Calculate the molarity of the original vinegar solution and its concentration in gdm-3, given that it reacts with NaOH in a 1:1 ratio. 7. 2.5 g of a sample of ethanedioic acid, H2C2O4.nH2O, was dissolved in water and the solution made up to 250 cm3. This solution was placed in a burette and 15.8 cm3 were required to neutralise 25 cm3 of 0.1 moldm-3 NaOH. Given that ethanedioic acid reacts with NaOH
Calculate the mass of KCl required to prepare 250. mL of 0.250 M solution. 3. Calculate the volume of 0.30 M KCl solution that contains 6.00 g of KCl. 6.00 g x 1 mole x 1 L = 0.27 L 74.6 g 0.30 mol 4. Calculate the volume of 0.250 M H2SO4 that contains 0.250 g H2SO4.
To perform this experiment, we will utilize emission spectra, titrations, and thermal gravimetric analysis, using knowledge from Experiments 10, 4, Titrations of Na2CO3 and NAHCO3 by HCl (hydrochloric acid) will be performed to determine the concentration of HCl, as well as the number of moles of HCl present within the sample of baking soda. As a result, we will be able to determine the molar concentration of HCl by determining its equivalence point (the point on the graph where the exact amount of rectant needed to perform a reaction has been added) from graphical analysis. Na2CO3(aq.) + HCl(aq.) ==> NaHCO3(aq.)
Results and Discussion For the first part of the experiment (Part A), five different 100 mL volumetric flasks were each filled with 1,2,3,4 and 5 mL of iron (II) solution. Then 5 mL of YY ligand, were poured to each of the five flasks. Each flask had 5 mL of 2M sodium acetate and 4 mL of 3M NH2OH. Then the whole solution was diluted up to the 100 mL fill mark with distilled water. This was the solution that was used in order to obtain the absorption spectrum for each of the different iron (II) ligand examples different flasks.
From your three trials, calculate the average volume of Na2S2O3 needed for the titration of 25.00mL of diluted bleach. 3. Use the average volume and the molarity of Na2S2O3 to determine the molarity of the diluted bleach. (Find moles of Na2S2O3, convert to moles of NaClO, and divide by volume of dilute bleach that was titrated in each trial to get M). 4.
Determination of the percentage purity of aspirin Introduction The aim of this experiment is to determine the percentage purity of 2-ethanoyl-hydrobenzoic acid (acetylsalicylic acid) in aspirin tablets. A known amount of standard sodium hydroxide solution is used in excess to hydrolyze a known mass of aspirin tablets: CH3COOC6H4COOH(s) + NaOH(aq) → C9H7O4Na(s) + H2O(l) The unused sodium hydroxide which remains is then titrated with standard nitric acid solution of 1 mol. NaOH(aq) + HCl(aq) → NaNO3(s) + H2O(l) The amount of alkali required for the hydrolysis can now be calculated and from the above equation, the amount of moles of acetylsalicylic acid which has been hydrolyzed can be found. Research question | Independent variablesnumber
Empirical formula: CH5N Steps for molecular formula: 1- Calculate the molar mass of the empirical formula. 2- Divide the known (given) molar mass by the calculated empirical formula molar mass to get a whole number 3- Multiply that whole number through subscripts of the empirical formula to obtain the molecular formula. Example CH5N 12.01 g C x 1 C= 12.01 g/mol 1.008 g H x 5 H = 5.040
Put exactly 5.0 mL of water in the 10.0 mL graduated cylinder. Record this volume in your data table (10.0 mL). Label the first pipet "Acid." To calibrate the pipet, fill it with LIU-2 water. Holding the pipet vertically, add 20 drops of water to the cylinder.
- Test tube - Distilled water - Volumetric flask. - LP4 tubes First 25ml of 0.1M Cupric Sulphate was made where the amount required was found in the following way... n=CV n-moles C-concentration V- Volume n= 0.1 x 25 x 10-3 =2.5 x 10-3 moles Then n = w/m n-moles w-mass required m- molecular weight 2.5 x 10-3 = w/249.71 molecular weight of CUSO4.5H2O=249.71 W = 0.624g Then as usual the solution was made by using the measured Cupric sulphate with the addition of water up to the point of 25ml in the volumetric flask. Then from the 0.1M stock solution of Cupric Sulphate the series of dilution was done as in the following table. The below mentioned volume of cupric sulphate was mixed with the corresponding volume of water as the final volume would be 2ml. The volume of cupric sulphate required for each concentration was calculated in the following way.
Micro – scale Reduction of a Ketone to an Alcohol: Benzophenone to Diphenylmethanol with Sodium Borohydride Abstract: Purpose of experiment 2.1 was to perform reduction reaction of benzophenone to diphenylmethanol with sodium borohydride as a reducing agent. The reducing agent was used in excess to ensure complete reduction of the carbonyl group. The product was isolated as a solid by filtration and its purity was checked using Thin Layer Chromatography with different ratios of mixture of polar and non – polar solvents and by checking its melting point, which was 520C - 620C. Infra – Red spectroscopy was not performed, however previously printed graphs were compared and analysed based on tables in Chemistry Laboratory Manual. Purpose of the Experiment: To produce diphenylmethanol from the reduction of benzophenone by using sodium borohydride as a reducing agent.