EXPERIMENT 2: COMMON-ION EFFECT AND BUFFERS MARVILE REA R. FERRER1 1DEPARTMENT OF MINING‚ METALLURGICAL & MATERIALS ENGINEERING‚ COLLEGE OF ENGINEERING UNIVERSITY OF THE PHILIPPINES‚ DILIMAN‚ QUEZON CITY 1101‚ PHILIPPINES DATE SUBMITTED: DECEMBER 13‚ 2012 DATE PERFORMED: DECEMBER 07‚ 2012 ______________________________________________________________________________________________________________ INTRODUCTION Monitoring the pH range of a laboratory reaction or a process is very
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CHLORIDE (KCL) AND POTASSIUM IODIDE (KI) IN WATER VARY WITH TEMPERATURE? AIM To observe solubilities of KCl and KI with water at different temperatures To compare the two solubility curves and discuss what might vary the solubility of different ionic compounds. THE VARIABLES DEPENDENT VARIABLE Temperature INDEPENDENT VARIABLE Amount of solute (KCl‚ KI) CONSTANTS Amount of the solvent (water)‚ pressure APPARATUS 100G OF POTASSIUM CHLORIDE 100G OF POTASSIUM IODIDE 10ML CYLINDER TEST TUBES
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(vi) Ion-induced dipole interactions [20(b)] In these interactions ion’s field induces a dipole moment in a molecule. If μ is the induced moment in a field E‚ ‘α’ is the polarizability (assumed to be constant)‚ then (26) (27) where FZ is the instantaneous force on the induced dipole (R >> δ) and the interaction energy at a given R‚ is (28) As the induced dipole is parallel to the field
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LAB 3.Ø.Ø: do ions combine in definite ratios PURPOSE The purpose of this investigation is to determine whether ions combine in definite ratios or not. To observe‚ and create a table of the different ions. QUESTION If copper (II) sulfate when mixed with sodium carbonate at different quantities combine to form ions in definite ratios. HYPOTHESIS / PREDICTION I believe that the ions will combine in definite ratios due to the fact that the valance electrons will not be changing throughout any
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UCD School of Chemical & Bioprocess Engineering CHEN20040 Chemical & Bioprocess Engineering Laboratory I Experiment: 1 Title: Reaction order of the oxidation of iodide by persulphate in neutral solution Name: Lab Partner: Group: Experiment Performed: Report Due: Report Submitted: Table of Contents Abstract Page 3 Materials and Methods 4 Results and Discussion 5 Conclusion 10 Report Questions 11 Appendices Appendix A. Experimental Data
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. ~.. r .. .‚III/!I.. ‚• •f t . ‚.‚;;;‚UUft Y f__ _ P_RO_O_O_c_1 PDS: 1-16 _DA_T_A_S_f5l~_T GU_IT_erl_t: SUperseI &10 l-10 Neme‚‚ . _ nrkc Gnphlte Anoryhout Gnphite Ctey Siticr Tdc Ilcrtrin ’ . -‚ _ OSHApcl CAS# . ‚. N.iosL 77t242-S 2.5 2.5 778?‚42-5 2‚5 2.5 [5’15" l?32-58-57 t4g0g60-? 0.051o lI 14t0?-96-6 2.0 2.0 9004-53-9 "Retpirablc fraction - .... ACSF t{v 2.5 2..5 l0 0.I 2.0 _ _‚ _ in mluesacprcsscd mg/m3 TotalDust I Respirablc dust IEYSfCIi
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1. When glucose‚ C6H12O6‚ is completely oxidized with excess oxygen‚ what are the products? A. H2O2 and CO2 B. H2O and CO2 C. H202 and CO D. H2O and CO 2. Which ion may form a scummy precipitate with ordinary soap? (soap has a negative charge) A. HCO3- B. CO32- C. Na+ D. Ca2+ 3. An element forms a basic oxide with the formula XO and a hydride with the formula XH2. The hydride reacts with water to give hydrogen gas. The element X could be? A. K B. Ca C. N D. O 4. Which metal reacts with concentrated
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Urea is produced in the liver from excess amino acids. Where are the substances excreted? Carbon dioxide is passed from the cells of respiring tissues into the blood stream. It is transported in the blood (mostly in the form of hydrogen carbonate ions) to the lung. In the lungs the carbon dioxide diffuses into the alveoli to be excreted as we breathe out. Urea is produced by breaking down excess amino acids in the liver. This process is known as deamination. The urea is then passed through the
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salts when reacted with (NH4)2CO3. The principle of periodicity applied to the results of this series of experiments. It helps‚ in trying to see the periodic pattern‚ to know the pattern that results when we do a separation and analysis of all metal ions. PROCEDURE Procedure A 1. 2 drops of 6 M HCl was added to 1 ml of the mixture of the metal cations. 2. The suspension was centrifuged for 1 minute as ppt. of chloride was formed. 3. 1 additional drop of 6 M HCl was added to the clear
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Purpose: To observe the characteristic colors produced when certain metallic ions are vaporized. Metallic Ion Color in Flame Na+ Light Orange K+ Pink / Orange Li Red Ca2+ Dark Orange Sr2+ Red Cu2 Green Co+2 Salmon Pink Ammonium Dichlorate Orange Sparks K2CR2O7 Orange Fe+1 No Reaction NaCl Orange Strantium Chloride Scarlet Red Ni+2 Dark Orange Copper Sulfate (solid) Green Fe+2
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