Aim To Find the Number of Moles of Water of Crystallisation in Copper (II) Sulphate salt. Introduction Water of crystallisation is the term given to the molecules of water that are used to build up a crystal lattice in some ionic compounds.In copper II sulphate the blue crystals would be impossible without using water molecules to act as ’scaffolding’ within the structure CuSO4.5H2O. When this is heated the water molecules are driven off and the blue crystals become a white powder. As most
Premium Crystal Water Chemistry
are needed to visualize the end-points. The first indicator is phenolphthalein which will turn from the pink ionic form while in a base‚ to a colorless form indicating the first end-point in this experiment. At this point exactly one mole of HCl has been added per mole of carbonate. This reaction of phenolphthalein occurs from pH 10 to 8.3 which is within 1 pH of the equivalence point for the carbonate to bicarbonate reaction. The second reaction has an equivalence point at ~ pH 3.7. This is where
Premium Hydrochloric acid Titration PH indicator
substances taking part in a reaction or forming a compound‚ typically a ratio of whole integers. You need to use numerous conversions‚ atomic weights‚ and mole calculations in order to get the grams of each reactant. Atomic weights are the weight of each element on the periodic table; for example‚ Oxygen is 16.00 grams and Carbon is 12.01 grams. Moles are a standard scientific unit for measuring large quantities of very small entities such as atoms‚ molecules‚ or other specified particles. In all Stoichiometry
Premium Chemical reaction Stoichiometry Reagent
ions in solution. The point at which this mole equivalency occurs is known as the equivalence point. An indicator in the solution will change color to signal that the equivalence has been reached (actually‚ the indicator responds to the slightest excess of OH ions). The color change in a titration is called the endpoint. At the equivalence point of the titration‚ the moles of OH (base) are equivalent to the moles of H+ (acid) in the sample. The moles of OH added to the solution from a buret are
Free Titration Acid
INTRODUCTION EDTA (H₄Y) is widely used to determine metals in complexometric (a volumetric analysis where the formation of a coloured complex is used to indicate the end point of a titration) titrations as it forms stable complexes with most metal ions. EDTA is a tetracorboxylic acid and in alkaline conditions‚ it exists as Y⁴⁻ ions‚ which form 1:1 complexes with metal ions like nickel(II) ions: Y⁴⁻ + Ni²⁺ NiY²⁻ A metal ion indicator (an organic dye which changes colour when it binds with metal
Premium Ammonia Titration Hydrogen
n; Number of moles - moles R; Gas Constant - JK-1mol-1 T; Temperature - K Gas Constant (R) is what we are trying to calculate Known Gas Constant: 8.31 JK-1mol-1 Sample Calculations: Temperature needs to be converted from degree Celsius in Kelvin Temperature in Kelvin: °C + 273 = … K e.g. 24.0 + 273 = 297.0 Kelvin From the Mass we need to calculate the number of moles (n) of Magnesium (Mg) Using the Final Mass minus the Initial Mass from the Raw Data table moles = mass/ relative
Premium Temperature Pressure Ideal gas law
Preparation of Aspirin The purpose of this experiment is to synthesize aspirin (acetyl salicylic acid) from salicylic acid and acetic anhydride. CO2H OH salicylic acid 2g 0.014 mole O O O CH3 H2SO4 ethyl acetate CO2H O O acetyl salicylic acid acetic acid CH3 O + H3C + H3C OH acetic anhydride 5 mL 0.05 mole The limiting reagent is salicylic acid. The theoretical yield of acetyl salicylic acid is 2.52 g. Physical Data:* mp MW salicylic acid 157-9˚ 138 acetyl salicylic acid
Premium Acetic acid Aspirin
Analysis of a Commercial Bleach Purpose: The purpose of this lab is to determine the amount of sodium hypochlorite (NaClO) in commercial bleach. This can be done by forming triiodide ions. To make the measurement more accurate‚ starch was added to help determine the endpoint of the solution. The significance of this lab is that industry can use these techniques to determine the amount of NaClO in the bleach of the rival industry and improve it. Hypothesis: The hypothesis is that‚ an accurate
Premium Iodine Titration Erlenmeyer flask
Illinois Central College CHEMISTRY 130 Laboratory Section: ________ Page 1 Name ______________________ Evaluation of the Gas Law Constant Objectives In this experiment‚ we will determine the Ideal Gas Constant‚ R‚ which relates the number of moles of gas present to its volume‚ pressure and absolute temperature. Background To see how "R" was derived‚ we must look at the proportionalities defined by the other fundamental gas laws. For example‚ Charles’ Law showed us that the volume of a gas sample
Free Pressure Ideal gas law Gas
EXPERIMENT A PREPARATION OF ASPIRIN Abstract This report gives a detailed account of the experimental preparation of aspirin in a laboratory environment as well as some basic industrial background on the product. It also contains information about safety precautions put in place to ensure the safety of the team who carried out the experiment. All results obtained have been included as well as a detailed analysis of what they represent alongside any improvements to the method used. Introduction
Premium Acetic acid Aspirin Acetic anhydride