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    Standardizing a Sodium Hydroxide Solution

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    PURPOSE The purpose of this experiment is to use our knowledge from previous experiments to determine the exact concentration of a 0.1M sodium hydroxide solution by titration (Lab Guide pg.141). QUESTION The question that was proposed for investigation was: Can the exact concentration of 0.1M sodium hydroxide solution be determined by titration (Lab Guide pg. 141)? BACKGROUND DISCUSSION For this experiment we used titration to standardize the exact concentration of NaOH. Titration is the process

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    standardized solution of sodium hydroxide solution (NaOH) and to determine the concentration of given unknown sulfuric acid (H2SO4) solution. Analysis: This experiment is divided into two parts. In the first part; the standardized solution of sodium hydroxide is prepared by titrating it with base Potassium hydrogen phthalate (KHP). Phenolphthalein (range 8.3 to 10.0) is used as indicator to determine whether the titration is completed. Part A: Standardization of a sodium hydroxide solution NaOH Code sample

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    MATERIALS AND METHODS: Before the acetic acid solution could be titrated with sodium hydroxide (NaOH), the actual concentration of NaOH needed to be determined. By way of standardization, the actual concentration of NaOH was established, to account for the fact that the solid is not pure and for its tendency to react with carbon dioxide in the air. A 50 mL burette (±0.01 mL, Kimax) was rinsed thoroughly, twice with reverse osmosis water, and then twice with approximately 5 mL of ~0.25 M NaOH solution

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    Energy In this lab, we dissolved Sodium hydroxide, a strong base and corrosive, in 50ml of water to observe the change in temperature of the solution. At room temperature, sodium hydroxide is a white crystal-like odorless solid that absorbs moisture from the air. When dissolved in water or used to neutralized acid, it unleashes substantial heat which undoubtedly the predominant catalyst for the change in the energy. The heat that is produced by sodium hydroxide is sufficient to ignite combustible

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    Temperature Changes During the Addition of Sulphuric Acid and Sodium Hydroxide Solution Aim To investigate the temperature changes during the addition of sulphuric acid and sodium hydroxide solution. Introduction In this experiment we are using sodium hydroxide, sodium hydroxide, sulphuric acid. We are trying to find out how much acid it takes to neutralise alkaline. But there are many things that could effect my final result and I think that the main thing will be measuring the acid

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    Investigating a Neutralisation Reaction Between Hydrochloric Acid and Sodium Hydroxide To investigate a neutralisation reaction I must know all the factors that affect it in order to investigate in this. Here are all the factors; Temperature - This will defiantly affect an exothermic or endothermic reaction. Concentration - If the solution is made more concentrated it means it contains more particles of reactant, therefore more collisions are likely and an result of this is that the

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    Discussion Objectives: This experiment is monitoring the reaction of sodium hydroxide and crystal violet using spectroscopy. Graphical methods will be used to determine the kinetic rate law, rate constant and activation energy for the reaction. General Discussion: The order of hydroxide was determined by the varying the initial concentration of hydroxide in runs 1 and 2. We used the isolation method, which calls for having much higher concentrations of one reactant then the other, in this case

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    02L C=0.02/0.01887 n=0.01887 moles C=1.06M   Bottled Lemon Juice + Sodium Hydroxide Volume (mL) Titre Volume Initial Final mL L Rough 0.0 3.9 3.9 0.0039 Titration 1 3.9 7.6 3.7 0.0037 Titration 2 7.6 13.7 6.1 0.0061 Titration 3 13.7 19.1 5.4 0.0054 Average in Litres (not including rough) 0.00567 L C6H8O7 +3NaOH  3H2O + Na3C6H5O7 3NaOH C=1.06M n=CV V=0.02L n=(1.06)(0.02) n= ?moles n=0.0212 moles The ratio of sodium hydroxide to citric acid is 3:1 so the number of moles in citric acid is: 0.0212÷3=7

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    between sodium hydroxide (NaOH) and acetic acid that form sodium acetate (CH3COONa) and water (H2O) as follow. CH3COOH (aq) + NaOH (aq) CH3COONa (aq) + H2O (l) However, the method of volumetric analysis is highly dependent on a pure standard which the amount of substance present is accurately known. Prior to estimation of the acetic acid, sodium hydroxide (NaOH) was used as the standard solution. Thus, the concentration of the sodium hydroxide (NaOH) was first determined because sodium

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    Volumetric Analysis practical

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    acid which is Hydrochloric acid be calculated by using titration with a standardized base solution of Sodium Hydroxide? Hypothesis That the pH of the hydrochloric acid solution can be calculated using titration with a standardised sodium hydroxide base solution as long as concentration and temperature of base solution remain constant. Variables Independent variable Volume of base (sodium hydroxide) needed to titrate the acid solution Dependant Variable Volume of acid (hydrochloric acid) placed

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