Solute Lab Report

Due to this fact, the concentration of copper in the solution is able to be calculated by using light absorbance. Since zinc doesn’t absorb any light, we are able to deduce that the greater the absorbance, the greater the concentration of copper.

After this, the solution was poured into a volumetric flask just about to the 1dm3 line and then it was left there to cool to the same temperature as the room before filling precisely to the 1dm3 line with distilled water. The molar mass of CuSO4.5H20 was 249.5 so that means 249.5g of copper sulphate was needed to dissolve, in order to make a standard solution, into 1dm3of distilled water. Following this, a linear dilution of the CuSO4.5H2O was made in order to be used to make a calibration curve after using the colorimeter to write down the absorbance of each sample. A linear dilution is diluted with distilled water in order for it to make the concentration weaker and weaker. For this investigation, the dilutions made ranged from 0.01 to 0.1 M/l . It was essential to only make up 10cm3

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.

Properties of Solutions: Electrolytes and Non-Electrolytes The objective of this lab the type of compounds formed in many different solutions dissolved in water based on the conductivity of each. Procedure: Refer to handout entitled “Properties of Solutions: Electrolytes and Non-Electrolytes” Materials: Refer to handout entitled “Properties of Solutions: Electrolytes and Non-Electrolytes” Data & Observations: Solution Conductivity (μS/cm) A – CaCl2 9100 μS/cm A – AlCl3 11920 μS/cm A – NaCl 6280 μS/cm B – HC2H3O2 485 μS/cm B – HCl 15400 μS/cm B – H3PO4 6000 μS/cm B – H3BO3 10 μS/cm C – H2Odistilled 1 μS/cm C – H2Otap 790 μS/cm C – CH3OH 1 μS/cm C – C2H6O2 2 μS/cm Conclusion: 1.

The purpose of this experiment is to figure out weather or not electricity could affect the pH of a solution. Adding the Epsom salt to the solution and pencil led as the conductors of the electricity and with a salt bridge connecting the two solutions in the middle. Chemicial reaction will form if the solution with Epsom salt reacts to the electricity with both positive and negative charges. To extend the experiment using both terminals of the battery, and figure out the effect of both positive and negative charges had on the pH was also apart of this lab.

Conductivity is the ability to pass on electrical current within a solution, a metal or even a gas. It can be affected by other chemical related factors such as the concentration, temperature and also the mobility and valence of ions. Yet the most conductive form occurs within aqueous solutions as it contains both cations and anions; where the solvent stabilises the attracting ions through a process called solvation. Within the various levels of ionic strength from low to high electricity flow, electrolytes can either be strong or weak, according to the reaction. Strong electrolytes are substances that are fully ionised in solution due to the positive and negative ions that migrate under the influence of an electric field. Therefore the concentration

Water boils at 212 degrees Fahrenheit; it freezes at 32 degrees Fahrenheit. If you add a solute to the water (solvent), it may change the temperature at which the water will boil or freeze. Depending on the solute, the solution may boil at an elevated temperature. The solution may also freeze at depressed temperature. If there is a change in the temperature, it will be because of the solute added to the solvent.

The last couple ones that actually did dissociate into ions in water, showed their high conductivity especially HCl. Tap water surprised also has high conductivity since it has ions that comes with it. Overall, I found that although in these solutions are consisted of atoms, the conductivity electricity depends on the

This is because as evaporite minerals precipitate out of solution, the remaining solution will have fewer of the ions that comprise the evaporite minerals. This is consistent with the degree of saturation values shown in table 5, where the fourth sample had the highest degree of saturation, indicating that it was between the time sample 4 and sample 5 were taken where the most precipitation occurred. Halite shows a similar effect, but does not dramatically decrease in concentration until between sample 5 and 6. Although the degree of saturation did not exceed 1 in calculations, there was a peak calculated at sample 5. Because sodium and chloride ions were measured to decrease significantly between the two samples, precipitation should have occurred to draw these ions out of the remaining modified seawater solution. It is possible that the degree of saturation did increase above one between the two sampling periods, but then decreased again as ions were pulled out of the solution by

* 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.

One of the strange results in the experiment was that on test 3 from 9g to 10g of salt it only went up by 0.03amps. This could of happened because the person who was holding the electrodes could have been holding them further away or closer tighter between the tests. This would of effected the results because of 4 reasons, one of the reasons could have been that when the scales were being used there could have been moisture in the salt which would have effected the weight so the salt amount could have varied as the salt was added. Another reason could have been that some of the salt might not have been dissolved throughly so it could of effected the amount increased. This is because…. Poor wire contact on with the ammeter is another reason there could have been strange results as …. The last reason that could have caused strange results is the quality of electrodes. This would have effected each test that was done because after each test was done, the electrodes

After trying the experiment with a small battery we tried it with a bigger battery to see if the liquid would conduct enough electricity to light the light bulb. After going through all of the different liquids the light bulb still did not light. This was a big shock because I figured one of the liquids would conduct enough energy to light the lightbulb. There was a tool in class that allowed observes to see how much each liquid conducted electricity. All of the liquids conducted, but the salt solution was the best conductor.

The above mine sample had a conductivity of 2200 µS/cm, whereas the below mine sample had a conductivity of 7500 µS/cm. This suggests that there are a significantly greater number of ions in solution in below mine water than above mine water.

In week one we performed a qualitative solubility test of our fats and oils, synthesized our soaps and detergents, and performed a solubility test and lathering test for the soaps and detergents. We wanted to test the solubility of our starting materials of the soap making process to understand the properties of the materials. In our initial solubility test of the starting materials, we found that most of the materials were insoluble. As you can see in Table 2.0, olive oil and vegetable oil were only soluble in toluene and the shortening and lard were only partially soluble in acetone. In order to understand the solubility of the soaps and detergents, after our synthesis and filtration, we performed a qualitative solubility test with each of

Typically a lower resistivity layer overlies a more resistive core (Arnason et al., 2008). The low resistivity layer is characterized by an electrically conductive clay (smectite), which forms in temperatures of 70°C. As temperatures increase the proportion of a less conductive clay (illite) increases until the formation of pure illite at 250°C (Anderson et al., 2000). Resistivity of smectitie is typically between 1 and 10 ohm-m compared to the 20 -100 ohm-m resistivity of the clay layers at 180°C (Anderson et al., 2000). Typical resistivity’s outside of geothermal systems vary but are typically between 50-200 ohm-m for volcanic rocks and less than 5 ohm-m for marine sediments (Anderson et al., 2000).