Analysis of Soda Ash and Carbonate-Bicarbonate Mixture

The goal of this experiment is to have students obtain Potassium and Sodium Carbonates from wood ash. Wood ash contains a mixture of various minerals and compounds that are combined in a heterogeneous mixture. This mixture of minerals contains the wanted Potassium and Sodium Carbonates, and the students will conduct various purification processes in order to extract the Potassium and Sodium Carbonates. This lab experiment also demonstrates the difficulties our ancestors had when extracting these Carbonates. The principle behind how the carbonates can be purified is due to the minerals various solubilities in warm and cold conditions. The process of purification that the students completed was a series of mixture heating and filtrations. Each

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

The volume of carbon dioxide gas produced from a reaction was measured in order to determine what carbonate sample was used. A gas assembly apparatus was used to capture the gas from a reaction between an unknown carbonate and 6M hydrochloric acid; three trials were performed. The mass of the unknown carbonate was determined, and the reaction occurred in a test tube. The volume of gas produced by the reaction was measured, and the partial pressure of carbon dioxide was calculated after the partial pressure of water vapor was determined using Dalton’s Law of Partial Pressures. The percent mass of carbon dioxide gas was then calculated, and the average mass percent was compared to the table of known carbonates. It was concluded that the unknown carbonate sample used in the reaction was magnesium carbonate.

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

The amount of soda ash needed for the experiment was calculated using the following equation: sample weight of unknown=0.1103M (18ml×150.99)/(10×2× %〖Na〗_2 〖CO〗_3 ) An analytical balance was used to weight the calculated amount of soda ash. A piece of weighing paper instead of a weighing boat was used. The mass was recorded. The weighed soda ash was transferred into a 250 mL beaker, then the sample was dissolved in approximately 70 mL of water. The pH meter and electrode was obtained, rinsed with DI water, and calibrated using pH 7 and pH 4 buffer. A burette was obtained, mounted on a ring stand, and filled with the standardized HCl solution, that was prepared in Experiment 2. Since magnetic stirring bars and stirring plates were not available, the students

In this lab, the pH of seven different substances and solutions were tested both before and after the addition of multiple drops of acid (HCl), or base (NaOH). Depending on the variation of the affected pH from the original, the buffer range of the substance could be calculated by finding the average pH fluctuation, both with the added acid and the added base. As shown in the graph above, the buffer is labelled in dark blue, and the average pH fluctuation from the original was only 1.12. This low pH variation characterizes a buffer, and therefore, the tested solutions and substances with an average buffer range close to the buffer solution can also be considered buffers as well. For example, both lemon juice (magenta) and baking soda (yellow)

Phenolphthalein is a pH indicator that changes from colorless to pink upon a pH of around 8.2 to 10.0. Indicators are weak acids or bases that change colors at a designated pH. The reaction in this lab did not require phenolphthalein because the pH of the reaction was not near the pH range of phenolphthalein of around 8.2 to 10.0 that would only have been reached at or beyond the equivalency point. Phenolphthalein was added due to a procedure used in a previously laboratory experiment in which it was added in order to ensure that the equivalency point was not passed. The amount of weak acid solution that was to be titrated was below the recommended volume of 20 mL. Phenolphthalein is slightly acidic so upon its addition to a solution of low volume, the solution's pH would be

The Erlenmeyer flask containing distilled water and 1 milliliter of the original mixture then had 2 drops of the indicator phenolphthalein added. Sodium hydroxide from the buret was slowly added to titrate the mixture until the it remained light pink after being swirled. The final buret reading was then recorded and the concentration of ethanoic acid could be calculated. Once the round bottom flask had completed the heating process, it was removed from the hot water bath, cooled, and 1 milliliters of the mixture was transferred into an Erlenmeyer flask containing 25 milliliters of distilled water. The round bottom flask was then set up the same way as before heated for 30 additional minutes.

Immediately after removing the tubes, hydrogen peroxide was added to each tube up to the second (5 cm) mark. They were then swirled to mix, and after fifteen seconds, the bubble columns in each vile were measured in millimeters, and then recorded in a data table. The procedure for analyzing pH levels was rather different. The three test tubes, marked at three different levels, were each filled to the first mark (1cm) with catalase, and to the second mark (3 cm) with water. However, the pH of the water had been adjusted differently for each vile. The first tube received water adjusted to pH three, the second received water adjusted to pH seven, and third received pH eleven. Consequently, each tube was then filled to the last mark (7 cm) with hydrogen peroxide, swirled to mix and then observed after twenty seconds. After twenty seconds passed, the bubble columns of each of he tubes were measured in millimeters. Results were recorded on a chart.

The method I used in the experiment was followed by the lab manual of “Fundamentals of Life Science by Brenda Leady” (Leady 2017). We conducted an experiment of 8 different tests, 4 of the different classifications of pH, and 4 different

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.

The first step in this experiment was to construct a titrator and prepare the corresponding lab materials. After assembly and placement of the titrator it was filled with 10 mL of EDTA. To rid the titrator of air bubbles a few drops of EDTA were released before conducting the experiment. The next step in the experiment was to prepare the tap water and solution of pH 10 and EBT indicator powder. The 100 mL beaker was filled with 10 mL of tap water in addition to 5 drops of pH 10 buffer and approximately 10 mm of EBT indicator powder, which was placed below the

In order to test the acidic pH (5.0) a cocktail containg 20.0ml of disttiled water and 1.0ml of chloroplast suspension were used. Instead of interesting the neutral Ph, 6.0ml 0.2M phosphate buffer (pH 5.0). Each test tube, W, X, Y, Dark, and Room were given the exact parameters as activity I. A set distance was placed of 34cm, 70cm, and 99cm respectively for each letter variable and both positive and trial run. Furthermore, a standardized curve was created with the similar dilution factors of activity II, but 0.2M phosphate buffer (pH= 6.0) was replaced with 0.2M phosphate buffer

In this lab, the pH scale was used to determine which waters are most healthy to drink. The term ph means potential hydrogen. It is a measure of the hydrogen ion concentration when talking about a solution. If a solution has a high concentration of hydrogen ions, it will have a low pH and solutions with a low concentrations of H+ ions will result in a high pH. pH is a very well known water test to ensure that the water is healthy to drink. pH reveals the water’s acidity and it is a measurement of the potential activity of hydrogen ions. The pH scale is from 0 to 14. If one has a pH of 7.0 that is considered neutral. Solutions with a pH below 7.0, are considered acids. Solutions above 7.0 are considered basic. The purpose of this lab is to conduct

The Effect of 5 Drops of 0.1M Hydrochloric Acid (HCl) and Sodium Hydroxide (NaOH) on The pH Level of 5mL of Tap Water, Distilled Water, Commercial Buffer, and 10% Homogenized Potato Solution