chemistry coursework
Experiment to determine the factors which affect the rate of oxidation of acidified potassium iodide solution by hydrogen peroxide. Plan As described in my preliminary introduction I intend to carry out an investigation to determine the factors which affect the rate of oxidation of acidified potassium iodide solution by hydrogen peroxide. H202 + 2KI + H2SO4 = K2SO4 + 2H2O + I2 I intend to vary the amount of potassium iodide entered into the 100cm³ solution (potassium iodide included in the solution). Potassium iodide is the independent variable. I plan to keep the volume of the solution at 100cm³. The dependant variable is time as this will vary depending on how quickly the solution turns a purple/black colour and the black cross marked on the paper below is not visible. I intended to keep the amount of sulphuric acid constantly at 40 cm³ also keeping the amount of hydrogen peroxide at 15 cm³ and the amount of special indicator at 5 cm³. In some cases where potassium iodide, sulphuric acid, hydrogen peroxide and the special indicator do not equal 100 cm³. Water is added to the solution to equal 100 cm³. . Potassium iodide is the independent variable therefore its volume must be changed in every solution. The apparatus required for this experiment consists of a stop clock, a 100 cm³ beaker, a 100 cm³ measuring cylinder, a 50 cm³ measuring cylinder, a 10 cm³
