Physically, the unknown compound was composed of white, grainy, crystal-like structures. The unknown was also odorless. From these observations, various physical and chemical testing was performed to determine properties of the unidentified compound. A series of solubility tests were performed, as shown in Table 2, and revealed that the unknown compound was soluble in water, but not in Acetone or Toluene. Because the compound dissolved in water, it is known that the compound is either polar or ionic3. Water is a polar substance, which maximizes its interactions with other polar molecules. Ionic substances also interact with and dissolve in water, because they can be considered an “extreme” case of polarity in which electrostatic forces hold atoms together. The interaction between water and the unknown compound can be described as “dissociation.” When a molecule is dissociated in a polar solvent, the anion of the molecule bonds with the solvent’s cation and vice versa4. In …show more content…
This result indicates that for every milliliter of water, .2 grams of the compound was dissolved; the science behind the test is that water is added in increments to determine how many mililiters of polar water molecules are necessary to break apart the polar or ionic bonds in a certain amount of solute. A Litmus paper pH test of the compound dissolved in water revealed that the solution had a pH of 7. This indicated that the solution of water and dissolved compound was neutral, or neither basic nor acidic5. The result of this test is in agreement with the identified compound because there are no OH- cations or H+ anions in KCl. OH- ions tend to make substances basic, and H+ ions make compounds more acidic1. Additionally, this pH test affirmed that sodium hydroxide and hydrochloric acid testing were not necessary in assessing the compound’s
Senegalia berlandieri (Acacia berlandieri) commonly known as Guajillo, is a legume small tree or shrub growing in northern Mexico and southern Texas. It belongs to the Leguminosae or Fabaceae family. It has seeds born in pods, compound leaves with numerous leaflets, and the roots are associated to bacteria that symbiotically fix nitrogen. This plant produce foliage and that are usually abundant in nitrogen compounds with a good indispensable amino acid composition. In addition.
Although this application has been discontinued, Chloroform is greatest known for it’s first use as an anesthetic. Prior to Chloroform, ether was the prevailing anesthetic for surgical procedures. However once Chloroform was introduced, ether was quickly replaced. Unlike ether, chloroform’s characteristically sweet odour isn 't irritating and was highly adored because it is 40 times sweeter than sugar. The sweetness of Chloroform coupled with it’s anesthetic properties made it a popular ingredient for toothpaste, cough syrup and skin ointments.
The more hydrogen ions present, it is said that the solution is more acidic and the smaller amount of hydrogen ions present, the solution is said to be basic or alkaline. pH is measured on a scale from 0-14, where 7 is the neutral value. The higher the pH value is the more basic and the lower the pH value, the more acidic. Significance of pH in the body [8]: pH maintenance is important in the body in order to support optimum health. The most critical pH is that of the blood and in order to maintain blood pH, homeostatic control takes place.
The formula for sodium acetate is NaC2H3O2, it is quite soluble in water, soluble in ether and slightly soluble in ethyl alcohol. While the chemical compound melts at 622.8℉, it does not have a boiling point for it will decompose. A hydrate is a chemical compound that forms when one or more water molecules are added to the molecules of another substance. Since sodium acetate is a trihydrate (NaC2H3O2·3H2O), it has three molecules of water for every molecule of sodium acetate and because of this, anhydrous sodium acetate quickly transitions into a trihydrate. This is due to sodium acetate being quite hygroscopic, meaning it readily absorbs moisture from the air.
SOLUBILITY AND SOLUBILITY PRODUCT OBJECTIVE In this experiment you will determine the solubility and solubility product of a sparingly soluble salt, potassium hydrogen tartrate, and also in four solutions containing a common ion. INTRODUCTION When a salt of low dissolubility dissolves in water, equilibrium is established between the solid solute and the dissolved ions. There are two terms used in discussing this condition.
Introduction Strong acids and strong acids both dissociate completely in water forming ions. However, strong acids donate a proton to form H3O+ along with a conjugate base and strong bases accept a proton to form OH- along with a conjugate acid. The chemical behavior of acids and bases are opposite. When they are together, their ions cancel out and form a neutral solution. In this experiment, HCl and NaOH will react to form NaOH and H2O with these two steps: The overall reaction is: Both Na+ and Cl- ions combine to form NaCl.
Confirmation tests for mercuric chloride: 1- After adding stannous chloride, gray precipitate will be formed: 2HgCl2 + SnCl2 → Hg2Cl2↓ (white ppt) + SnCl4 Hg2Cl2↓ + SnCl2→ 2HgO ↓ (black ppt) + SnCl4 2- Add potassium iodide, scarlet red precipitate is obtained and it's soluble in excess Iodide: Hg2+ + 2I- → HgI2↓ HgI2↓ + 2I- → [HgI4] Special reactions of HgCl2: