calculate the change in boiling point for the NaCl solution (versus the pure water) and calculate of the boiling point of the solution. This is what is given: 100ml of H2O , density 1.00mg/ml , Initial temp 100°C for the water , 11.57g of NaCl (s) temp after NaCl is added to solution and brought to a rolling boil 104°C I performed 2 experiments. I first boiled 100ml of water and measured the temp at 100°C , then I got another beaker added 100ml of water and the 11.57g of NaCl and measured the temp at a rolling boil and got 104°C
I need help with my chemistry lab. I need to: calculate the change in boiling point for the NaCl solution (versus the pure water) and calculate of the boiling point of the solution.
This is what is given: 100ml of H2O , density 1.00mg/ml , Initial temp 100°C for the water , 11.57g of NaCl (s) temp after NaCl is added to solution and brought to a rolling boil 104°C
I performed 2 experiments. I first boiled 100ml of water and measured the temp at 100°C , then I got another beaker added 100ml of water and the 11.57g of NaCl and measured the temp at a rolling boil and got 104°C
These are my calculations so far: 11.57g NaCl * 1mol / 58.44g = 0.19798 mol NaCl
100ml = 100g of H2O = 0.100kg of H2O
molality = 0.19798 mol / 0.100 kg H2O = 1.98m
Tb= 1.980m * 2(i) * 0.512°C = 2.027°C
I don't know what to do after this and should I use the van't Hoff factor because some equations use it and others don't. And do I need to do another calculation for pure water and subtract the temps? I'm really confused. Thanks!
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