Iodine Clock Method Lab Report

(.1063 KIO31) (1 mol KIO214 g) x 6 mol S2O41 mol KIO= .00298.04150= .259 M

As a group, we obtained our salt mixture of calcium chloride and potassium oxalate, and weighed the mixture. We were able to make an aqueous solution from the mixture and distilled water. We boiled and filtered off the solution, leaving the precipitate. Once the precipitate was dried overnight, it was weighed and the mass was measured. Then we calculated the moles of the precipitate.

sodium thiosulphate + hydrochloric acid = sodium chloride (salt) + sulphur + water + sulphur dioxide

1. Suppose that you have an unlimited supply of copper (II) sulfate to react with iron. How many moles of copper would be

Rate= k [I-]1[H2O2]. (2.13675*10-5 ) = k [0.015] [0.015] then solve for k. For this trial, k=0.09497.

Hypothesis: The stoichiometric ratio of the reactants in the chemical synthesis of the (2, 4-pentanedianato) iron (III) complex ion is 3:1.

1. The time for the phenolphthalein to turn from pink to colourless will be taken using the stopwatch.

thiosulfate anion needed to react with each mole of hypochlorite anion in the bleach sample.

7. In a procedure developed to determine the percent zinc in post 1982 pennies, 50 ml of an HCl solution was used to react (dissolve) all of the zinc in the penny. To ensure complete reaction, the solution contains twice as many moles of HCl that is actually needed. What concentration of HCl should be used?

The purpose of this experiment is to study ionic reactions, to be able to write balanced equations, and to be able to write net ionic equations for precipitation reactions.

Molarity for sol. # 2 = (0.0016 g/l)/(350.13 g/mol) = 4.6 × 10-6 moles/ l

These equations can only be carried out and be visible after the iodine has completely reacted with thiosulphate added – two moles of thiosulphate for every mole of iodine. Once all the thiosulphate has been used up in the reaction, the colour will start to appear.

The process was then repeated for the second reaction but using 1.00-mL of a 6.00-M phosphoric acid solution and 4.00-mL of a 3.00-M sodium hydroxide solution.

In this experiment, a sample of K2S2O8 was prepared by the electrolysis of an aqueous solution of H2SO4 and K2SO4. The peroxodisulfate anion, S2O82-, was also observed for its ability to serve as a counterion for precipitation by preparing a copper (II) complex by reacting hydrated copper (II) sulfate with ammonium peroxodisulfate in the presence of pyridine. This same ability, coupled with its strong oxidizing ability allowed for stabilization of the unusual oxidation state of 2+ for silver which was observed by preparing an analogous silver (II) complex by reacting silver (I) nitrate with ammonium peroxodisulfate in the presence of pyridine. IR spectra for the three products were

In the fourth reaction, 15 mL of 6.0 M sulfuric acid was added to the copper (II) oxide while stirring. The balanced equation for this reaction is as follows: