius postulated that: Acids produce hydrogen

More information

BCHS 3304: General Biochemistry I, Section 07553 Spring 2003 1:00-2:30 PM Mon./Wed. AH 101 1 http://www.uh.edu/sibs/faculty/glegge Instructor: Glen B. Legge, Ph.D., Cambridge UK Phone: 713-743-8380 Fax:

More information

ACID-BASE PHYSIOLOGY. Dr. Ana-Maria Zagrean

ACID-BASE PHYSIOLOGY. Dr. Ana-Maria Zagrean ACID-BASE PHYSIOLOGY 1 Dr. Ana-Maria Zagrean Acid-base physiology consists in all the processes inside the body which keep the H + concentration within normal values, thus maintaining the proper balance

More information

Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved.

Section 32 Acids and Bases. Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Section 32 Acids and Bases 1 Copyright (c) 2011 by Michael A. Janusa, PhD. All rights reserved. Acid-Base Concepts Acids and bases are among the most familiar and important of all chemical compounds. You

More information

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O.

1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H 2 O. 1) Write the Brønsted-Lowry reaction for weak acid HCN reacting with H O. HCN + H O º H O + + CN ) Write the Brønsted-Lowry reaction for weak base NH reacting with H O NH + H O º OH + NH + ) Using the

More information

ACID BASE EQUILIBRIUM

ACID BASE EQUILIBRIUM ACID BASE EQUILIBRIUM Part one: Acid/Base Theories Learning Goals: to identify acids and bases and their conjugates according to Arrhenius and Bronstead Lowry Theories. to be able to identify amphoteric

More information

I. Acids & Bases. A. General ideas:

I. Acids & Bases. A. General ideas: Acid-Base Equilibria 1. Application of equilibrium concepts. 2. Not much else new in the way of theory is presented. 3. Specific focus on aqueous (H O is 2 solvent) systems. 4. Assume we are at equilibrium

More information

Chapter 9 Aqueous Solutions and Chemical Equilibria

Chapter 9 Aqueous Solutions and Chemical Equilibria Chapter 9 Aqueous Solutions and Chemical Equilibria At equilibrium, the rate of a forward process or reaction and that of the reverse process are equal. 9A The chemical composition of aqueous solutions

More information

Equilibrium constant

Equilibrium constant Equilibrium constant Equilibrium constant Many reactions that occur in nature are reversible and do not proceed to completion. They come to an equilibrium where the net velocity = 0 The velocity of forward

More information

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College

Proton Transfer Acids - Base. Dr. Fred Omega Garces Chemistry 201. Miramar College 16.2 Acids Base Proton Transfer Dr. Fred Omega Garces Chemistry 201 Miramar College Important Notes: K a when H 3 O + is produced, K b when OH is produced 1 Acids Bases; Proton Transfer BrønstedLowry AcidsBases

More information

continuing education Acid-Base Review

continuing education Acid-Base Review continuing education Acid-Base Review James P. Dearing, B.S., C.C.P. In the normal, healthy individual the acid-base balance within the body is remarkably constant. For example, arterial blood, drawn from

More information

Understanding the shapes of acid-base titration curves AP Chemistry

Understanding the shapes of acid-base titration curves AP Chemistry Understanding the shapes of acidbase titration curves AP Chemistry Neutralization Reactions go to Completion Every acidbase reaction produces another acid and another base. A neutralization reaction is

More information

Chem 1102 Semester 1, 2011 ACIDS AND BASES

Chem 1102 Semester 1, 2011 ACIDS AND BASES Chem 1102 Semester 1, 2011 ACIDS AND BASES Acids and Bases Lecture 23: Weak Acids and Bases Calculations involving pk a and pk b Strong Acids and Bases Lecture 24: Polyprotic Acids Salts of Acids and Bases

More information

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter

Aqueous solutions of acids have a sour Aqueous solutions of bases taste bitter Acid and Bases Exam Review Honors Chemistry 3 April 2012 Chapter 14- Acids and Bases Section 14.1- Acid and Base Properties List five general properties of aqueous acids and bases Properties of Acids Properties

More information

The body has three primary lines of defense against changes in hydrogen ion concentration in the body fluids.

The body has three primary lines of defense against changes in hydrogen ion concentration in the body fluids. ph and Nucleic acids Hydrogen Ion (H+) concentration is precisely regulated. The H+ concentration in the extracellular fluid is maintained at a very low level, averaging 0.00000004Eq/L. normal variations

More information

Chapter 2 Water: The Solvent for Biochemical Reactions

Chapter 2 Water: The Solvent for Biochemical Reactions Chapter 2 Water: The Solvent for Biochemical Reactions SUMMARY Section 2.1 Water is a polar molecule, with a partial negative charge on the oxygen and partial positive charges on the hydrogens. There are

More information

Chem 1046 Lecture Notes Chapter 17

Chem 1046 Lecture Notes Chapter 17 Chem 1046 Lecture Notes Chapter 17 Updated 01-Oct-2012 The Chemistry of Acids and Bases These Notes are to SUPPLIMENT the Text, They do NOT Replace reading the Text Book Material. Additional material that

