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A student uses 24.0 mL of a .550 M Na2S2O4 (sodium thiosulfate) solution to titrate a 10.0mL sample of bleach.
1. What is the mass % of NaOCl used in the bleach?
2. How many moles of sodium thiosulfate were used?
3. How many moles of iodine (I2) will react with this amount of sodium thiosulfate? Include the equation for this reaction
4. If all the sodium hypochlorite present in the sample of bleach was completely reacted to make the iodine, how many moles of sodium hypochlorite was used? Include the equation.
5. What is the mass % of sodium hypochlorite in the bleach? Assume a bleach density of 1.00 g/mL.
1. What is the mass % of NaOCl used in the bleach?
2. How many moles of sodium thiosulfate were used?
3. How many moles of iodine (I2) will react with this amount of sodium thiosulfate? Include the equation for this reaction
4. If all the sodium hypochlorite present in the sample of bleach was completely reacted to make the iodine, how many moles of sodium hypochlorite was used? Include the equation.
5. What is the mass % of sodium hypochlorite in the bleach? Assume a bleach density of 1.00 g/mL.