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 of carefully adding one solution from a buret to another substance in a flask until all of the substance in the flask has reacted. Standardizing is the process of determining a solutions concentration. When a solution has been standardized it is referred to as a standard solution. To know when a solution is at its end point an indicator is added to acidic solution. An indicator is an organic dye that is added to an acidic solution. The indicator is one color is in the acidic solution and another color in the basic solutions. An end point occurs when the organic dye changes colors to indicate that the reaction is over (Lab Guide pg. 141). Sample Calculations In this experiment three different equations were used and they are the Stoichiometry of Titration Reaction, Converting mL to L, and Calculating the Molarity of NaOH and HCl (Lab Guide pg. 142 and 143). Stoichiometry of Titration Reaction: H_3 O^+ (aq)+〖OH〗^- (aq)→2H_2 O (l) Converting mL to L: (_^V)NaOH=(24.42mL)(1L/1000mL)= 〖2.442×10〗^(-2) L (_^V)HCl=(25.00mL)(1L/1000mL)= 〖2.500×10〗^(-2) L Calculating the Molarity of NaOH and HCl: (_^M)NaOH=(((_^M)HCL)((_^V)HCl,L))/(((_^V)NaOH,L) ) PROCEDURE (Attached) STUDENT REPORT DATA SHEET (Attached) ANALYSIS OF DATA HYPOTHESIS: I hypothesize that by titrating a known amount of a substance in a solution, I can use the data from the experiment to calculate how many moles of the solution of the known concentration were required to completely react with the titrant and then using the formula C=n/V(in liters) to calculate the molarity of NaOH. OBSERVATIONS: In this experiment the Sodium Hydroxide solution went through three different phases where its quality and quantity changed. The first phase was called I. Preparing Approximately 0.1M NaOH, 1000mL of clear distilled water was boiled and then chilled to room temp.
Record the volume of the sodium thiosulfate solution used in the titration, and repeat the procedure in a duplicate titration.
We finally took 1ml of the 0.01% solution from test tube using the glucose pipette and adding it to test tube 4, we then used the H2O pipette and added 9ml of H2O to test tube 4 creating 10ml of 0.001% solution.
This lab contains two different procedures to titrating vinegar. One procedure uses phenolphthalein while the other uses a pH meter. Bothe procedures can be found on “An Analysis of a Household Acid: Titrating Vinegar” by the Department of Chemistry at APSU.
Afterwards, we conducted crystallization to evaporate the liquid in an attempt to detect the presence of a salt. Before stating which of the potential
We were then to make a base solution of 0.7 M NaOH. In order to standardize
The same procedure was done using 10ml of CV and 20ml of sodium hydroxide, both separately diluted to 50ml and added in a large beaker. The absorbance was recorded. In the last trial, 10ml of CV, 10ml of NaOH were diluted to 50ml. Before adding the two mixtures, 1ml of soap was added to the NaOH solution and then poured into a large beaker, along with the CV. Absorbance was recorded and the materials
Determining the Concentration Of Limewater Solution Aim: The aim of this experiment is it to find out the concentration of Limewater by performing a titration with hydrochloric acid which has concentration exactly 2.00M.. What is required for me is that I have to design my own experiment and chose the right and appropriate apparatus and equipment. I will be provided with 250cm3 of limewater, which has been made to which contains approximately 1g/dm3 of calcium Hydroxide. This hypothesis from www.studentcentral.co.uk We were also give Hydrochloric acid (HCl) with a concentration of 2.00 mol/dm3 normal laboratory apparatus was also given and so was an indicator.
Experiment: First prepared a well plate with the appropriate amounts of distilled water, HCl, and Na2S2O3 in each well according to the lab manual. The well where the reaction
In a 100ml beaker 30mls of water was placed the temperature of the water was recorded. 1 teaspoon of Ammonium Nitrate was added to the water and stirred until dissolved. The temperature was then recorded again. This was to see the difference between the initial temperature and the final temperature.
The resulting solution can then be titrated against hydrochloric acid with methyl orange as the indicator in order to determine how much urea was present initially.
Neutralization Experiment AIM:- To investigate how heat is given out in neutralizing sodium hydroxide (NaOH) using different concentrations of Hydrochloric Acid. Background Information:- Substances that neutralize acids are called alkalis. An acid is a substance that forms hydrogen ions (H+ ) when placed in water. It can also be described as a proton donor as it provides H+ ions. An example of an acid is hydrochloric acid (HCl), Sulphuric acid (H2SO4) etc.
viii. The experiment could have been performed over one a longer period of time day (rather than 14 days), which would have greatly reduced any loss of water from the sodium hydroxide solution, which may have improved results slightly.
As more NaOH is added, the pH will become more basic as H2C2O4 .2H2O has been completely neutralized and now an excess of OH- ions are present in the solution.12
This was done by using a pH strip and comparing the color to a pH chart. Once the pH of the wastewater was found, a wastewater titration was performed. A If the pH of the solution was a base, an 1 M HCl would be used as the titrant and vice versa. The software, capstone, was used to calculate the change in pH and the number of drops that passed through the drop counter while simultaneously creating a graph. 50 mL of the titrant (in this experiment it was HCl) was first placed in the burette, situated above the wastewater. Slowly the stopcock was opened letting the drops flow through the drop counter into the wastewater. The volume of the titrant dispensed over time was then calculated using the formula: [Drop Count (drops)] *
Firstly, we need to keep the chemical at a constant concentration. So, in this experiment we have chosen to keep hydrochloric acid at a constant concentration (5cm3). We could have, however, used Sodium Thiosulphate as a constant, but we had chosen to use Hydrochloric acid. Next, we must make sure that the solution is kept at a constant volume throughout the experiment. If the volume is different, then it could give different results if it was at a constant volume.