Titration Investigation Essay examples

Sometimes in chemistry, the concentration of a solution is not known, and titration is the process of determining that concentration. The goal of this experiment is to determine the concentration of an NaOH solution and a citric acid solution with the greatest possible accuracy. The unknown concentration of the analyte is found by comparing it to the known concentration of the standard solution. An acid and a base form a salt and water upon reaction; thus, the pH of the solution should be neutral at the end of the titration. The base used for this experiment is NaOH, sodium hydroxide. During the titration, and equivalence point is hit when the moles of H^+ and 〖OH〗^- are equal, regardless of

A suitable indicator for determining the endpoint in the neutralization of a weak acid with a strong base is phenolphthalein. Phenolphthalein has a pH range of 8-10. It is colorless in acidic and neutral solutions. According to the titration curve of a weak acid-strong base titration, the pH at the end point is basic. Phenolphthalein only changes color when the solution becomes basic. Hence, it is an ideal indicator for this lab because it will change color when the end point is reached.

While the goal of this lab was mainly to be able to perform an acid-base titration. Complete a traditional titration and then and a pH electrode titration. Calculate the molarity of citric acid from the titration volume of NaOH. Calculations should be fairly close in average and the ending point should coincide with the equivalence point. All while effectively being able to compare and contrast the two methods to detect the endpoints of an acid-base titration.

Acid-Base titration is a method used to find the unknown pH of solution through measuring the amount of Basic added to an Acidic compound (Sparknotes.com, 2016). In a titration process, one chemical’s concentration has to be known, after the solution has been neutralised using the formula C2 = (V1 x C1)/V2 as it measures the amount of hydrogen ions (C2) that are in the mixture. This process and formula allow for the aim of the experiment to be completed as, if the amount of hydrogen ions in the solutions is known, then the aim of the experiment is

In this experiment we will be titrating the titrant sodium hydroxide against the analyte, which is the substance being analyzed, hydrochloric acid. Titration is the process of analyzing base and acid added together. The objective is to calculate the unknown concentration of hydrochloric acid with the standardized solution of solid sodium hydroxide. The standardized solution is the known concentration but since sodium hydroxide naturally reacts with air, we must first determine the true concentration of NaOH by titrating against a weak acid, potassium hydrogen phthalate (KHP) that is the known concentration.

The data stored in the device was then transferred to a computer and saved. The charts and data collected can be found on the last page. The volume of NaOH used to reach the equivalence point was calculated for each of the three titrations. The equivalence point was found graphically. Using the volume of NaOH and the molarity of NaOH, the moles of NaOH were calculated. Using the volume of the soda used, the molarity of citric acid was found. Then the mean and standard deviation of the molarity of citric acid was calculated.

Abstract: The experimental experiment will be to make pH measurements and make a titration curve that will result the weak acid we are trying to identify. This procedure will be done twice to make sure the same characteristics of the unknown are both constant. The volume of the drop counter will be noted in the graph to help distinguish the molarity of the solution which will be noted in MicroLab.

Abstract: In this experiment, our team analyzed an unknown acid and a sample of vinegar solution by the process of titration using a 0.1 M sodium hydroxide solution as the titrant, as this solution is a strong base. In addition, our team members used phenolphthalein as indicator in the reaction.

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. In order to discover the concentration of a solution, acid-base titration must be executed during the experiment, (French et al. 2014). The standard solution (known concentration) is reacted entirely during titration due to stoichiometry located in the equation, and because the chemical reaction is between a base and an acid, the products formed from the reaction will be salt and water, (French et al. 2014). The equivalence point occurring in an acid-base titration will have the same amount of moles in H+ as in OH-. The equations that are used for this acid-base titration are as follows:

The pH probe of the device was rinsed in distilled water between every measurement to return back the pH of the probe to a neutral pH, and between tests to avert cross contamination of solutions. This procedure was repeated two times for attaining Waterfall Gully, Johnston’s Creek and Port Adelaide River pH. The Dhaka water sample was tested via titration method which is used to measure the unknown concentration of a known reactant. This involves reacted a known volume of a known concentration solution (a standard solution), with a measured volume of the volume of unknown concentration. The solutions are mixed until they just react completely. In an acid-base titration, an indicator allows to determine when the reaction has reached an endpoint. The method for titration used was that a burette was rinsed with 10ml of 0.1M NaOH(aq). A stand, clamp and flask were obtained and set up making sure there was about 5cm between the burette and the flask. Stopcock of burette must be shut, then the burette was filled with 0.1M NaOH(aq) until the reading was between 0 and 1ml. This value was then recorded as initial value. The 20ml pipette was cleaned with 5ml of HCl. 20ml HCl was transferred to 250ml conical flask. 5 drops of phenolphthalein were added. The titration began by opening stopcock to add 0.1M NaOH(aq) to the flask. To detain a light pink colour the solution must be constantly mixing and swirling. When it starts to go

Introduction: The purpose of this experiment is to identify an unknown weak acid by titration with a standard sodium hydroxide solution.

This experiment introduces us the pH measurement and application of macroscale titration of aqueous solutions of acids and bases. The first part of 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 universal indicator is used for specifying whether a substance is a Base, Neutral, or an Acid along the pH scale, by measuring the concentration of H3O+ ions in a substance. (N.a, 2016) The pH scale is a scale that determines whether a substance is an Acid product, or a Basic product. The ‘H’ in pH stands for Hydrogen, however, the ‘p’ is often debated, therefore is thought of as the power of the hydrogen. (Morrissey, 2016) The pH scales ranges from ranking between 0 (Being more

The size of (NaOH) was reduced to about 0.1 mL per intervals. A titration curve was made for 0.20 M of Formic Acid and results were shared in class. After the data has been collected from the rest of the class, compare and contrast the properties of various acids titrated with a strong base. Keep in mind that that the pH of the strong acid reacted with strong base will give a pH of about 7 and a weak acid with a strong base will give a pH higher then 7.

pH indicator Iodine solution Fehling solution A and Fehling solution B Ammonium chloride solution Ammonium hvdroxide Ammonium oxalate Potassium sulphocynaide solution