Sodium hydroxide

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    Experiment to investigate the amount of sodium hydroxide needed to neutralize the solution of vinegar CH3COOH(aq) + NaOH(aq) -> CH3COONa(aq) + H2O(l) (Reaction between sodium hydroxide and solution of vinegar, which produces an aqueous solution of sodium acetate and water) Hypothesis: Approximately 8.8ml of sodium hydroxide will be required to neutralize 100ml of acetic acid. (http://schoolworkhelper.net/titration-of-vinegar-lab-answers/) -----------------------------------

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    Procedure [C, 8] Part A: Iron (III) Nitrate and Sodium Hydroxide 1. Sliding the mini test tube into the empty Erlenmeyer flask and sealing it with the rubber stopper were practiced a few times before conducting the experiment. 2. 5 ml of Sodium Hydroxide solution was measured using the graduated cylinder. After, it was poured into the empty Erlenmeyer Flask. 3. 3 ml of Iron(III) Nitrate was poured into the mini test tube. Next, the Erlenmeyer Flask was tilted and the mini test tube

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    EXPERIMENT: 1 AIM: To prepare 100 ml of 0.1M NaOH (Sodium hydroxide) solution. MATERIALS REQUIRED: NaOH, beaker, distilled water, measuring cylinder, stirrer, weighing machine, paper. THEORY: NaOH is an organic compound aka caustic soda. It has Na+ as cationic part and OH− as anionic part. At ambient ordinary temperature this alkali decomposes protein causing severe burns. It is highly soluble in water and absorbs moisture and carbon dioxide from air. In many industries pulp and paper, textiles

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    Discovering the Concentration of Sodium Hydroxide and Citric Acid Introduction: This laboratory experiment focuses on determining the quantity of a substance that is existing in a certain solution, by using titration in the experiment, (French et al. 2014). A hypothesis for this experiment is that the unknown concentration of a solution will be identified. The objectives are to identify the concentration of citric acid and the concentration of sodium hydroxide in solutions of unknown concentration

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    To conduct a reaction between solutions of a weak acid and sodium hydroxide. • Determine the half-way point of titration of an acid-base reaction. • To calculate the pKa and the Ka for the weak acid. • To calculate Molar Mass of a weak acid from the titration results. • To determine the identity of a weak acid. Introduction: The purpose of this experiment is to identify an unknown weak acid by titration with a standard sodium hydroxide solution. The pH of the titration solution will be monitored

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    Stephanie Thao Chemistry 1151 Laboratory Analysis of acid by titration with sodium hydroxide Ms. Hoang November 2012 Introduction: The purpose of this experiment is to demonstrate an example of how to determine the unknown molarity of hydrochloric acid by titration with a base (sodium hydroxide). Titration is a common laboratory method of quantitative chemical analysis that is used to determine the unknown concentration of an identified analyte (wekipedia). The first step will be measuring

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    were used are ethyl acetate and sodium hydroxide in a saponification reaction. The expected products were sodium acetate and ethanol. This reaction was conducted in a batch reactor in isothermic conditions and adiabatic conditions. The variables of interest in this reaction are Conductivity, temperature, time and concentration. The reactants used were 400 ml of 5.0% ethyl acetate and 400 ml of 2.3% Sodium hydroxide. This is equivalent to 9.2 grams of sodium hydroxide which has 0.23 moles. The measured

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    This experiment tested the hypothesis that there was no difference between cellular respiration before vigorous exercise and cellular respiration after vigorous exercise in terms of rate of cellular respiration. During cellular respiration, glucose broke down into carbon dioxide in order to convert the chemical energy stored in glucose into usable energy in ATP. Cells did not perform cellular respiration to create carbon dioxide, for carbon dioxide was a byproduct, and thus, carbon dioxide was released

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    were performed order to experimentally determine the rate constant(k), for the rate of the reaction of the crystal violet solution and sodium hydroxide. To start, a Beers Law calibration experiment was conduction. Also, two kinetic experiments were ran using both 5ml and 10ml of sedum hydroxide in order to determine the reaction order(k^1), of the sodium hydroxide. The Beers Law calibration experiment used many concentrations of crystal violet solutions. Each of these solutions were test and analyzed

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    The organic phase was then added back into the separating funnel with 40ml of 0.1M sodium hydroxide solution and shaken well for 2 minutes. The organic phase was released and disposed of and the aqueous phase was kept and transferred to a 250ml volumetric flask and the volume was made up with 0.1M sodium hydroxide. Standards were then made using the 50mg/L standard provided and mixing with 0.1M sodium hydroxide to create standards with 1,2,3,4,5 mg/L concentrations. Each solution was run through

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