titration will be used to determine the concentration of HCl at equilibrium when it reacts with the NaOH H+ (aq)+ Cl- (aq) + Na+ (aq) + OH- →H2O(l) + Na+ (aq)+ Cl- (aq) Procedure When performing this experiment one must first obtain and wear goggles. Next add 40mL of distilled water to a 100mL beaker‚ then add 5.00mL of HCl to the beaker.Then obtain 40mL of 0.1M NaOH. Place the NaOH in a 60mL reagent reservoir and drain a small amount into a 250mL beaker to fill the tip. Connect the
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experiment‚ a weak electrolyte‚ phenol is used‚ and the change in enthalpy is endothermic‚ ΔH=q=25.3kJ/mol. The first part of this experiment involves the neutralization of strong electrolytes. 40 mL of 2.0 M HCL was used to neutralized 50 mL of 2.0 M NaOH. Both the solutions were mixed in the calorimeter and the temperature was recorded after 2 seconds until it reaches maximum‚ then every 10 seconds for one minutes‚ and finally every 30 seconds
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in commercial vinegar Introduction: The aim of the experiment was to determine the molarity of ethanoic acid in table vinegar by titrating a sample with alkali sodium hydroxide (NaOH) with a known concentration of 0.1molL-1. The equation of the reaction between ethanoic acid and sodium hydroxide is as follows: CH3COOH + NaOH CH3COONa + H2O When the titrations end point is determined and volumes of reactants are measured the concentration of the ethanoic acid can be calculated. Keywords:
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presence of polypeptide chains while for the rennin test‚ curd formations were observed in test tubes 3 and 4 only. In gastric analysis‚ the values for free acidity and total acidity were computed. The free acidity is 20.83 N NaOH/ 100 ml sample while the total acidity is 20.0 N NaOH /100 ml sample. Lactic test was also performed in in relation with the gastric analysis. Addition of gastric juice to FeCl2 was done to determine the presence of lactic acid‚ in which a distinct canary yellow color gives
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10 ml of acid was used for all the three trials to keep a constant. During the first trial it took 3.700 ml of NaOH to titrate the HCl‚ in the second trial it took 3.750 ml‚ and in the third trial it took 3.750 ml. These differences in amounts of NaOH required to titrate the acid led to different molarities being calculated for the NaOH. The first being 0.270M and the other to being 0.267M. In order to calculate the total volume of base used‚ the readings from the burette
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Titration with an Indicator 1. Fill the 50-milliliter buret with a 0.25 molar NaOH solution. 2. Record volume. 3. Measure out between 20 milliliters and 40 milliliters of the unknown HCl solution. 4. Record volume. 5. The amount of unknown HCl is then added to the 100-milliliter Erlenmeyer flask. 6. Add two drops of the indicator‚ phenolphthalein‚ to the acid in the flask. 7. Using the slider on the right hand side‚ add NaOH to the HCl in the Erlenmeyer flask (This action is known as titrate).
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two 50.00cm3 measuring cylinders‚ stopwatch‚ three 80cm3 beakers‚ dropper Variables: Manipulated variable: Type of acids used In this experiment‚ type of acids used would be manipulating variable. Different acids such as HCl or CH3COOH are added to NaOH respectively and measure the increase in temperature respectively. Responding variable: Temperature‚ T Responding variable will be the temperature. First‚ we have to measure and record the initial temperature of the sodium hydroxide solution. After
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paper under your beaker to help observe the change in color. Fill the syringe from the top with NaOH from the dropper bottle with 9-10 mL of the 0.5 M NaOH solution. Let a few drops drip into the beaker to be sure there is no air in the tip of the titrator. Pour in drain and flush with water‚ wash and dry beaker to be use in the experiment Experiment: Read and record the intial volume of the NaOH solution in the titrator on your data table. Use a graduated cylinder to measure 5 mL of vinegar
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of sodium hydroxide‚ NaOH(aq). In this investigation‚ students are to act as quality control chemists. Their purpose is to test the acetic acid concentration of the vinegar to discover whether it has been diluted. In this theoretical report‚ the manufacturer claims on the label that the vinegar contains 5% (0.87 mol/L) acetic acid. Thus‚ the concentration of acetic acid in the vinegar sample should be the same. Materials * Lab apron * Eye protection * NaOH(aq) * Vinegar
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mL H2O | Mass of NaOH | 2.535 g NaOH | Initial temperature in calorimeter | 24.2 °C | Final temperature in calorimeter | 27.8 °C | Calculations: Show your work and write a short explanation with each calculation. 1. Write out a balanced "equation" for the process you investigated in Part I‚ including phase symbols. NaOH(s) + H2O(l) --> NaOH(aq) 2. Calculate the number of moles of sodium hydroxide dissolved. Show your work. Moles NaOH = 2.535 grams NaOH X (1 mol/40.00 grams)
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