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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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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[H3O+] = (( Ka1 Ka2) (approx.) (eq 13-4) |Example: Calculate the hydronium ion concentration of a 0.100 M NaHCO3 solution. | |We first examine the assumptions leading to Equation 13-4. The dissociation constants for H2CO3 are Ka1 = 1.5e-4 and Ka2 = | |4.69e-11. | |[H3O+] = ((1.5e-4 x 4.69e-11) = 8.4e-8 M
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which marked the endpoint of this titration. As a result‚ the concentration of the NaOH solution was found to be 0.124 M with a standard deviation of 0.004 M. In the second titration‚ the goal was to use both an acid’s formula weight and acid dissociation equilibrium constant (pKa) value to determine the identity of this unknown acid. Both values were found by preparing the unknown acid solution‚ preparing a buret‚ titrating the acid solution with the strong basic NaOH solution from the previous
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Laboratory report Shae Aquino Chemistry 161L February 25‚ 2014 Conductivity of Solutions of Ionic and Covalent Compounds Purpose The purpose of this experiment was to use electrical conductivity on ionic‚ molecular acids‚ and covalent compounds in order to determine the properties of each compound. Introduction In chemistry‚ the term of an aqueous solution is defined as a substance that is soluble in water. For example‚ sodium chloride (NaCl) dissolves in water‚ or other
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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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In the reverse reaction‚ NH4+‚ the conjugate acid‚ loses a proton‚ forming our base NH3. Acid-Base Strength and Conjugate: The relative strength of acids is often described in terms of an acid-dissociation equilibrium constant‚ Ka. Generic Equation: HA(aq) + H20(l) ↔ H3O+(aq) + A-(aq) Therefore‚ Ka = [H3O+][A-]/HA When a strong acid dissolved in water‚ the acids reacts extensively with water to form H3O+ and A- ions. The product of the concentrations
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dissociated in water) with a PH probe. After we got the PH‚ we could find out the concentration of H+ by applying the relationship pH = -log [H+]. Having the determined value of [H+] of a weak acid with a known molar concentration [HA]‚ The acid dissociation constant‚ Ka‚ can be determined according to Ka = [H+][A-] /[HA]. In “Part B” experiment‚ we use a strong acid (HCl) and a weak acid (acetic acid) titrates with a strong base (NaOH). In both titrations‚ we will monitor the change in PH to determine
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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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