Saturation Point Lab

    One possible source of error that can affect the results was that a mercury thermometer was used instead of an electronic one. The use of a mercury

Water (H2O) is a good solvent because it is partially polarized. The hydrogen ends of the water molecule have a partial positive charge, and the oxygen end of the molecule has a partial negative charge. This is because the oxygen atom holds on more tightly to the electrons it shares with the hydrogen atoms. The partial charges make it possible for water molecules to arrange themselves around charged atoms (ions) in solution, like the sodium (Na+) and chloride (Cl−) ions that dissociate when table salt dissolves in water.

Ionic compounds are soluble in water to a certain point depending on the compound. The level of solubility changes among different compounds. Some ionic compounds can completely dissolve in water and appear to be a homogeneous mixture. Although, some ionic compounds dissolve very little, and could be considered insoluble, since it does not dissolve fully. Depending on the compound, the level of solubility can be high or low. However, ionic compounds could dissolve to a certain degree. If the solution appears to be a heterogeneous mixture, many may assume through visual representation that it may be insoluble. As stated previously, the smallest amount of solubility should be considered. To confirm whether or not the substance is soluble, observe the efficiency when conducting electricity. Due to practical reasons, the slightest solubility could be considered insoluble by people.

The experiment this week had two different purposes. The first is to teach us about freezing points. This lab was designed to show us the freezing point of a pure solvent, in comparison to a solvent in a solution with a non-volatile solute. The second goal of the experiment is to teach students about osmosis. In the experiment, we got to observe osmosis as well as understand dialysis.

The experimental error in this lab included the question whether the digital scale was as precise as it could be, how the cooling time affected the water in the hydrates, and any miscalculations that could have occurred. The digital scale could have been more precise since they are more precise scales that could deliver more accurate masses in this lab.

An error that could have occurred during this experiment would be the failure to heat all of the water particles in the air off the

Describe the "strength" of ionic bonds. Use salt as your example. Ionic bonds are weak, that’s why salt can dissolve in liquids

For this lab inquiry, students were placed in groups of 2-3 and tasked with finding the correlation between the temperature of a solvent, and the dissolution rate of a solute. These materials were necessary in order to successfully conduct the experiment: One 10 mL graduated cylinder, one 25 mL graduated cylinder, one 50 mL graduated cylinder, 1-2 100 mL graduated beakers, 1-2 900 mL graduated beakers, some 1-3 squirt bottles, water, 1-3 pounds of ice, a heated container, 11 start/stop timers, roughly 15 styrofoam cups, and a yogurt cup filled to the brim with M&Ms. In order to collect data, students would need to prepare cold and hot water, using the materials provided. Nextly, students would create ratios of cold and hot water, making the maximum amount of each type of water to be 100 mL, with the max amount of water being 100 mL. The ratio would act like so:

The third error encountered during testing also occurred during the first experiment. After the first three days of the trial, since the beakers were not covered, the water level began to decrease. Since more and more water was evaporating, the salt concentration became higher and higher causing the results to be completely inaccurate. In order to avoid this, the beakers could have been covered whilst not being used to ensure that minimal evaporation

The first possible source of experimental error in this experiment was the fact that our lab setup was not working properly since it was giving the lab group different data which lead to a higher than usual percent difference. This may hvae been caused by faulty lab equipment. The second source could've came from the PASCO since our data was incorrect depsite having a correct set-up. The third source may have been a faulty curcuit board since the data was also incorrect. Every source could have been responsible for the high percent difference.

Introduction This report, discusses how the concentration of a substance can be found through titration. A titration is where a substance with a known concentration is tested with a substance that has an unknown concentration to find that concentration (What Is a Titration). Titrations are very important in the food industry. It is important to know the concentration of an ingredient or chemical especially when it comes to nutrition facts and labels for a particular product.

Part 2 of the experiment produced an average maximum temperature of 70.3 ⁰C. Part 4 had an average of 77.8 ⁰C and Part 5 had an average of 76.9 ⁰C. These differences could have been clarified by having more trials. Conducting more trials would improve this experiment, in that there would be less percent error due to the more accurate averages. Part 1 of the experiment appears to be an outlier, because its results were not half that of the other parts of the experiment. This could be a source of error. It is undetermined whether this major difference was due to random or systematic error.

In the ion lab elements and compounds were combined in mixing wells in order to observe their reactions. The purpose of the ion lab was to gain an understanding of the reactions and solubility of ionic compounds, to practice writing balanced chemical equations, and to practice observational skills. During the lab it was found that when ionic solids dissolve the compound separates into its individual ions. This state of ions being dispersed within a solution when dissolved is what we describe as aqueous, and the act of being able to dissolve is called being soluble. When a combination of ions is insoluble, or not able to dissolve it results in a precipitate, because the ions in the compound could not separate or dissolve. This insolubility is

First, if the exact same equipment and materials are not used in every test, the results can be skewed. For example, if three different meter sticks, made of different materials, were used in this experiment, the results could be messed up, because each meter stick may produce a different pitch, depending on its material. To prevent this problem, simply use the exact same materials and equipment for each test. If something breaks or needs to be replaced, it is best to just start the experiment over, so that all the results come from the same materials. Another possible error is the use of different methods in the experiment. For example, for the kazoo test, if one way of humming, or one pitch is used, and then a different one is used, that will negatively affect the results. Like before, the use of the exact same methods is very important, so that the results are as accurate as possible.

The four salts that were given were ammonium chloride (NH4Cl), ammonium nitrate (NH4NO3), sodium thiosulfate (Na2S2O3), and magnesium sulfate (MgSO4). With the intention of saving time, my group was given only ammonium chloride and ammonium nitrate to do and then we would compare the results with the entire class. First, the probe needed to be calibrated and in order to do that three 250 mL beakers were filled to 50.0 mL of distilled water. One beaker was room temperature and a thermometer was placed in it that measured to 19.9 degrees Celsius. Another beaker was cold water (iced added to it) and a