(b) Calculate the volume of 0.2M UO3- needed to react with 20.00 cm3 of 0.1M Cr2O72-. 3. 24.40 g of hydrated iron(II) sulphate, FeSO4.xH2O was dissolved and made up to 1.0 dm3 of aqueous solution, acidified with sulphuric acid. 25.00 cm3 of the solution was titrated with 20.00 cm3 of 0.022M potassium manganate(VII) solution for complete oxidation. a) Write the equation for the reaction.
Controlled The controlled variables of the experiment were: A. The volume and concentration of the Hydrochloric acid. B. The concentration of the Sodium Hydroxide. Equipment List * Boiling Tube * 10 cm3 1mol dm-3 Hydrochloric Acid (HCL) * 15 cm3 1mol dm-3 Sodium Hydroxide (NaOH) * pH and Temperature Probes * Data Logger * Measuring Cylinder ‘ * Boiling Tube * Teat Pipette Method * Add 10ml of Hydrochloric acid, measured in a measuring cylinder, into a boiling tube.
Calculate the surface area of the circle formed (πd2/4): Surface area = .785 cm2 2. Calculate the number of molecules on the top layer. We must convert the surface area in centimeters squared to nanometers squared and then multiple that by the surface area of a sodium stearate molecule. Convert the surface area of the circle formed (#1) to molecules per layer using the matrix below: Answer = 4.76*10^14 molecules/top layer 3. Calculate the concentration of grams of sodium stearate per milliliter of diluted solution.
The molar mass of a compound or atom is the mass of 1 mole of anything; this is relative to the atomic mass from the periodic table. The percentage yield from an experiment would be the actual yield divided by the theoretical yield multiplied by 100. We need to know how to balance chemical equations due to law of conservation of mass. Being able to turn moles into mass and mass into moles through the equation “m=nM” rearranged to find out other components. We need to be able to find the limiting reagent and be able to go through the process of gravimetric stoichiometry.
Lab 4: Determination of Percent by Mass of the Composition in a Mixture by Gravimetric Analysis Introduction Thermal gravimetric analysis is used to determine the percent by mass is used to determine the percent by mass of a component in a mixture. When a mixture is heated to an appropriately high temperature, one component in the mixture decomposes to form a gaseous compound. The mass of this particular component is related to the mass of the gaseous compound. In this experiment, the percent by mass of sodium hydrogen carbonate (NaHCO3) and potassium chloride (KCl) in a mixture will be determined. Experimental First, we weighed 2 samples, each has 1 gram of NaHCO3-KCl mixture Second, we put the samples in 2 crucibles (A and B) and weighed them.
Percent H2O in Hydrate is equal 0.34/2.33=14.6% 3. The general formula of barium chloride hydrate is BaClg-nHZO, where n is the number of water molecules. Calculate the theoretical percent water for each value of n—divide the sum of the atomic masses due to the water molecules by the sum of all the atomic masses in the hydrate, and multiply the result by 100. Complete the table. | BaCl2 | BaCl2•H2O | BaCl2•2H2O | BaCl•3H2O | Sum of atomic masses (BaCl2) | 208.23 | 208.23 | 208.23 | 208.23 | Sum of atomic masses (nH2O) | 0 | 18.02 | 36.04 | 54.06 | Sum of atomic masses (hydrate) | 208.23 | 226.25 | 244.27 | 262.29 | Percent water in hydrate (theoretical) | 0% | 7.96% | 14.75% | 20.61% | In this lab we used a Balance, centigram
Part B: The graduated pipet’s average density at 22.3 °C was determined to be 0.9785g/mL with a percentage error of 1.89% shows the graduated pipet to be more accurate and precise. Part C: Density of an unknown NaCl solution was measured and a calibration curve used to determine the percentage of NaCl by mass in the solution. y=0.007x + 0.998 which concluded that the concentration of the sodium chloride solution was 3.14%. INTRODUCTION Anything that you can see, touch, taste or smell, occupies space and has mass, it is called matter. Matter can be a gas, a liquid,
Report of chemistry experiment on redox titration Name: Beverly Wong 6S (26) Date: 28-10-2010 An analysis of iron tables 1. Objectives To find out the actual percentage of iron (Ⅱ) ions are in a particular brand of iron tables and compare the result with the quantity claimed by the producer. 2. Introduction of the experiment Iron tables usually contain iron (Ⅱ) sulphate which is soluble in water. Assuming all the iron in the tables is in the form of iron (Ⅱ), Fe2+.
P.V. is defined as milliequivalent peroxide per 1000g fat. As mentioned, peroxide is produced during lipid oxidation. PV test thus base on the fact that iodine produced by reaction of KI and lipid is proportional to the amount of peroxides generated in oil. ROOH + 2KI I2 + 2KOH + RO- The amount of Iodine produced can be further determined by titration with sodium thiosulphate (NaS2O3) using soluble starch to indicate the endpoint (color change from blue to colorless) I2+NaS2O3 S2O3 + 2NaI After the titrations, we can calculate the P.V.
Reversely, in reduction reactions, the oxidation number is decreased. For the oxidation-reduction reaction to occur, the two half-reactions must be combined to form a redox reaction. For easy comparison, all half-cell reactions depicted as reductions, and the tendency for reduction to occur is known as the reduction potential, “E.” When the conditions are standard at 25ºC with 1M concentrations, the reduction potential is referred to as the standard reduction potential, “E°.” Both potentials are measured in volts. There are several standard potentials that have been measured and recorded. Voltaic/Galvanic cells are a particular type of redox reaction that involves the creation of a spontaneous electric current.