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Q:A 5.0 mL of solution of H2O2 liberates 0.508 g of iodine from acidified KI solution.Calculate the strength of H2O2 solution in terms of volume strength at STP.?
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Q:A 5.0 mL of solution of H2O2 liberates 0.508 g of iodine from acidif...
Calculation of Volume Strength of H2O2 Solution

Given:
- Volume of H2O2 solution = 5.0 mL
- Mass of iodine liberated = 0.508 g
- Acidified KI solution used for the reaction

Step 1: Calculation of Number of moles of Iodine
The reaction between H2O2 and KI is as follows:
H2O2 + 2KI + 2H+ → I2 + 2K+ + 2H2O
From the reaction, it is clear that 1 mole of H2O2 liberates 1 mole of I2.
Therefore, the number of moles of I2 liberated can be calculated as follows:
Molar mass of I2 = 2 x atomic mass of I = 2 x 126.9 = 253.8 g/mol
Number of moles of I2 = Mass of I2 liberated / Molar mass of I2
= 0.508 / 253.8
= 0.002 mol

Step 2: Calculation of Volume Strength of H2O2 Solution
Volume strength is defined as the volume of H2O2 required to liberate 1 mL of oxygen at STP (Standard Temperature and Pressure).
1 mole of H2O2 liberates 1 mole of oxygen.
1 mole of any gas at STP occupies 22.4 L.
Therefore, the volume of oxygen liberated by 0.002 moles of H2O2 at STP can be calculated as follows:
Volume of oxygen liberated = 0.002 x 22.4
= 0.0448 L
= 44.8 mL
As 44.8 mL of oxygen is liberated by 0.002 moles of H2O2, the volume strength of H2O2 solution can be calculated as follows:
Volume strength of H2O2 solution = (44.8 / 5) x 1000
= 896 mL/L
= 896 volume strength

Therefore, the strength of H2O2 solution in terms of volume strength at STP is 896.
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Q:A 5.0 mL of solution of H2O2 liberates 0.508 g of iodine from acidif...
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Q:A 5.0 mL of solution of H2O2 liberates 0.508 g of iodine from acidified KI solution.Calculate the strength of H2O2 solution in terms of volume strength at STP.?
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