There are three types of solutions we used in this lab, based on their electrical conductivity properties, we can classify them as strong electrolyte, non-electrolyte and weak electrolyte. Distilled Water, CH3OH and C2H6O2 are an example of non-electrolyte, they do not conduct electricity to any appreciable extent. NH3, CH3COOH and Tap Water are weak electrolyte, they give a not too high but not too low conductivity, they show an equilibrium condition. KBr and HCI are strong electrolyte, they give a high conductivity. I would expect when the concentration of the solution increase, the conductivity will increase too, the same for the charge of the solution, when the charge(the number of ion) increases, the conductivity increases too. I would also expect the numbers of atom will have effect on conductivity of the solution too. For the calculation part of this lab, we will basically use Excel to rank conductivity of solutions and analyze the graph with their slopes, and then compare their slopes. We can use the tool in Excel to calculate the linear regressions and the R values for the graphs.
Calculation and Discussion:
1. Conductivity from lowest to highest(in microsiements/cm): Distilled water: 38
0.05M CH3OH: 41
0.05M C2H6O2: 41
0.05M NH3: 328
0.05M CH3COOH: 363
Tap Water: 697
0.05M KBr: 6081
0.05M HCI: 13009
Non-electrolyte: Distilled Water, CH3OH and C2H6O2
Weak electrolyte: NH3, CH3COOH and Tap Water
Strong Electrolyte: KBr and HCI
Tap Water and Distilled Water
Tap Water and Distilled Water have different conductivity because tap water contains ions such as sodium, copper, fluoride, and chloride ions, those will cause the conductivity of tap water higher than the conductivity of distilled water.
Summary of Result:
From the calculations of the linear regressions for the graphs, we can tell the effect of concentration and charge on the measured conductivity. Effect of...
Please join StudyMode to read the full document