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higherme
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Homework Statement
Anhydrous liquid hydrazine is used as a rocket propellant. It is a highly hazardous, toxic, carcinogenic substance.
The %-purity of a sample, presumed to be neat anhydrous hydrazine, is to be determined by iodimetric titration.
First, the titrant iodine (+potassium iodide) solution (I2 + I− ⇌ I3−) was standardized.
61.24 mL of iodine solution was required to titrate 0.2802 g of As2O3 dissolved in a sodium hydroxide solution adjusted to near neutral pH.
H2AsO3− + I3− + 4H2O → HAsO42− + 3I− + 3H3O+
What is the molarity of the standard solution?
The Attempt at a Solution
I have to find the concentration of the standard which is iodine. I know that it took 61.24ml of that soln to titrant the analyte As2O3. So, my attempt is to take the mass of As2O3 that was used and convert that to moles using the molar mass.. then this moles will be the same as moles of iodine that reacted. from there i can find concentration...
BUT, what I don't get is the equation given... it started with H2AsO3... is that what the analyte is? or is it a different compound.. since the 2 after the As is missing