The temperature of the sulphuric acid was not measured throughout the experiment, however the room in which the experiment was conducted was kept constant, so the chance of any large error due to unknown temperature of the sulphuric acid was most likely reduced. The amount of sulphuric acid used was also controlled by measuring 100mL with a 100mL measuring cylinder to ensure that the results would be consistent. The volume of the agar cubes was calculated from the surface area of each agar cube, both before and after they had been in the sulphuric acid. This increased the reliability of the results as it allowed the rate of diffusion of the sulphuric acid into the agar cubes to be calculated more accurately. The concentration of the acid was 0.1M, which was placed in all three agar cubes to maintain consistency of results.
Purpose The purpose of this experiment is to find information and explore similarities about eight compounds- NaCl (Salt), Sugar, Paraffin Wax, Acetylsalicylic Acid (Aspirin), Calcium Chloride (deicer), Ascorbic Acid, Cornstarch, Epsom Salt, all through six tests- physical appearance, hardness, conductivity as a solid, solubility in water, conductivity as a liquid or solution, and melting point. Hypotheses If we test physical appearance then all compounds will be white and somewhat transparent. Sugar and salt will be composed of small grains.
The solution with pH 3 has a higher H+ concentration than the one with pH 12. The numbers 12 and 3 signify whether a solution is acidic, neutral, or basic (alkaline) based on the concentration of hydrogen ions contained within the solution. If an anthocyanin molecule is added to a solution and releases a proton once being added into the solution, the anthocyanin molecule is behaving like an acid. A proton (or a hydrogen ion), is being lost, which is a characteristic of an acid. When anthocyanin molecule is being added into a solution, the double bonds shift and its color changes depending on whether the solution is acidic or basic.
ABSTRACT Due to the potential harmful effects of the glacial acetic acid, a commonly used diluting fluid for manual WBC count, the researchers proposed to use commercially-prepared ascorbic acid to lyse the red blood cells while maintaining the morphology of the white blood cells. This study aimed to compare the capability of commercially-prepared ascorbic acid as a lysing agent in a diluting fluid to glacial acetic acid. Specifically, this study aimed to compare their capabilities in lysing red blood cells, maintaining white blood cell morphology and white blood cell count.
Why did the liquid water increase in temperature? Due to the beaker sitting on the hot plate during the experiment, it resulted in the liquid water’s temperature to increase. In other words, the hot plate was used as a heating source/device without the use of an open flame such as a bunsen burner (which served as a major advantage for this specific experiment).
Abstract The purpose of the experiment was to test which antacid medicine was most effective in decreasing the acidity levels in the stomach. Titration experiments involving hydrochloric acid and sodium hydroxide were used to test different antacids to see which one needed the least amount of sodium hydroxide to turn the solution pink. The antacids that were being compared in this experiment were Alcalak, Alka-Seltzer and Medi-First. With the use of M1 x V1 = M2 x V2 the excess volume of hydrochloric acid was found in order to find the amount of hydrochloric acid volume neutralized out of the original 100 mL of hydrochloric acid.
The purpose of this lab was to determine the melting and freezing point of an unknown (Q) substance and to identify the unknown substance based on the melting and freezing properties. First, to start the lab, a double ring system was set up for a hot water bath. Next, unknown Q was examined and observations about the solid were taken at the lab station. Next, a test tube that contained unknown Q was placed onto a test tube clamp.
Furthermore, the value attained for the calorimeter constant was 0.1748 KJ/°C, this value allowed to apply the correction for heat loss to the calorimeter. However, during the calculation for the calorimeter constant, the assumption that the specific heat of water was 4.184 J 〖deg〗^(-1) g^(-1). The concentration of NaOH was attained when assuming no heat loss was 0.8170 M and including the heat loss the concentration of NaOH was 0.9493 M. These values are very close to the expected value of the concentration, which is 1.071M considering the experimental error is only about 11 percent off.
Lab Report In this Lab Report at the end you will learn how to set it up and how to work it out I am going to be telling you how to write a Lab Report, this lab report will be about Acids and Bases lab I am looking for how you did it & how u set it up For your hypothesis/predictions you would need use what u used to do your lab do your work. Hypothesis/Prediction is what I would give u to do your work on and it tells you how to do everything what I have given you to do this lab is 11 Plastic cups, 10 Pipets, 10 Test Strip Pieces, Graduated Cylinder, Chart, Pencil/pen. In this lab you will learn what PH is and a PH is The p stands for potential and the H stands for Hydrogen, when you wait on other directions on what to do u have 11 cups sitting in front of you the have components what that means a part or element of a
Acesulfame-potassium Chemistry of Acesulfame-potassium Acesulfame-potassium also known as acesulfame K or Ace K. The molecular mass of it is 202.245 g/mol. Its chemical name is Potassium 6-methyl-4-oxo-4H-1,2,3-oxathiazin-3-ide 2,2-dioxide. [1] It also have a pH value of 6.5-7.5, having a melting point of 229-232 °C and it is soluble in water. Ace K is a white odorless, free flowing crystalline powder.
CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt, the pH level of Calcium Carbonate is 9.91, and it is therefore, a basic substance, due to the fact that it is comprised of a pH level higher than 7, which is neutral3. HCl, however, is the bodily acid found in the stomach of human beings.
Acids are proton donors in chemical reactions which increase the number of hydrogen ions in a solution while bases are proton acceptors in reactions which reduce the number of hydrogen ions in a solution. Therefore, an acidic solution has more hydrogen ions than a basic solution; and basic solution has more hydroxide ions than an acidic solution. Acid substances taste sour. They have a pH lower than 7 and turns blue litmus paper into red. Meanwhile, bases are slippery and taste bitter.
Hydrogen chloride has a very powerful smell. It is in the form of a gas but only when it is at room temperature which is approximately 25 Celsius and when the pressure is high. When you add water to hydrogen chloride then it breaks down into small pieces which are known as dissolving. The solubility of hydrogen chloride is very high this means that it can dissolve in water quickly because it dissolves many times in its own solution (the gas form of hydrogen chloride). It is very soluble because the smaller the chain of the molecules are then the energy will be required in small quantities however if the chain is long then it will need more energy
Introduction The goal of the experiment is to examine how the rate of reaction between Hydrochloric acid and Sodium thiosulphate is affected by altering the concentrations. The concentration of Sodium thiosulfate will be altered by adding deionised water and decreasing the amount of Sodium thiosulphate. Once the Sodium thiosulphate has been tested several times. The effect of concentration on the rate of reaction can be examined in this experiment.
Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.
