{[ promptMessage ]}

Bookmark it

{[ promptMessage ]}


LeChatelier's - NaCl to come out of solution because...

Info iconThis preview shows page 1. Sign up to view the full content.

View Full Document Right Arrow Icon
LeChatelier’s Principle Introduction - The goal of this experiment was to observe LeChatelier’s Principle in action. The principle states that if a system already at equilibrium is disturbed, the system will react so as to minimize the disturbance. Chemical Responsibility - Many of the chemicals present in this experiment are toxic and/or corrosive to the skin. The iron chloride, potassium thiocyanate, silver nitrate, ammonia, ammonium chloride, and hydrogen chloride must all be handled with care. All wastes are to be discarded in the properly labeled containers at the front of the room. Report Sheet/Sample Calculations- See report sheet. Discussion - Based on the data we collected, LeChatelier’s Principle could be observed at work in every situation we created. Adding HCl to saturated NaCl caused
Background image of page 1
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: NaCl to come out of solution because additional chloride ions were added, resulting in a shift to the reactants. Adding Fe3+ and NCS- to [FeNCS2+] both caused more [FeNCS2+] to be created, resulting in a much darker red solution. Adding Ag+ removed the SCN- ion and resulted in less [FeNCS2+], making the solution a lighter red. Adding more NH4 + to its system resulted in a colorless solution, indicating an acidic pH, as the reaction shifted left and less OH- ions were created. Conclusion-LeChatelier’s Principle is easily observed in a system that is disturbed at equilibrium. Based on a balanced formula, one can predict how the system will react to counter the disturbance and in which direction it will shift....
View Full Document

{[ snackBarMessage ]}

Ask a homework question - tutors are online