i_like_sun Posted May 1, 2007 Posted May 1, 2007 Can someone tell me WHY, oh WHY, I am posting spray on my laptop in the middle of a 2 hour chemistry lab??? I really should get to my acid-base titrations.... Quote
Sherri Posted May 1, 2007 Posted May 1, 2007 Potenticolori-wha?? Now I know why I avoided chemistry. Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Colorimetric, today. Photometric was last Tuesday (% absorbance from an unkown Nickel Complex). My calculations got jacked becuase I ended up with a 70% water mass in my complex. The empirical formula was perfect....almost - [Ni(en)4 (H2O)34 (SO)4] See something wrong?????? Theres no way theres 34 waters attached to Nickel Ethylenediamine! Theres only space for 6 at a time! WTF? Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Fat Kid, yur just scared of us smart kids....... fatty! Quote
G-spotter Posted May 1, 2007 Posted May 1, 2007 Colorimetric, today. Photometric was last Tuesday (% absorbance from an unkown Nickel Complex). My calculations got jacked becuase I ended up with a 70% water mass in my complex. The empirical formula was perfect....almost - [Ni(en)4 (H2O)34 (SO)4] See something wrong?????? Theres no way theres 34 waters attached to Nickel Ethylenediamine! Theres only space for 6 at a time! WTF? ummm maybe it wasn't attached but rather you had a hydrous form with the extra water trapped in the crystal structure? Quote
counterfeitfake Posted May 1, 2007 Posted May 1, 2007 i hope you climb better than you chemistrate Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 That could be the case...... it still doesn't make sense though. I put aqueous Nickel Ethylenediamine in a dual exray absorbometer and found the % absorbance of actual nickel to be 0.085. Now thats pretty small, but it just means that it was a very dilute solution... From a calibration curve I made with 5 standard solutions, I could calculate the actual number of moles I was dealing with. From that, I calculated the mass % of each nickel, water, and sulfate ion. Then, I could come up with the empirical formula... Its weird, the data and calculations look solid....... just super F*****ed, thats all. Quote
fenderfour Posted May 1, 2007 Posted May 1, 2007 Fat Kid, yur just scared of us smart kids....... fatty! I've never been afraid of smart kids. They cry when you hit them. Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Well, I'll just squirt some HCL in your eye. That would hurt more than getting punched! Quote
kevbone Posted May 1, 2007 Posted May 1, 2007 Can someone tell me WHY, oh WHY, I am posting spray on my laptop in the middle of a 2 hour chemistry lab??? Its called addiction. We all have it. Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Can someone tell me WHY, oh WHY, I am posting spray on my laptop in the middle of a 2 hour chemistry lab??? Its called addiction. We all have it. I TOLD YOU climbers all have addictive personalities! Quote
ivan Posted May 1, 2007 Posted May 1, 2007 Colorimetric, today. Photometric was last Tuesday (% absorbance from an unkown Nickel Complex). My calculations got jacked becuase I ended up with a 70% water mass in my complex. The empirical formula was perfect....almost - [Ni(en)4 (H2O)34 (SO)4] See something wrong?????? Theres no way theres 34 waters attached to Nickel Ethylenediamine! Theres only space for 6 at a time! WTF? ummm maybe it wasn't attached but rather you had a hydrous form with the extra water trapped in the crystal structure? easily fixed by remodulating the emmiter array to pulse a tacheon beam Quote
catbirdseat Posted May 1, 2007 Posted May 1, 2007 That could be the case...... it still doesn't make sense though. I put aqueous Nickel Ethylenediamine in a dual exray absorbometer and found the % absorbance of actual nickel to be 0.085. Now thats pretty small, but it just means that it was a very dilute solution... From a calibration curve I made with 5 standard solutions, I could calculate the actual number of moles I was dealing with. From that, I calculated the mass % of each nickel, water, and sulfate ion. Then, I could come up with the empirical formula... Its weird, the data and calculations look solid....... just super F*****ed, thats all. Do a Karl Fischer titration to find out how much water there is. Dry under mild condition to drive off adsorbed water and repeat your nickel analysis. Quote
foraker Posted May 1, 2007 Posted May 1, 2007 Colorimetric, today. Photometric was last Tuesday (% absorbance from an unkown Nickel Complex). My calculations got jacked becuase I ended up with a 70% water mass in my complex. The empirical formula was perfect....almost - [Ni(en)4 (H2O)34 (SO)4] See something wrong?????? Theres no way theres 34 waters attached to Nickel Ethylenediamine! Theres only space for 6 at a time! WTF? When in doubt, blame a pre-med. Quote
archenemy Posted May 1, 2007 Posted May 1, 2007 That could be the case...... it still doesn't make sense though. I put aqueous Nickel Ethylenediamine in a dual exray absorbometer and found the % absorbance of actual nickel to be 0.085. Now thats pretty small, but it just means that it was a very dilute solution... From a calibration curve I made with 5 standard solutions, I could calculate the actual number of moles I was dealing with. From that, I calculated the mass % of each nickel, water, and sulfate ion. Then, I could come up with the empirical formula... Its weird, the data and calculations look solid....... just super F*****ed, thats all. Do a Karl Fischer titration to find out how much water there is. Dry under mild condition to drive off adsorbed water and repeat your nickel analysis. I was totally going to say that. That post should be subtracted from your total and added to mine. Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Colorimetric, today. Photometric was last Tuesday (% absorbance from an unkown Nickel Complex). My calculations got jacked becuase I ended up with a 70% water mass in my complex. The empirical formula was perfect....almost - [Ni(en)4 (H2O)34 (SO)4] See something wrong?????? Theres no way theres 34 waters attached to Nickel Ethylenediamine! Theres only space for 6 at a time! WTF? When in doubt, blame a pre-med. Yeah, you pretty much CAN blame us pre-medies for everything! For the most part we are just a bunch of assholes trying to fuck each other over so we get the highest GPA possible... For that reason alone I don't trust doctors! I'm not a super high achieving pre-meddy though.. I'm not even sure my GPA will allow me to get into school. I'm just a massive nerd who likes to suffer, thats all. Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 easily fixed by remodulating the emmiter array to pulse a tacheon beam mmmm... Do you think the Borg would do that? I'll give it a wee try captain! Quote
i_like_sun Posted May 1, 2007 Author Posted May 1, 2007 Potenticolori-wha?? Now I know why I avoided chemistry. Hey Sherri, yeah, definately a good move on avoiding chem! I think everyone just has their own idea of what is interesting. I've been avoiding english lit. forever, and dont' plan on changing that..... numbers are just cooler than idiots like us Spray folk rambling. Drawing and painting are cool though. Quote
fenderfour Posted May 1, 2007 Posted May 1, 2007 (edited) Well, I'll just squirt some HCL in your eye. That would hurt more than getting punched! Why don't you just get a gun and shoot everybody in the classroom instead? EVERYBODY PANIC!!!! Edited May 1, 2007 by fenderfour Quote
ClimbingPanther Posted May 2, 2007 Posted May 2, 2007 Well, I'll just squirt some HCL in your eye. That would hurt more than getting punched! weak. use pirahna. Quote
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