Pre-Laboratory Assignment 1. What are the hazards associated with sodium hydroxide (NaOH) solution? Sodium hydroxide solutions‚ especially in high concentrations‚ are toxic and corrosive. 2. (a) What buret reading should you record when the liquid level is as shown in Figure 2? In Figure 2‚ the lower meniscus lies below the 3 mL line and 4 minor gradations that signify 0.1 values. Estimating the uncertain digit to be 0.04 mL‚ the reading we record for this particular buret is 3.44 mL.
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needed to be made‚ which was about four grams of NaOH placed into 200 mL of distilled water. After they were cleaned the titration process could now begin. The burets had to be filled with approximately fifty liters (record the level). Then measure about ten mL of the solution into another beaker (record exact amount). Take the distilled water and add ten mL. Then add three drops of phenolphthalein. Finally‚ begin titration with the base which is NaOH. Stop titrating when the acid stays pink for five
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Lab Report: Titration Lab Prepare a solution of a given concentration; understand titration including acid-base reactions‚ pH‚ stoichiometry and molar equivalence. Chemicals and equipment: NaOH pellets close to purity‚ HCl 3M‚ phenolphtalein Beckers‚ flasks‚ burette‚ magnetic or manual stir pHmeter Waste management: The waste disposal will be handled through neutralization of your excess reactant to a pH between 4.0 and 10.0 and disposal with abundant rinsing. As a preparation for the
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Acid Base Titration Purpose: The purpose is to calculate the molarity of a NaOH solution by titrating the base with 5mL of standard HCl solution in each trial. By adding the base with unknown molarity to the acid with 0.10M the molarity of NaOH can be calculated. The base‚ NaOH‚ helps bring the pH of the acid‚ HCl‚ closer to seven‚ which neutralizes it. When using the buret the amount of NaOH used is able to be determined. Then by writing a balanced chemical equation and using the titration
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solution until the substance being analyzed is just consumed. In this lab‚ experimenters using hydrochloric solution to react with the solution of NaOH according to this equation: HCl (aq)+ NaOH(aq) → NaCl(aq) + H2O(l) HCl is a strong acid‚ NaOH is also a strong base‚ therefore they will dissolve completely. By adding NaOH into HCl‚ the hydrogen ions neutralized with hydroxide ions‚ the theoretical endpoint and then the solution will be weak basic solution. The endpoint
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weak acid (acetic acid) titrates with a strong base (NaOH). In both titrations‚ we will monitor the change in PH to determine the volume of 0.100 M NaOH required neutralizing both 10ml sample of HCl and acetic acid. And refer to the neutralization reaction of these two acid‚ H+ (aq) + OH-(aq) → H2O(l) for HCl‚ and CH3COOH(aq) + OH-(aq) → CH3COO-(aq) + H2O(l) . as we can see ‚ in both case‚ two reaction have 1:1 stoichiometry‚ the moles of NaOH added = moles of acid present in the 10.00 mL sample
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Calorimetry: Enthalpy of Neutralization Introduction: The purpose of this lab experiment was to determine the molar concentration of the unknown HCl by using a coffee cup calorimeter. A coffee cup calorimeter is made of Styrofoam cups with a thermometer that is placed from the top and into the calorimeter to measure the temperature as the reaction happens. The Styrofoam cup used for the calorimeter creates an isolated system as it acts as a heat insulator between the cup and the surrounding
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constant and to observe the effect of different flow rates to the conversion. It is a homogenous reaction with only liquid phase is present. Also the reaction is endothermic. The saponification reaction is as follows; NaOH + EtOAc NaOAc + EtOH The reactants were taken as 1:1 ratios. 0.1 M NaOH and 0.1 M EtOAc was taken as reactants. The tank volume is 141 mL‚ the length of the reactor is 20 m and the diameter of the reactor is 1 mm. Reactor is placed in a water bath to keep the temperature constant during
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100-mL beaker of water. The 100 mL beaker was then placed on the assembled ring stand. Approximately 40 mL of the 0.1M NaOH was added to the 250 mL beaker. The 40-mL of NaOH was then added to the buret which was then attached to the ring stand. The LabQuest and the Vernier pH sensor was then hooked up and turned on to measure and graph the pH of the solution and the volume of NaOH. The Vernier pH sensor was then was placed in the solution and remained in the solution throughout the duration of the
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with the concentration of the components of a buffer. For a given addition of acid or base‚ the buffer component concentration ratio change less when the concentration are similar than what they are different. Materials: Acetic acid (MW=60 g/mol)‚ NaOH solution (0.5M)‚ HCl solution (0.001M)‚ calibration buffer (pH3.5 and pH 5.5)‚ 7-UP‚ 100 Plus. Apparatus: pH meter‚ pipettes (10mL)‚ volumetric flask (250mL)‚ beakers (150mL)‚ burettes‚ burette holder and stand‚ funnel‚ graduated
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