Solubility

An equilibrium constant for a solid substance that is dissolving in an aqueous solution is represented by the solubility product constant, where the concentrations of different ions from the solid substance (compound) are used to calculate the solubility product constant. If the solubility product constant vale is high then the substance is very soluble in an aqueous solution. The solubility product constant is denoted by Ksp, and for a common reaction: aA(s) ⇌ cC(aq)+dD(aq)T The Ksp= [C(aq)]c[D(aq)]d

Rate of drug release at any given location within gastrointestinal tract depends on the mechanism by which the drug released from pellets and local environment within git. In order to predict in vivo behavior of dosage forms, knowledge of release mechanism and physiological conditions of git should be understood. Type of coating and method of applying coating will determine dominant mechanism of drug release from coated pellets. Release kinetic is predominantly determined by the behavior of coating

to the solubility rules. Some compound are soluble under certain conditions and others are not. The formation of a solid when two compounds react is called precipitation, resulting in precipitate. This lab helps one to better understand how precipitate is formed and under what conditions. We are given solubility rules, which help us to predict with reactions would form precipitate. Procedure/Experimental First, partners predict which reactions would form precipitate by using the solubility rules

Introduction Microscale involves using smaller amounts of chemicals and solids. Therefore, the purpose is to determine the density, solubility, recrystallization, extraction, separation, and drying of products by using small quantities. The mass of volume was determined by using the density formula: Density= Weight (g) / volume (mL). Solubility is defined as the extent to which a substance is soluble. Crystallization is a technique used for purifying solid compounds. The percent recovery determined

for the Crystal Growth experiment is to identify which Solubility and temperature produces larger crystals, and to simulate natural crystal growth. We will achieve the results we desire by conducting the experiment thoroughly and correctly, as well as correctly

ammonium hydroxide and 0.1 M lead nitrate, however their corresponding number was unknown. The first identified unknown was 98, acetic acid, given its highly prevalent scent, in addition to it not forming a precipitate with any substance due to the solubility rules. Given that two bases were present on the initial pH test, one being strong (93) and one being weak (91), it was then concluded that they were the strong base NaOH and the weak base NH4OH, respectively. Once identified, the precipitates formed

yellow. But when researching the actual reaction there most likely shouldn’t have been a precipitate. In table 2.1 the given reagents and metal ion reactions are given as they reacted with each other. This was done hugely with the help of the solubility rules given in the lab manual. Once recognizing which ions had a positive and negative charge from

Method In order to achieve the best result, this experiment was broken into two part: the first part of this experiment involves carrying out solubility tests on known compounds, N-pivaloyl-o-toluidine, and in the second part the TLC and solubility tests was used to find a suitable recrystallization solvent for an unknown compound. For Experiment 6A, a 50 mL round-bottom flask with a small stir bar and septum was flame-dried under the hood, and

Extraction of Caffeine from Tea Leaves Introduction Caffeine is soluble in boiling water and as a result it is easily extracted from tea bags by steeping in hot water. This process leaves behind the water insoluble portions of the tea bag. However, water extracts more than just caffeine, so a final separation is done with an organic solvent that will dissolve primarily caffeine. The organic solvent used in this experiment is Dichloromethane (CH₂Cl₂). Dichloromethane is less polar than water

different bottles. In this experiment a flame test and a solubility test were conducted in order to identify the unknown solutions. It is hypothesised that the flame test will be successful in identifying which cation (sodium, potassium and strontium) is in which solution through the colour of the flame. It is also predicted that the precipitate tests will successfully identify the anions (carbonate, sulphate and chloride) by testing the solubility of the solutions. The dependant variable is the chemicals