Investigation Of Chemistry Involving Quantitative Analysis

We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30

The preparation for the experiment started by gathering the solutions of enzyme Peroxidase, substrate hydrogen peroxide, the indicator guaiacol and distilled water. Two small spectrometer tubes and three large test tubes with numbered labels. In addition, one test tube rack, one pipet pump and a box of kimwipes were also gathered. Before the experiment, the spectrometer must be set up to use by flipping the power switch to on. Following, the machine was warmed up for 10 minutes and the filter lever was moved to the left. In addition, I set the wavelength to 500 nm with the wavelength control knob. Before the experiment, I had to create the blank solution by pipetting 0.1 ml of guaiacol, 1.0 ml of turnip extract and 8.9 ml water into tube #1. Following the creation of the blank, a control 2% solution was created.

B.|HCl + BTB|A3|The mixture turned yellow instantly. Under white paper the mixture was more of mustard yellow and under black paper it was less of a bright yellow. |

After the twenty minutes elapsed, the flask was cooled to room temperature and then titrated with the remaining NaOH until the colorless solution remained pink. The final volume was then recorded. While solution #1 was heating the same process was repeated with solution#2 and the second burette

In this experiment redox-based titrimetric analysis was used to determine the amount of ascorbic acid (Vitamin C) contained in a serving of lemonade. This was done to confirm the 100 percent recommended daily allowance claimed on the package for a serving of Country Time Lemonade. The titration method used was adding a thyodene indicator to the analyte (lemonade solution) there is a visible colour change when the endpoint of the reaction between the titrant (KIO3) and the analyte occurs. The following reactions show how this titration method is viable. (Draw in reactions) KIO3 first reduced with iodide (I-) to generate iodine (I2 ) which then oxidized the ascorbic acid within the lemonade. Once all the ascorbic acid had reacted any iodine

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

Table 4.20 and Table 4.21 shows the readings for the test conducted at pH11 for cationic and anionic dye solutions. From the readings it was seen that least color removal of 81.49% for cationic dye and 70.21% for anionic dye was obtained at WTR dose of 120mg/L at pH11 for both the set of dyes. From the Figure 4.17 and Figure 4.18 also it can be seen that minimum color removals were obtained at WTR dose of 20mg/L. Therefore it can be said that the best color removal was obtained at pH3 and as the pH increases color removal. However from pH 7 to pH9 there was marginal increase in color

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 main objective of this experiment is to carry out qualitative analysis to identify metal cations in unknown solution 1.

To find the nature of each substance, the results from the practical were compared to the expected results for the possible substances given which were potassium chloride, sodium chloride, sucrose, glucose, sulfur, copper chloride and copper sulfate. Research was conducted to match these known substances to the unknown substances to determine whether they were covalent or ionic. From the results, it could be determined that substance 1 was copper sulfate with covalent bonds. Substance 2 was sulfur with covalent bonds. Substance 3 was copper chloride with ionic bonds. Substance 4 was sucrose with covalent bonds. Substance 5 was sodium chloride with ionic bonds. Substance 6 was potassium chloride with ionic bonds. Substance 9 was glucose with covalent bonds.

Introduction: A rate of reaction is how fast or slow a chemical reaction happens. In order for a chemical reaction to occur it must have a great amount of energy and the particles in a chemical reaction must collide frequently. There are a variety of factors which can affect the rate of a reaction, these include temperature, surface area, concertation, agitation and a catalyst. One of the factors that we have investigated above includes the measurement of the surface area between three Aspirin tablets. The first tablet was kept whole, the second tablet was cut into four pieces and the last tablet was crushed into fine powder.

Hold the grating several inches from your face, at an angle. Look at the grating that you will be using. Describe what you see at the grating surface.

To vary the concentrations of each reactant along with the sulphuric acid in order to observe and measure its effect on the overall rate of reaction in absorbance using colourimetry.

Fe3+ before the oxalate ion will readily bind to it. Hydrogen peroxide is the oxidant of choice: 2Fe2+ (aq) + H2O2 (l) + 2H+ (aq) ---> 2Fe3+ (aq) + 2H2O (l), in acidic solution.

The purpose of this experiment was to determine how much KMnO4 was needed to titrate approximately 1 mL of an Unknow X101 concentrated solution of Oxalic Acid. A standardized KMnO4 solution was used on a known solution of Oxalic acid to help determine the unknown percent oxalic acid in unknown X101. The unknown sample for this experiment was sample x101 which theoretically was a % Oxalic Acid dehydrate sample but, the average of all three trials determined it to be a 6.7% percent Oxalic acid.