Ka‚ Acid Dissociation Constant and Kb‚ Base Dissociation Constant (Lesson Recap) Ka‚ Acid Dissociation Constant Ka- is the Keq for the dissociation for a weak acid. e.g Acetic Acid‚ when dissolved in H2O CH3COOH (aq) + H2O (l) (ACID) (BASE) CH3COO (aq) + H3O(l) (CONJ BASE) (CONJ ACID) CH3COOH (aq) + H2O(l) ↔ CH3COO (aq) + H3O(l) *ONLY weak acid and back can be reversible Equation for Ka : Keq= [CH3COO(aq)] [H3O(l)][CH3COOH(aq)] [H2O(l)] Keq x [H2O
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= 55.56 M K = 1.8 x 10-16 ; pKa = 15.74 pKa is the acid dissociation constant; low pKa (strong acid‚ high pKa (weak acid we can also write Kw = [H3O+][OH-] Kw = 10-14 In water‚ pH + pOH = 14 pH scale Strong Acids: Complete dissociation of the acid in water: HA ( H+ + A- note: H+ in H2O is hydrated (H3O+) K (Ka since it is an acid) is large (For complete dissociation‚ K = infinity; however there is some very tiny amount that is not
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Acid Rain Introduction: Titrations are often recorded on graphs called titration curves‚ which generally contain the volume of the titrant as the independent variable and the pH of the solution as the dependent variable (because it changes depending on the composition of the two solutions). The equivalence point on the graph is where all of the starting solution (usually an acid) has been neutralized by the titrant (usually a base). One can easily find the pKa of the monoprotic acid by finding
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gradually neutralizing the acid. The volume of base added can be determined by the difference in the initial and final volume marks on the buret. At a certain volume of added NaOH‚ all the KHP acid will be neutralized due to the large equilibrium dissociation constant (Kb) of the base. This point of titration is referred to as the equivalence point. Considering the 1:1 stoichiometry of this acid-base reaction NaOH(aq) + C6H4(COOH)(COOK) (aq) C6H4(COONa)(COOK)(aq) + H2O(l) the point of equivalence
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Unit Plan On Acids & Bases May 25‚ 2006 Table of Contents I. General Objectives Page 3 II. Learning Outcomes Page 4 III. Assessment‚ Grading & Resources Page 5 IV. Tending to different Learning styles Page 7 V. Schedule Page 8 VI. Appendix 1 Page 20 Acids and bases Unit plan Grade 12 General Objectives: ▪ Introduce pH‚ acid and base definition ▪ Discuss acid
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the acid dissociation constant (Ka) for the weak acid HX in aqueous solution is 3.01 × 10–5 mol dm–3. (i) Calculate the value of pKa for HX at this temperature. Give your answer to 2 decimal places. ............................................................................................................... ............................................................................................................... (1) (ii) Write an expression for the acid dissociation constant
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Chapter 13 Acids and Bases (Dr Chong Fai Kait) 1) A 7.0 103 M aqueous solution of Ca(OH) 2 at 25.0 °C has a pH of __________. A) 12.15 B) 1.85 C) 1.4 102 D) 7.1 1013 E) 11.85 Answer: A 2) The acid-dissociation constant at 25.0 °C for hypochlorous acid (HClO) is 3.0 108 . At equilibrium‚ the molarity of H 3 O in a 0.010 M solution of HClO is __________. A) 1.7 105 B) 0.010 C) 5.8 1010 D) 4.76 E) 2.00 3) Using the data in the table‚ which of the conjugate acids below is the weakest
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Using a primary standard to analyze acid and base solutions Acid-base titration Lab 13G Jake Shewchuk Lab 13C Dominique Genereux Purpose 13G: 1. To prepare a standard solution of oxalic acid and use it to standardize an unknown sodium hydroxide solution. Purpose 13C: 1. To titrate a hydrochloric acid solution of “unknown” concentration with standardized 0.5M sodium hydroxide. 2. To titrate a hydrochloric acid solution of “known” concentration
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beta 2- adrenoreceptors 1”. Atenolol has the molecular formula of C14H22N2O3. Its molecular mass is 266.3 grams and its IUPAC name is (RS)-4-(2-hydroxy-3-isopropylaminopropoxy) phenylacetamide. Its melting point 152-155 degrees Celsius‚ has a dissociation constant (pKa) of 9.6 at 24 degrees Celsius. It is soluble in water‚ ethanol and methanol but it is insoluble in ether 2.Atenolol can be synthesized in two parts. The first synthesis is with the reaction of phenol and formaldehyde to form the
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Structural and electronic effects Acids and Bases Acknowledgement Some material have been sourced from the following websites and books Reference • http://facstaff.gpc.edu/~matteya/organicppt/Ch2.ppt • http://atom.chem.wwu.edu/dept/facstaff/pavia/351pavia.html • www.fccj.us/chem1212/powerpoint/Ch17_Lewis_B.ppt • CH102 Course book • Organic Chemistry 7th Edition by John McMurry 2 Acids & Base Definitions Definition #3 – Lewis • Lewis acid - a substance that accepts an electron pair • All BrØnsted-Lowry
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