conductometric measurements Flashcards
Why did you get a difference in the voltage readings for the 0.01M acetic acid and 0.01M hydrochloric acid solutions using the “home-made” conductivity probe in the previous lab activity An Investigation of Electrochemical Reactions?
Hydrochloric acid is a strong acid, making it a strong electrolyte that will completely dissociate in water. Acetic acid is a weak acid, making it a weak electrolyte so it will only partially dissolve in water
Why is it critical not to change the spacing between the electrodes in a conductivity cell?
Because moving the farther apart increases the density
What is the equivalence point?
The point in a titration at which the amount of titrant added is just enough to completely neutralize the analyte solution. At the equivalence point in an acid-base titration, moles of base = moles of acid, and the solution only contains salt and water
Why is the potentiometric titration of acetic acid with ammonia considered infeasible?
Potentiometric titration is very sensitive to pH, leading to more errors. Acetic acid is a weak acid and ammonia is a weak base, so when the ammonia is added to the acetic acid the pH levels are hard to read
Explain the warning found on the extinguisher: DO NOT USE ON ELECTRICAL FIRES!
Regular fire extinguishers are water-based and water is a conductor, so if it were used on an electrical fire there would be a risk of electrocution