More information

LECTURE #25 Wed. April 9, 2008

LECTURE #25 Wed. April 9, 2008 CHEM 206 section 01 LECTURE #25 Wed. April 9, 2008 LECTURE TOPICS: TODAY S CLASS: 18.1-18.2 NEXT CLASS: finish Ch.18 (up to 18.5) (1) 18.1 The Common Ion Effect basis of all Ch.18 = shift in eqm position

More information

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases

1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Chemistry 12 Acid-Base Equilibrium II Name: Date: Block: 1. Strengths of Acids and Bases 2. K a, K b 3. Ionization of Water 4. Relative Strengths of Brønsted-Lowry Acids and Bases Strengths of Acids and

More information

Acid Base Equilibria

Acid Base Equilibria Acid Base Equilibria Acid Ionization, also known as acid dissociation, is the process in where an acid reacts with water to produce a hydrogen ion and the conjugate base ion. HC 2 H 3 O 2(aq) H + (aq)

More information

Preparation of different buffer solutions

Preparation of different buffer solutions Preparation of different buffer solutions 1 - Buffers: - All biochemical reactions occur under strict conditions of the concentration of hydrogen ion. - Biological life cannot withstand large changes in

More information

Lecture 12. Acid/base reactions. Equilibria in aqueous solutions.

Lecture 12. Acid/base reactions. Equilibria in aqueous solutions. Lecture 12 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added

More information

Lecture Presentation. Chapter 16. Aqueous Ionic Equilibrium. Sherril Soman Grand Valley State University Pearson Education, Inc.

Lecture Presentation. Chapter 16. Aqueous Ionic Equilibrium. Sherril Soman Grand Valley State University Pearson Education, Inc. Lecture Presentation Chapter 16 Aqueous Ionic Equilibrium Sherril Soman Grand Valley State University The Danger of Antifreeze Each year, thousands of pets and wildlife species die from consuming antifreeze.

More information

Water, ph and pka. Lecture 2: Margaret A. Daugherty. Fall Water: What makes it so good for life? Solvent properties.

Water, ph and pka. Lecture 2: Margaret A. Daugherty. Fall Water: What makes it so good for life? Solvent properties. Lecture 2: Water, ph and pka Margaret A. Daugherty Fall 2004 Water: What makes it so good for life? Structure ice vs. water or more technically solid vs. liquid Solvent properties High heat capacity High

More information

Chapter 16 - Acids and Bases

Chapter 16 - Acids and Bases Chapter 16 - Acids and Bases 16.1 Acids and Bases: The Brønsted Lowry Model 16.2 ph and the Autoionization of Water 16.3 Calculations Involving ph, K a and K b 16.4 Polyprotic Acids 16.1 Acids and Bases:

More information

Ionic Equilibria. In the Brönsted Lowry classification, acids and bases may be anions such as HSO 4

Ionic Equilibria. In the Brönsted Lowry classification, acids and bases may be anions such as HSO 4 Ionic Equilibria Brönsted Lowry Theory According to the Brönsted Lowry theory, an acid is a substance, charged or uncharged, that is capable of donating a proton, and a base is a substance, charged or

More information

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY

Acids And Bases. H + (aq) + Cl (aq) ARRHENIUS THEORY Acids And Bases A. Characteristics of Acids and Bases 1. Acids and bases are both ionic compounds that are dissolved in water. Since acids and bases both form ionic solutions, their solutions conduct electricity

More information

Chapter 13 Acids and Bases

Chapter 13 Acids and Bases William L Masterton Cecile N. Hurley http://academic.cengage.com/chemistry/masterton Chapter 13 Acids and Bases Edward J. Neth University of Connecticut Outline 1. Brønsted-Lowry acid-base model 2. The

More information

6.02 Acids - Bases. Dr. Fred Omega Garces. Chemistry 100. Miramar College Acids - Bases. January 10

6.02 Acids - Bases. Dr. Fred Omega Garces. Chemistry 100. Miramar College Acids - Bases. January 10 6.02 Acids - Bases Dr. Fred Omega Garces Chemistry 100 Miramar College 1 10 Acids - Bases Acids-Bases Characteristics Acids (Properties) Taste Sour Dehydrate Substances Neutralize bases Dissolve metals

More information

The Chemistry of Acids and Bases

The Chemistry of Acids and Bases The Chemistry of Acids and Bases 1 Acid and Bases 4 Acid and Bases 2 Acids Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain metals to produce

More information

2. WATER : THE SOLVENT FOR BIOCHEMICAL REACTIONS

2. WATER : THE SOLVENT FOR BIOCHEMICAL REACTIONS 2. WATER : THE SOLVENT FOR BIOCHEMICAL REACTIONS 2.1 Water and Polarity Both geometry and properties of molecule determine polarity Electronegativity - The tendency of an atom to attract electrons to itself

