Anhydrous sodium sulfate was added to the filtered organic solution to absorb excess water. Although water has a higher affinity towards sodium sulfate than cyclohexanol‚ excess anhydrous sodium sulfate may lead to the absorption of cyclohexane and thus loss of product. Anhydrous sodium sulfate absorbs water due to its polarity and therefore may also absorb cyclohexanol because of its polar O-H bond. If too much anhydrous sodium sulfate was added to the solution‚ part of the product would be absorbed
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Megan Entwistle‚ Maria Amos‚ and Paul Golubic CHEM 0330 Organic Lab 1 Sodium Borohydride Reduction: Diphenylmethanol from Benzophenone 11/16/11 Introduction Redox (shorthand for REDuction-OXidation) reactions are chemical reactions in which the oxidation state (or oxidation number) of atoms has changed. Oxidation can be observed through the loss of electrons or an increase in oxidation state by an atom‚ ion or molecule. Reduction describes the gain of electrons or decrease in oxidation state
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Sodium hydroxide‚ also known as caustic soda‚[2][3] or lye‚ is an inorganic compound with the chemical formula NaOH (also written as NaHO). It is a white solid‚ and is a highly caustic metallic base and alkali salt. It is available in pellets‚ flakes‚ granules‚ and as a 50% saturated solution.[citation needed] Sodium hydroxide is soluble in water‚ ethanol and methanol. This alkali is deliquescent and readily absorbs moisture and carbon dioxide in air. Sodium hydroxide is used in many industries
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Making Sodium Chloride Equipment: Method: 1. Firstly‚ safety measures were taken by putting on laboratory coats‚ wearing safety goggles and tying long hair back. This was to protect clothing‚ eyes and to avoid burning as the experiment included dealing with open flames. 2. The equipment needed (as shown and labelled in picture A) was collected. 3. Using a measuring cylinder for each‚ to be exact with measurements‚ we measured out 10cm³ of HCl and 10cm³
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The electron transfer reaction between hexacyanoferrate (III) and sodium borohydride resulted in the formation of hexacyanoferrate (II) ion and dihydrogen borate ion which was strongly catalyzed by AuNPs. The redox reaction is described as BH4- + 8 [Fe (CN)6]3- + 3H2O 8 [Fe(CN)6]4- + H2 BO3- + 8H+ The advantage of hexacyanoferrate ion for this redox study is that both oxidation states of iron (+2 and +3) are quite stable with respect to dissociation and hydrolysis
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KNES 470 Dr Rubin 4-18-12 Sodium Bicarbonate and Boxing Performance Boxing is a sport which relies on anaerobic power since it contains short-duration and high intensity work. A typical boxing match today consists of 3 minute rounds with a 1 minute seated recovery rest. When an athlete performs exercise at maximal level for more than 30 seconds‚ most of the energy comes from anaerobic glycolysis. During this process‚ lactic acid is produced which causes a decrease in pH levels within the muscle
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In the experiment‚ we tested a sodium chloride solution. Along with the tested solution‚ control groups (water and sodium phosphate) were used to be help understand whether or not NaCl was a buffer. Water was the negative control group and sodium phosphate was the positive control group. If NaCl was a buffer than the pH would be stabled as the sodium phosphate buffer. If NaCl was not a buffer than the pH would fluctuate like the negative control‚ water. During the first trial and prior to the drops
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12-STANDARDIZATION OF SODIUM HYDROXIDE Standard solutions for titrations are especially pure mixtures with exactly known concentrations. Primary standards are very pure solids. They have the advantage that they can be weighed (the analytical balance is normally the most accurate instrument in the laboratory) and they are stable under laboratory conditions. In this experiment‚ the primary standard is oxalic acid dihydrate‚ H2C2O4 ( 2H2O. It will be used to standardize a solution of sodium hydroxide
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believe that if the amount of sodium citrate is too low or too high‚ the sodium alginate solution would not form into a ball. The recommended amount of sodium citrate to be added to the sodium alginate solution was ⅛ teaspoon‚ or 0.5 grams. We supposed that if we exceeded this measurement‚ the sodium citrate would unbalance the whole solution‚ making the balls deform. If we added too little of the sodium citrate‚ we thought that there would be too little for the sodium citrate to fully do its job of
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Lab 4. Volumetric Determination of Impure Sodium Carbonate (Na2CO3) Introduction: To determine the total amount of carbonate in unrefined sodium carbonate‚ soda ash‚ a titration is done using a standardized solution of HCl. Aqueous HCl is a strong acid and therefore almost completely disassociates into H+ and CL-. Therefore‚ when HCl is used in a titration‚ the H+ is the titrant. Carbonate in aqueous solution is able to accept a proton‚ i.e. it acts as a base. When carbonate accepts the H+ a bicarbonate
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