of this lab involved the standardization of the base NaOH with potassium hydrogen phthalate‚ or KHP. First‚ about 400 mL of NaOH (10 M) were poured into the 600-mL beaker. This was used to fill the burette. The 50-mL burette was rinsed through twice with 5 mL of NaOH. Then‚ the burette was mounted on the ring stand using a burette clamp and filled to 0 mL. Some of the NaOH was drained to fill the tip of the burette. The initial volume of NaOH‚ rounded to two decimal places‚ was recorded on a piece
Premium Titration Pink Erlenmeyer flask
number of moles of HCl reacted with the NaOH is 0.00216 moles‚ which is less than Gaviscon. The number of moles of NaOH that were added from the burette is 0.00327 moles (1 tablet of Gaviscon). However‚ for Quick-eze‚ the number of moles is 0.00216 moles (1 tablet). This means the average volume of the NaOH have affected the number of moles as the concentration of the sodium hydroxide is 0.1M. This means that if less NaOH was required to neutralise the acid‚ the number of moles of HCl neutralized by
Premium Acid Chemistry Water
An Introduction to Titration: Standardization of HCl and NaOH Lab Report Introduction: It is important to standardize solutions in order to have the accurate amount of concentration known. A standard solution can be prepared in either of two ways: A primary standard is carefully weighed‚ dissolved‚ and diluted accurately to a known volume. Its concentration can be calculated from this data. A solution is made to an approximate concentration and then standardized by titrating an accurately weighed
Premium Titration Sodium hydroxide Chemistry
Methods/Procedure: First begin by mixing up and standardizing a 500mL solution of NaOH to titrate. For each of the six bottles‚ measure the directed amounts of ester‚ water‚ alcohol‚ and HCl. The bottles of different solutions will be left to come to equilibrium for two weeks. Once the NaOH is standardized‚ the solutions in the bottles have come to equilibrium‚ and a molarity is calculated‚ use the molarity of NaOH to discover how many mols were used to neutralize the solutions in each bottle. Once
Free PH Acid dissociation constant Hydrochloric acid
Add 0.5 g of eggshell dust to each beaker‚ measured by balance. While the reaction of eggshell with acid occurs‚ prepare the buret and clamp for titration. Make sure they are clean. Pour NaOH solution into the buret to the ’0’ level. Make sure all of the eggshell reacted with the HCl. If not‚ you can help the reaction by using the baguette. Put two drops of phenolophateine into each beaker using the plastic pipette. Take the first beaker and titrate the
Premium Calcium carbonate Titration
reaction will be measured using a styrofoam calorimeter. The three reaction are shown below. Reaction 1: The dissolving of solid sodium hydroxide in water. NaOH(s) ---> Na+(aq) + OH-(aq) + heat Reaction 2: The reaction of solid sodium hydroxide with dilute hydrochloric acid. NaOH(s) + H+(aq) + Cl-(aq) ---> Na+(aq) + Cl-(aq) + H2O Reaction 3: The reaction of sodium hydroxide solution with dilute hydrochloric acid solution. Na+(aq) + OH-(aq) + H+(aq)
Premium Sodium hydroxide Chlorine Hydrochloric acid
Joseph Corey‚ Chris‚ Grant Thermodynamics – Enthalpy of Reaction and Hess’s Law I. Purpose The purpose of this lab is to verify Hess’s Law through the three reactions of NaOH and HCl‚ NH4Cl and NaOH‚ and NH3 and HCl. The sum of the enthalpies of the first two reactions should equal the enthalpy of the third reaction. II. Background Hess’s Law is used to determine the enthalpy of a reaction from adding two or more preceding reactions. To determine the enthalpies of certain
Free Enthalpy Thermodynamics Temperature
the experiment was applying macroscale titration to calculate the mass of an HCl solution consumed that was initially done by pounding the tablets and getting a weight of 0.15 grams. The powdered form antacid was mixed with 100mL of 0.1M HCl in the erlenmeyer flask. It was stirred and heated until it boiled then was filtered. Two drops of phenolphthalein was added to the filtered solution. It was titrated with 0.1M NaOH until its color turned pink. The procedure was repeated for the second trial
Premium PH Acid PH indicator
Chemical Equilibrium Lab Report Aim: The aim of the lab “Chemical Equilibrium” is to observe the effects of changes in concentrations of products and reactants on the position of the equilibrium of given chemical reactions. Background Information: We are going to use our knowledge of the Le Chatelier’s principle in order to observe this experiment. The principle states that the equilibrium will shift in the direction that will minimize the effects of the change. This lab consists of two
Premium Chemical reaction Change Chemistry
instructor to dilute the 6M NaOH to 0.1M in 300mls instead of 500mls in Part B of Experiment 21. One objective for performing these two experiments was to observe qualitatively the reactions between common acids‚ bases‚ and the indicators phenolphthalein‚ methyl orange‚ bromothymol blue‚ and red cabbage extract. Another focus of this experiment was to perform a
Premium Chemistry Acid Sodium hydroxide