Solubility Lab

Two small cup were filled with salt, both cups weighed about 31-32 grams. 5. A cup of salt was then used to slowly pour salt into the beaker of warm water. 6. The contents of the beaker were stirred with a stirring rod.

The purpose of using solubility analysis on an unknown is to narrow the possible unknowns given based on the solubility analysis. Acetone was a control for ketone and was soluble in water. Hexanal was a control for an aldehyde and was insoluble in water due to intermolecular forces, such as an increased amount of hydrophobic area rather than hydrophilic area. As a result, by identifying the solubility of the

some of the particles may have peptized causing us to filter out some of the silver chloride

While looking at the results, I noticed that the cold temperature solution glowed for the longest time with an average of 14.5 minutes. The room temperature solution was next with an average of 13.5 minutes. Finally, the warm temperature glowed for the shortest amount of time with an average of 9.5 minutes. I noticed that the solubility affected the glow rate. The warm water was able to quickly dissolve the copper sulfate, Luminol, and Perborate mixture. However, the cold water took the longest because it was hard for it to dissolve. In order to keep the dissolving process going, every so often, I mixed it.

On the other hand, Part B provided insight on organic substances and their properties of solubility. Each solute was shown to be soluble in at least one of the three different solvents. Benzophenone was soluble in methyl alcohol, but not in water.

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

• Neutral compounds do not react with either NaOH or NaHCO3. They are soluble in organic solvent and not soluble in water.

Meaning, compounds with the same type of bonding tend to be soluble with one another. Polar substances would dissolve in polar solvents such as water, however, would not dissolve in non-polar solvents. Non-polar substances dissolve in non-polar solvents but do not dissolve in polar ones. Most ionic compounds are able to be dissolved in water as the water molecules hydrate ions. For an ionic compound to be dissolved, the water molecules must stabilize the ions, which thus would result in the separation of the ionic bond to form a solution. Water is a polar molecule, it has a permanent dipole. The oxygen atom has a partial negative charge whilst the hydrogen atom has a partial positive charge. When an ionic substance is placed in to the water, the water molecules would quickly attract the charged ions from the substance. They then become free to move about. However, this only occurs when the attractive forces between the water molecules and ions are stronger than the attractive forces within the ionic compound. CaOH is a slightly insoluble compound, the solubility of CaOH is approximately 0.189 g/100 mL of water at 20. A more soluble ionic compounds solubility such as NaCl is only 35.7 g/100 mL of water at 20°C. CaOH is only slightly insoluble as calcium and oxygen are +2 and -2 ions in

The definition of solubility is a property of a solid, liquid, or gas solute to dissolve in a solid, liquid, or gas solvent. The two parts of a solution are the solvent and the solute. When a solute is dissolved, particles of the solute leave each other and become surrounded by particles of the solvent. In this lab, we tested stirring speed, concentration, particle size, and temperature and their effect on solubility. The question was, “How can you control the rate at which certain salts dissolve in water?” My hypothesis for stirring speed was, “If stirring speed is increased, then solubility is increased.” My hypothesis for concentration was, “If concentration is increased, then solubility is decreased.” My hypothesis for particle size was, “If particle size is increased, then solubility is increased.” My hypothesis for temperature was, “If temperature is increased, then solubility is increased.”

When ionic compounds are added to water dissociation can occur and the solid dissolves. But only a certain amount of solid can be added to a volume of water before the solution becomes saturated and no more solid will dissolve. This saturation point can be affected by a number of variables including temperature.

Before I start the experiment, I predicted that all crystal form solutes would dissolve while powder form solutes will not, but my prediction was partially supported. A baking soda was a one that showed an unexpectedly result because even though it is in a powder form, it dissolved in the water. Except for a baking soda, everything could be observed from what I predicted. Sugar and salt, which are in a crystal form dissolved in water and had high solubility while flour and cornstarch, which are in a powder form didn’t dissolve and had low solubility.

In this experiment, the changes in free energy (ΔG), enthalpy (ΔH), and entropy (ΔS) of the potassium nitrate’s (KNO3) dissolving reaction are determined by finding the equilibrium constant (Ksp). After this experiment is performed one should be able to have a better understanding of the thermodynamic properties and solubility constant (Ksp), and those properties relation to ∆G˚. Thermodynamics is the study of hat energy and other values of work, temperature, and energy regarding the process of a chemical reaction. A goal of this experiment is to be able to measure the solubility of KNO3 as a function of temperature, and analyze this function graphically. This graph is based off of solubility and temperature change, or more specifically the

A basic rule for polarity is polar compounds dissolve in polar compounds and non polar dissolve in non polar. Polarity of an organic compound can be effected by the number of carbons in its chain and by the functional group connected to that chain. One example of how polarity effects solubility is when you put the NaCl (salt) in H2O (water). The positive charged dipole moment ends of the H2O molecule, the hydrogen, will surround the negative Cl

A solution consists of two or more different substances. The dissolving process that takes place in a solution occurs due to the intermolecular forces that act between molecules in the solution. The solubility rule, “Likes dissolve likes”, explains why certain solutes dissolve in a given solvent, while other solutes do not. In most cases, ionic or polar solutes dissolve in polar solvents. Similarly, non-polar solutes dissolve in non-polar solvents. This is usually what occurs, but there are exceptions in particular cases.

(I’m going to use the water solubility test to figure out if the unknown compounds are Ionic or Covalent by putting in the powders in distilled H20. As stated above ionic compounds can be identified if dissolved in h20 but non polar covalent does not dissolve in water. How ever, polar covalent dissolves in water and to make sure whether it is polar or non polar we use ethanol to identify what type of covalent compound it is.