Experiment IV Solubility of Dissolved Oxygen Purpose To demonstrate the effect of partial pressure‚ temperature and salinity on the solubility of dissolved oxygen and to demonstrate the interference of nitrite in dissolved oxygen analysis by the Winkler Method. To demonstrate the use of the oxygen electrode and the difference between activity and concentration. References 1. Mancy‚ K. H.‚ Jaffe‚ T.‚ "Analysis of Dissolved Oxygen in Natural and Waste Water‚" USDHEW Public Health Service
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Synthesis Procedure 1 -1.0 Introduction A Cobalt-Amine-Halide compound is synthesized from cobalt (II) chloride hexahydrate. An orange-tinted solid is produced and is considered to be unknown since the specific ligand amounts are unknown. By determining the percent composition of various elements and compounds in the unknown‚ its true identity can be predicted. Chloride‚ ammonia‚ and cobalt are three examples of percent compositions determined to help narrow the selection of possible unknowns
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SSN COLLEGE OF ENGINEERING DEPARTMENT OF CHEMICAL ENGINEERING V Semester – CH 2307 TECHNICAL ANALYSIS LAB -2010 INDEX SHEET CYCLE ONE Date of Condn. Date of Subn. Sign 1 Estimation of COD of the given sample of water. 2 Estimation of Manganese in the given pyrolusite ore. 3 Estimation of Magnesium by EDTA method. 4 Estimation of purity of drug using pH meter. 5 Estimation of Ammonia in ammonium salts. 6 Polarimetric estimation of sugar
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w w ap eP m e tr .X w om .c s er June 2003 INTERNATIONAL GCSE MARKING SCHEME MAXIMUM MARK: 40 SYLLABUS/COMPONENT: 0620/01 CHEMISTRY (Multiple Choice) Page 1 Mark Scheme IGCSE EXAMINATIONS – June 2003 Syllabus 0620 Question Number Key Question Number Key 1 2 3 4 5 C B A D A 21 22 23 24 25 B D A B D 6 7 8 9 10 C A A B C 26 27 28 29 30 B D D D B 11 12 13 14 15 B D C D
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Experiment 3 ACID – BASE TITRATION I. Objectives * Determine the purity of Potassium Acid Phthalate * To titrate effectively II. Data and Results A. Measurement of the Relative Strengths of Acid and Base B. Standardization of Sodium Hydroxide Primary Standard used: Potassium Acid Phthalate (KHP) Formula Mass of Primary Standard: 204.22 g/mol% % Purity of Primary Standard: 99.9% Trials | 1 | 2 | 3 | Mass of Std. KHP | 0.7059 | 0.7345 | 0.7189 | % Purity KHP
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are examples of each type of acid undergoing a reaction with sodium hydroxide. Monoprotic: HCl(aq) + NaOH(aq) → H2O(l) + NaCl(aq) Diprotic: H2SO4(aq) + 2 NaOH(aq) → 2 H2O(l) + Na2SO4(aq) Triprotic: H3PO4(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3PO4(aq) Any acid that has more than one proton that undergoes a reaction with a base is called a polyprotic acid. Citric acid is a weak‚ polyprotic acid that undergoes the following reaction with sodium hydroxide. H3C6H5O7(aq) + 3 NaOH(aq) → 3 H2O(l) + Na3C6H5O7(aq)
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to 318K at normal atmospheric pressure. It was found that the solubility of potassium hydrogen tartrate decreases with a decrease in temperature and consequently a smaller volume of sodium hydroxide is needed to neutralize it. The molar solubility of potassium hydrogen tartrate was calculated from the volume of sodium hydroxide used. The experimental result for the solubility at 298K was compared to literature data‚ to verify the reliability of this method. The experimental value is in agreement with
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(Part A and B) ABSTRACT The purpose of this experiment is to prepare a standard solution of potassium hydrogen phthalate and use titration to perform an acid/base reaction between the potassium hydrogen phthalate and sodium hydroxide to standardize approximately 0.10 M sodium hydroxide solution. To prepare the Potassium Hydrogen phthalate‚ a 2.00 grams of KHP was measured to an accurate measurement of 1.980 grams. A total of 100 mL of water was mixed with the KHP solution in the volumetric flask
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tabs and through a back titration‚ we were able to find out how much acid was needed to neutralize two tablets of TUMS. In the first process of the titration‚ we added excess HCl and then we had to back titrate it by adding NaOH. We had to do a standardization test because the NaOH has a high reactivity and that could cause a small change. The NaOH solution was supposed to have a molar concentration of .5 however when we standardized the solution we found the actual molarity of the solution to be .4761
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Objective The rate constant of the depolymerization of diacetone alcohol via basic catalysis was determined by monitoring the change in volume as a function of time at constant temperature of a pseudo first order reaction where the species in excess was sodium hydroxide. This was accomplished by using a dilatometer as the apparatus and following both methods: isolation and initial rates in conjunction. Introduction Depolymerization is the process in which a compound is converted into one of a smaller
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