Methyl Orange Synthesis Lab Report

That mixture was then filtered through a coffee filter. Nine test tubes were prepared in order to perform this dye coupled reaction. One contained 5.0ml of the potato and pH buffer mixture, 2.0 ml of hydrogen peroxide, and 1.0 of guaiacol to serve as a blank for the spectrophotometer. Four test tubes were filled with 2.0 ml of hydrogen peroxide and 1.0 ml of guaiacol, used for measurement by the spectrophotometer, each. The last four were filled with 4.0 ml of the potato and pH buffer mixture and 1.0 ml of peroxidase.

Name Lab Section Course Code Drawer Number Date The Reaction of a Food Dye with Bleach Introduction The goal of this experiment was to determine the reaction of a food dye with a bleach, x. It was hypothesized that x would be in 1st order with respect to the dye. By examining the slope of the line, the concentration vs. time graph was used to determine the value of x. It was hypothesized that a graph of In[A]versus time would produce a linear line; the order of x with respect to [A] would be first order.

Two titration were performed for each buffer: HCl and NaOH. A pH meter was used to record the pH change, and the volume of the buret was recorded every .1 change in pH. This potentiometric titration method was stop once the solution change by 2 pH units. The

Each sample of solution #3 being tested by the three reagents will have the most noticeable change in color in result of a positive reaction between solution #3 and the reagent. 5. We took three samples of three solutions, a positive control, and a negative control (fifteen test tubes total.) Each sample was tested by Benedict’s, Biuret’s, and Lugol’s Reagent for a reaction. The result of the reaction was then recorded in notes.

The nitronium ion mixture was slowly added to the concentrated sulfuric acid methyl benzoate mixture to prevent vigorous reaction that if present could lead to unwanted dinitro by-products. The mixture after settling and heating to room temperature was poured over ice in order to rapidly cool the sample inducing formation of the crystals. The water was allowed to melt before it was vacuum filtered to neutralize the acid that might be remaining

Beginning with the principles, Brønsted-Lowry acid base theory demonstrates that an acid donates a hydrogen ions, while a base accepts hydrogen ions. Strong acids have the an easier ability to donate hydrogen ions compared to weak acids. The goal for Experiment 8 Acid-Base Equilibria: Determination of Acid Ionization Constants is to recognize how different amounts of quantitative values can alter the pH in a solution. This procedure was carried out by mixinging specific acid or base solutions together and comparing the experimental value with the actual accepted value.

The central purpose of this experiment was to determine the experimental empirical formula of an oxide of magnesium by performing a synthesis reaction. It was hypothesized that the formula that was derived from the recorded data would be identical to the theoretical empirical formula. After performing calculations with the data that had been collected within the duration of the experiment, it was deduced that the empirical formula of the product generated by the synthesis reaction was Mg5O6. Since the calculated formula did not match the postulated formula, MgO, the inceptive hypothesis was confuted. There was a large discrepancy in the results of students who replicated this experiment, the variation in data possibly having been evoked by the dissimilarity in

The purpose of this laboratory experiment was to identify the molarities of dye present in green Powerade and then create a solution that possessed the same concentrations. This experiment consisted of two parts of experimentation, the first part focused on identifying the dyes present and at what concentration, and the second part focused on the recreation of the stock solution. To successfully complete this experiment, a small cuvette, full of 2 mL of green Powerade, was placed into a UV spectrometer in order to identify which wavelengths were being absorbed and reflected. With this information a complete series of dilutions using yellow #5 and blue #1 dye in ratios of 1:1, 1:2, 1:3, 1:4, and 1:5 were conducted to find the max peak absorbancy

The maximally effective pH was determined to be approximately 5. The maximally effective temperature was determined to be 37°C. The Q10

In this lab, our hypothesis was proven for the most part. All primary colors (red, blue, and yellow) had no color change, while secondary colors (black, brown, green, purple) changed colors and had two or more dyes. The only exception to the statement was orange. While there is no orange dye, the dyes for yellow and red are so similar that there would be no change in color. Another possibility is that the dyes were not attracted to the solvent so they did not separate.

Pigments from the red cabbage help determine the pH of a solution. The pH scale is used to measure how acidic or basic a solution is. The scale used ranges from 0-14; a pH of 7 is neutral, less than 7 would be acidic and greater than 7 would be basic [1]. A pH indicator is used as a chemical detector for hydroxide and hydrogen molecules [2]. In the experiment, the red cabbage pigment called Anthocyanin was used as a pH indicator.

Blue vitrial (copper sulphate) also bring out green colours. The copper sulphate does not need others substances to perform. Its only perform by itself. The treated fabric need to be rinse well and caution blue vitriol is poisonous. Tannic acid is a mordant for great colours for tans or browns.

After preparing a solvent mixture, it was titrated with sodium thiosulphate but during titration time color change was not observed. The experiment was not completed successfully. METHODS AND MATERIALS A) Iodine Value: Hanus

The pH level of water tells you how acidic it is.

A clean 250-mL beaker was taken and around 0.3 to 0.5 g of potassium acid phthalate was weighed into it. 50 mL of distilled water was approximately added to this 250 mL beaker and gently swirled so that the solid (potassium acid phthalate) got fully dissolved into the water. 2 drops of phenolphthalein indicator solution was added to the beaker. The pH electrode was calibrated using the pH buffers.