reaction with the analyte. In this experiment‚ the oxidation of iodide (I-) to produce iodine (I2) is taken into consideration. The use of this concept in a redox titration is called iodometry. Iodimetry‚ on the other hand‚ deals with the reduction of I2 into I-. Between these two methods‚ iodometry is more popular because it is more efficient to conduct due to the presence of more oxidizing agents strong enough to react with the iodide. The copper concentration of an unknown copper sample was determined
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Measure the potassium iodide. Weigh out approximately 2 g of solid KI. This amount is a large excess over that which is needed. 3. Oxidize the iodide ion with hypochlorite ion. Using a graduated cylinder‚ transfer 25 mL of the dilute bleach into an Erlenmeyer flask. Add the KI and about 25 mL of distilled water. Swirl to dissolve
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zinc and iodine‚ and comparing their total to the mass of the zinc iodide product plus the excess zinc. The total mass of the reactants was determined by subtracting the mass of the empty beaker from the mass of the beaker with initial amounts of zinc and iodine in it. The mass of the reactants was 5.266g. The mass of the products was obtained by adding the mass of zinc iodide with the mass of the excess zinc. The mass of zinc iodide was 2.412g. The mass of excess zinc was 2.695g. 2.142g was then added
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other (groups of twos) in test tubes to test which reaction will result in an insoluble solid. See method for more detail. It is expected that the following compounds will form precipitates Silver Sulphate‚ Copper Hydroxide‚ Copper Iodide‚ Silver Hydroxide‚ Silver Iodide‚ Cobalt Hydroxide and two Silver Chlorides. This was worked out by completing the double displacement reactions and using a table of solubilities. (See appendix one & two) In any experiment involving chemicals a hard wearing plastic
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Please refer to General Chemistry Laboratory Experiments‚ Volume 1‚ 2011‚ by Robert Tatz and Judith Casey‚ Exp 4‚ pages 32-33‚ for proper procedure. Data See attached sheet. Report Questions 1. The charge on an iodide ion is -1. It is determined by the formula for potassium iodide in which neither element has subscripts. This signifies that they have equal amount charges and cancel each other out. The charge of the lead ion is +2‚ as shown on the periodic
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halogen ion that is displaced from the carbon atom is called the leaving group‚ and the overall reaction is called a nucleophilic substitution reaction. Procedure: 1. Sodium Iodide in Acetone. Acetone‚ with a dielectric constant of 21‚ is a relatively nonpolar solvent that will readily dissolve sodium iodide. The iodide ion is an excellent nucleophile‚ and the nonpolar solvent‚ acetone‚ favors the Sn2 reactions; it does not favor ionization of the alkyl halide. The extent of reaction can be observed
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reactivities of different alkyl halides with two different reagents; sodium iodide in acetone and silver nitrate in ethanol. Below the reaction equations 1. RX+NAIRI+NAX (X=Cl or Br) in the presence of acetone 2. RX+AgNO3+EtOHROEt+AgX+HNO3 We used three substrates primary secondary and tertiary compounds are 1-bromobutane‚ 2-bromobutane and 2-bromo-2-methylpropane respectively to react with the two nucleophiles that are sodium iodide with acetone solvent and silver nitrate with ethanol solvent. Based
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methods is the iodine-thiosulfate titration procedure. Iodide ion‚ I-‚ is easily oxidized by almost any oxidizing agent (It has many electrons to lose!). In an acid solution‚ hypochlorite ions oxidize iodide ions to form iodine‚ I2. The iodine that forms is then titrated with a standard solution of sodium thiosulfate. The analysis takes place in a series of steps: 1.Acidified iodide ion is added to hypochlorite ion solution‚ and the iodide is oxidized to iodine. 2H+ (aq) + ClO-(aq) + 2I-(aq)
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prepare the Grignard reagent methylmagnesium iodide and react it with benzoin to form the 3o alcohol 1‚2-diphenyl-1‚2-propanediol‚ through an addition reaction pathway. Introduction: Grignard reagents are alkyl or aryl-magnesium halides that act as the nucleophile in Grignard reactions‚ where ketones are reacted with the reagent‚ then treated with acid to produce an alcohol. In the case of this experiment‚ methylmagnesium iodide was created from methyl iodide and magnesium metal. It acted as the Grignard
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keep it completely dry. Later the dried substance along with a colored solution ‚ the grey solid leftover‚ white product in H2O‚ standard zinc metal‚ standard iodine solid‚ standard zinc Iodide dissolved in water and standard zinc ion- Iodide ion- Iodine- Triiodide ion in H2O were tested for Iodine(I2)‚ Iodide‚ Triiodide‚ Zinc ion(Zn 2+) and Zinc metal. Then we dissolved some of the white substance with deionized water and made an electrolysis apparatus with a 9.38V battery. We then dried
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