Iodide Oxidation by Hydrogen Peroxide

In summary, the conversation discusses the preparation of various solutions for a chemistry lab, including a buffered iodide solution, a 0.025M thiosulfate solution, and a peroxide solution. The mixtures of these solutions are then combined and cooled on ice before adding peroxide. The conversation also mentions questions about calculating the moles of sodium thiosulfate reacted and the concentration of a solution containing a certain number of moles of thiosulfate.
  • #1
buzzingbee
3
0
In my chemistry lab we prepared the following solutions:
Buffered Iodide Solution
25 mL acetic acid/sodium acetate buffer
6mL of 0.5 % starch solution
6 mL of 1.0M KI
fill to the 250 mL mark with distilled water

0.025M Thiosulfate Solution
5 ml of 1 M Na2S2O3
fill to the 200 ml mark with distilled water

Peroxide Soution
30ml of 1 M H2O2
fill to the 150 ml mark with distilled water

Then mixing these solutions together:
Mixture 1:
Buffered Iodide 40ml
Thiosulfate Solution 10ml
Distilled Water 10 ml

Mixture 2:
Buffered Iodide 40ml
Thiosulfate Solution 10ml
Distilled Water 20ml

Mixture3:
Buffered Iodide 40ml
Thiosulfate Solution 10ml

Mixture 4:
Buffered Iodide 40ml
Thiosulfate Solution 5 ml
Distilled Water 5ml

Separately put each beaker into ice water and measure the following amounts of peroxide solution separately into the container of ice:
Mixture 1: 20ml
Mixture 2: 10ml
Mixture 3: 30ml
Mixture 4: 30ml
when the two flasks have cooled on ice below 3°C add the peroxide
time as soon as you add peroxide into the flask

I am unsure for my lab questions what values to use for each trial to calculate the moles of sodium thiosulfate reacted? and how to calculate the mol/L H2O2 reacted
 
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  • #2
Strangest lab I've ever seen.
 
  • #3
buzzingbee said:
0.025M Thiosulfate Solution
5 ml of 1 M Na2S2O3
fill to the 200 ml mark with distilled water

How many moles of thiosulfate in 5 mL of 1M solution?

What is the concentration of solution that contains this number of moles of thiosulfate in 200 mL?
 
  • #4
wouldn't the concentration be 1 M
 
  • #5
No. Don't guess, try to calculate, following exactly questions as I listed them. This is mostly a simple plug and chug - use the definition of the concentration rearranged to isolate thing that you want to calculate.
 

1. What is the purpose of iodide oxidation by hydrogen peroxide in scientific studies?

The purpose of iodide oxidation by hydrogen peroxide is to study the kinetics and mechanism of the reaction. It is also used in analytical chemistry to determine the concentration of hydrogen peroxide in a solution.

2. How does iodide oxidation by hydrogen peroxide occur?

The reaction between iodide and hydrogen peroxide occurs in two steps. First, the hydrogen peroxide oxidizes iodide to iodine. Then, the iodine reacts with more hydrogen peroxide to form iodate ions.

3. What factors can affect the rate of iodide oxidation by hydrogen peroxide?

The rate of iodide oxidation by hydrogen peroxide can be affected by the concentration of reactants, temperature, pH, and the presence of catalysts. Light can also speed up the reaction due to the photolysis of hydrogen peroxide.

4. How is the rate of iodide oxidation by hydrogen peroxide determined?

The rate of the reaction can be determined by measuring the change in concentration of either the reactant (iodide) or the product (iodate). This can be done using spectrophotometry or titration methods.

5. What are some practical applications of iodide oxidation by hydrogen peroxide?

Iodide oxidation by hydrogen peroxide has practical applications in industries such as water treatment, food processing, and pharmaceuticals. It is also used in the production of certain chemicals and in the detection of explosives.

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