In this lab, lab 4.3 Comparing the Concentrations of Saturated Solutions, we set out to find and compare the solubilities of two solids in water. In addition, we tested if solubility is a characteristic property of a solid in a given liquid. This lab allowed us to test and use a reliable way to measure the solubility of a solid. This lab can be replicated for any solid with the same procedure, thus it gives us a method to calculate solubility. The two solids we tested in this experiment were NaCl (Sodium Chloride) and NaNO3 (Sodium Nitrate). To begin the experiment, we measured 5cc of water and 5g of NaCl and added them to a test tube. Next, we stoppered the test tube and shook vigorously for two or three minutes. After we observed that …show more content…
Six of the ten sodium chloride groups found the solubility of sodium chloride to be statistically 36g/100cc of water, with a +3g/100cc margin of error. Three of the four groups outside this margin of error had solubilities in the forties, 42, 48, 49g/100cc. These three groups made an experimental error that altered their results and can be excluded from our analysis of data. Another group was in the low thirties with 30g/100cc. Yet the beginning masses that compose the solubility equations do differ. For example, one group found that the mass of their solution was 4.21 grams, but another recorded a mass of 5.47 grams. When it comes to the mass of the solid (solute) the former recorded a mass of 1.11 grams, the latter reported a mass of 1.38 grams. Nonetheless, they came out with the same solubility of 34 grams per 100 cc of water. Thus we can prove that that solubility is a characteristic property. This is because every group started with a different mass of solution and solid, but they concluded with the same solubility (given the +3 gram margin of error and excluding outliers) or were close. Therefore, solubility is a characteristic property. Of the eight sodium nitrate groups three of them found statistically, with a +3g margin of error, 86g/100cc as the solubility of sodium nitrate in water. Another group calculated the solubility to be 82, which is just below the margin of error. Two of the eight groups
I. LIQUID - Identification of an Unknown Liquid: Using the physical properties of Solubility, Density, and Boiling Point.
The purpose of this particular lab was to experiment and identify the chemical and physical changes throughout the experiment.
The main objective of this experiment is to differentiate between a physical change and a chemical change.
6. The solubility of the solids were tested using a micro tray, by placing them in water and oil to observe their polarity,
The two salts AgX and AgY have very similar solubilities in water. It is known that the salt AgX is much more soluble in acid than is AgY. What can be said about the relative strengths of the acids HX and HY?
AP Chemistry Background The solubility product constant, Ksp, is a particular type of equilibrium constant. The equilibrium is formed when an ionic solid dissolves in water to form a saturated solution. The equilibrium exists between the aqueous ions and the undissolved solid. A saturated solution contains the maximum concentration of ions of the substance that can dissolve at the solutions temperature. A knowledge of the Ksp of a salt is useful, since it allows us to determine the concentration of ions of the compound in a saturated solution. This allows us to control a solution so that precipitation of a compound will not occur, or to find the concentration needed to cause a precipitate to form. The solubility product which will be
Solutions of 6M H2SO4, 6M NH3, 6M HCl, 6M NaOH, and 1.0 M of NaCl, 1M Fe(NO3)3, 1M NiSO4, 1M AgNO3, 1M KSCN, 1M Ba(NO3)2, and 1M Cu(NO3)2 were given in separate test tubes. The color of possible precipitates, ions, acid-base behaviour, odor and solubility rules were conducted and were reported in Table 1. The key information about a mixture of two solutions was
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.
If you dissolve a substance such as ordinary table salt (NaCl) in water, the boiling point of the water will increase relative to the boiling point of the pure water. In this assignment, you will dissolve a sample of NaCl in water and then measure the boiling point elevation for the solution.
Abstract: This experiment introduced the student to lab techniques and measurements. It started with measuring length. An example of this would be the length of a nickel, which is 2cm. The next part of the experiment was measuring temperature. I found that water boils around 95ºC at 6600ft. Ice also has a significant effect on the temperature of water from the tap. Ice dropped the temperature about 15ºC. Volumetric measurements were the basis of the 3rd part of the experiment. It was displayed during this experiment that a pipet holds about 4mL and that there are approximately 27 drops/mL from a short stem pipet. Part 4 introduced the student to measuring
By identifying the solubility of the unknown, it could lead to a closer interpretation as to what the functional group the unknown may be. Solubility is determined based on intermolecular attractive forces, such as hydrogen bonding, dipole-dipole, and London dispersion forces. Intermolecular attractive forces arise due to different electron environments in different molecules. For example, water molecules are good at dissolving
As the temperature of water increases, the particles of solid Potassium chloride, KCl, which are absorbing energy from its surrounding, start moving more easily between the solution and its solid state because. According to the second law of thermodynamics, the particles will shift to the more disordered, more highly dispersed solution state. I predict that as the temperature of a KCl and water mixture increases, then the solubility of the KCl will also increase.
If there are different concentrations of solutes in a solution then it can affect its shape and function. If there is more salt in a blood cell then that cell will shrivel up and won't function properly. Another example is if you have a plant cell from a pond and you change what type of water you submerge it in, it changes
Do they coincide with the theoretical effects? Explain. From the data gathered, presence of common ions decreased the solubility of Calcium Hydroxide (see: Table 2.2 vs Table 3.0 data). The effect of ionic strength on the solubility, on the other hand, has a general trend of increasing solubility as the ionic strength increase. However, it can also be observed that the ionic strengths of the different KCl solutions has an inconclusive relationship with the solubility and the concentration of the solution (see: Table 5.0).
The purpose of this lab was to study colligative properties. These properties are properties that are affected when a solute is added to a solvent. Thus, the amount is important, not the actual type of substance, for the colligative properties. A couple types of this property are the freezing point and boiling point of a substance. (1)