More information

Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria

Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria Edexcel Chemistry A-level Topic 12 - Acid-Base Equilibria Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base Proton

More information

Water: The Solvent for Biochemical Reactions

Water: The Solvent for Biochemical Reactions Chapter 2 Water: The Solvent for Biochemical Reactions 11 SUMMARY Section 2.1 Section 2.2 Section 2.3 Section 2.4 Water is a polar molecule, with a partial negative charge on the oxygen and partial positive

More information

Introduction into Biochemistry. Dr. Mamoun Ahram Lecture 1

Introduction into Biochemistry. Dr. Mamoun Ahram Lecture 1 Introduction into Biochemistry Dr. Mamoun Ahram Lecture 1 Course information Recommended textbooks Biochemistry; Mary K. Campbell and Shawn O. Farrell, Brooks Cole; 7 th edition Instructors Dr. Mamoun

More information

Kotz 7 th ed. Section 18.3, pp

Kotz 7 th ed. Section 18.3, pp Lecture 15 Acid/base reactions. Equilibria in aqueous solutions. Titrations Kotz 7 th ed. Section 18.3, pp.821-832. In a titration a solution of accurately known concentration is added gradually added

More information

Advanced Placement Chemistry Chapters Syllabus

Advanced Placement Chemistry Chapters Syllabus As you work through the chapter, you should be able to: Advanced Placement Chemistry Chapters 14 16 Syllabus Chapter 14 Acids and Bases 1. Describe acid and bases using the Bronsted-Lowry, Arrhenius, and

More information

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species

A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species 3 ACID AND BASE THEORIES: A) Arrhenius Acids produce H+ and bases produce OH not always used because it only IDs X OH as basic species B) Bronsted and Lowry Acid = H + donor > CB = formed after H + dissociates

More information

Part 01 - Assignment: Introduction to Acids &Bases

Part 01 - Assignment: Introduction to Acids &Bases Part 01 - Assignment: Introduction to Acids &Bases Classify the following acids are monoprotic, diprotic, or triprotic by writing M, D, or T, respectively. 1. HCl 2. HClO4 3. H3As 4. H2SO4 5. H2S 6. H3PO4

More information

Chapter 15 - Acids and Bases Fundamental Concepts

Chapter 15 - Acids and Bases Fundamental Concepts Chapter 15 - Acids and Bases Fundamental Concepts Acids and Bases: Basic Definitions Properties of Acids Sour Taste React with active metals (Al, Zn, Fe) to yield H 2 gas: Corrosive React with carbonates

More information

AP Chemistry: Acid-Base Chemistry Practice Problems

AP Chemistry: Acid-Base Chemistry Practice Problems Name AP Chemistry: Acid-Base Chemistry Practice Problems Date Due Directions: Write your answers to the following questions in the space provided. For problem solving, show all of your work. Make sure

More information

Functional Genomics Research Stream. Lecture: February 24, 2009 Buffer & Reagent Production, ph

Functional Genomics Research Stream. Lecture: February 24, 2009 Buffer & Reagent Production, ph Functional Genomics Research Stream Lecture: February 24, 2009 Buffer & Reagent Production, ph Agenda State of the Union Acid / Base Theory Buffers in Physiology Buffers in the Laboratory Assignment Six

More information

Analytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS

Analytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS Analytical Chemistry Lecture III by/ Dr. Ekhlas Q. J. BUFFER SOLUTIONS Buffer solutions Definition Solutions which resist changes in ph when small quantities of acid or alkali are added. a solution that

More information

Chem 5 PAL Worksheet Acids and Bases Smith text Chapter 8

Chem 5 PAL Worksheet Acids and Bases Smith text Chapter 8 D.CHO3HE.KOHB.NHC.CHC3OHHCl3F.H.CHHCH3COG.H2HCHEM 5 PAL Worksheet Acids and Bases Fall 2017 Chem 5 PAL Worksheet Acids and Bases Smith text Chapter 8 Many substances in the body are acids and bases. Many

More information

OCR (A) Chemistry A-level Topic Acids, Bases and Buffers

OCR (A) Chemistry A-level Topic Acids, Bases and Buffers OCR (A) Chemistry A-level Topic 5.1.3 - Acids, Bases and Buffers Flashcards Define a Bronsted-Lowry acid Define a Bronsted-Lowry acid Proton donor Define a Bronsted-Lowry base Define a Bronsted-Lowry base

More information

Buffer Solutions. Buffer Solutions

Buffer Solutions. Buffer Solutions Buffer Solutions A buffer solution is comprised of a mixture of an acid (base) with its conjugate base (acid) that resists changes in ph when additional acid or base is added The Henderson-Hasselbalch

More information

The Chemistry of Acids and Bases

The Chemistry of Acids and Bases The Chemistry of Acids and Bases 1 Acid and Bases 2 Acid and Bases 3 Acid and Bases 4 Acids 5 Have a sour taste. Vinegar is a solution of acetic acid. Citrus fruits contain citric acid. React with certain

More information