Procedure- The procedure for this lab includes many simple steps and a few different things we are testing. Our first Procedure was to combine water and salt to see what kind of reaction it would make. First we fill the graduated cylinder with 100 ml of water. We then measured 1.0 grams of table salt on a balance to get an accurate amount. After, we took the measured amount of salt and poured it into the water filled beaker. Lastly, we watched and recorded the reaction.
b) Spray a small amount of distilled water on the electrical leads of the conductivity apparatus. Insert the electrical leads of the conductivity apparatus into the beaker.
19. Stir the solution with a toothpick and observe any changes. Measure the pH of the new solution and record into Table 2.
The first step that needed to be done in this experiment was adding hydrochloric acid (HCl)
* First, combine 10.0 mL of the Ba(OH)2 solution with 50 mL of distilled water. Then, measure out 60 mL of 0.100 M H2SO4. Set up a conductivity probe and open programs by connecting to logger pro. After that, start to titrate with increments of 1.0 mL. Keep titrating with smaller increments until it is pretty close to the 100 microsiemens/cm mark.
so that the conductometric data were treated by Fuoss–Shedlovsky method  by using a computer program, to evaluate the ion-pair association constants of the studied salts and to re-evaluate the limiting molar conductance (Λ0), where they proposed the following equation:
The diagram below shows a labelled circuit which is used for the experiment. This is set up by collecting all equipment needed and attaching the DC power supply to the ammeter with a wire this is all connected to the anode and cathode with a red and black wire to differentiate between the two electrodes. The two electrodes are shown to be placed in a beaker of copper sulphate
The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.
1. Using the information provided in the Introduction and your observations from Part 1, hypothesize as to the type of electrolyte the following solutions would be. Justify the hypothesis from a chemical standpoint.
For example, sodium chloride is an ion because it components are oppositely charged which are Na+ and Cl-. The ions were measured in the lab by the conductivity meter. There is a straight direct relationship between salinity and conductivity which means that whenever salinity increases conductivity also increases and when salinity decreases conductivity also decreases. If there is less water, but still the same amount of ions, I would expect that conductivity would increase, as there is more ions in less amount of space which makes the salinity increase and as a result the conductivity also increases. The standard curve is a curve that is used to determine the value of unknown quality. It is used for this lab to determine the salinity of the Seven River estuary. The standard curve enabled us to experimentally determine the relationship between two quantities which are the salinity and conductivity. The dilution was made by putting together each part of the sample which were the distilled water and the salted water. We the distilled water in a separate breaker and the NaCl solution in another breaker. We also had a measuring cylinder to use when we were testing the samples. Then, we start using doing each sample that we had and after measuring them we measure the conductivity by the conductivity meter by plugging the conductivity probe in the breaker to get the amount of conductivity in each sample Furthermore, we had to