Distillation is used to purify a compound by separating it from a non-volatile or less-volatile material. When different compounds in a mixture have different boiling points, they separate into individual components when the mixture is carefully distilled. The boiling point is the temperature at which the vapor pressure of the liquid phase of a compound equals the external pressure acting on the surface of the liquid. The external pressure is usually the atmospheric pressure. Different compounds boil at different temperatures because each has a different, characteristic vapor pressure: compounds with higher vapor pressures will boil at lower temperatures.
This explanation can be demonstrated in table 3 also because the results of the reactions demonstrates that chloride reacted more by the color of the product compared to the color of chloride in the mineral oil. Also it also demonstrates that iodine is the weakest oxidizing agent because the results show that iodide didn’t change much from the color that it showed in the mineral oil. In example 6 we have shown the activity series for the halogens used in this
They are both very soluble in alcohol and hexane so that doesn’t help, but in water ethyl ether is semi soluble and pentane is in soluble. This would make us lean toward pentane but we felt strongly that ethyl ether because of the density was a much better test because there is much less human error and the we asked about how do you decide if something is insoluble
A) is neutralized by water B) is surrounded by water molecules C) reacts and forms a covalent bond to water D) aggregates with other molecules or ions to form a micelle in water Answer: B Page Ref: Section 3 11 9) Which would you expect to be most soluble in water? A) I B) II C) III D) IV Answer: A Page Ref: Section 3 10) Solutes diffuse more slowly in cytoplasm than in water because of A) the higher viscosity of water. B) the higher heat of vaporization of water. C) the presence of many crowded molecules in the cytoplasm. D) the absence of charged molecules inside cells.
The freezing point depression has some limitations and factors which affect to what extent the freezing point of the solvent will be decreased. One major limitation is the choice of the solute to be dissolved in the solvent because the solute must be able to dissolve sufficiently to lower the freezing point of the solvent. The solute must be soluble in the solvent in order to form a homogenous mixture. A few experiments with the unknown and different solutes will tell you what kind of properties the substance has and what substances will dissolve in it. Also, there is a limit of how much solute you can put in the solvent and you should not exceed that certain percentage.
As it was uncapped some of the heat would have been lost to the air and as one of our assumptions was that the heat released by the reactions was used only to heat the water the value calculated will be off. The consequence of this source of error would be the measurement of a lesser final temperature and therefore the heat of reaction calculated would also be less. Another source of error could be due to the use of a white Styrofoam cup and the dissolving of white sodium hydroxide pellets. It would be easy to miss if the reaction had yet to fully take place meaning the final temperature recorded would be lower and heat of reaction calculated would be lower. A final possible source of error could be that not a precisely even amount of HCl and NaOH were used for the neutralization reactions in part two and three.
For example, the reaction |BaCl2•2H2O ( BaCl2 + 2H2O |(2) | is reversible, and if water is added to the anhydrous salt BaCl2, formation of BaCl2•2H2O takes place: |BaCl2 + 2H2O ( BaCl2•2H2O |(3) | The reaction of dehydration of hydrated ferrous sulfate |FeSO4•7H2O ( FeSO4 + 7H2O |(4)
The dissolving process involves a consideration of the relative strength of three intermolecular attractive forces. The type of forces between solute-solute molecules and solvent-solvent molecules must be considered. These intermolecular attractions must be broken before new solute-solvent attractive forces can become effective. A solute will dissolve in a solvent
Determination of a Solubility Product Abstract: The purpose of this experiment was to determine the solubility product constant (Ksp) for a sparingly soluble compound, Ca(OH)2, in pure water and in a NaOH solution. To determine the solubility product constant a solution of Ca(OH)2, in pure water was titrated with HCl. The concentrations of OH- and Ca2+ were used to calculate the solubility product constant. Another solution, containing Ca(OH)2, in NaOH was also titrated. The concentrations of OH- and Ca2+ were used to calculate the solubility product constant.
The slower molecules gain more thermal energy and collide with other molecules in the cooler object. This process continues until heat energy from the warmer object spreads throughout the cooler object. Some substances conduct heat more easily than others. Solids are better conductor than liquids and liquids are better conductor than gases. Metals are very good conductors of heat, while air is very poor conductor of heat.