To determine the amount of iron in the iron tablets I carried out a titration, however the titration I carried out in a school lab is different to how titrations are carried out in industry. For example in schools, titrations are carried out by hand using a burette and measurements carried out by us, whereas in industry there are machines that are automated to carry out titrations by themselves. In schools when the titration is carried out by hand it means that it will take longer, and be less accurate because there is room for human error compared to the machine in industry which takes less time and is more accurate however it costs a lot more money than the cost of burettes and measuring cylinders etc. Another disadvantage of the method used in school is that the cleaning method is not always certain to get rid of all contamination left in the equipment as we only clean the equipment by hand, this is by rinsing with distilled water 3 times and then rinsing the equipment with the solution it will be holding, whereas most equipment will have specific cleaning instructions and will sometimes be able to perform a process in which it cleans itself. This also effects the impact on …show more content…
In industry they need to do this on a bigger scale and with a higher level of accuracy, some industries use a multichannel array spectrometer which is equipped with a fibre optic probe and this helps the acquisition of emission spectra. This has many significant advantages over the usual method in schools because in schools the result is based on people’s opinions which can lead to inaccuracy whereas this piece of equipment analyses the colour itself to give an accurate result. However the price of the school method is far cheaper than the piece of equipment used in industry so the buyers would need to evaluate if the cost of the product is worth the time and accuracy benefits of
The absorbance and the maximum wavelength of all eight standard solutions were determined using the same spectrophotometer in this section. First, approximately 3 mL of each solution was added into a cuvette using a plastic pipette. The solution was added until the level reached the frosty part of the cuvette and any bubbles were dislodged by gently tapping the cuvette against a hard surface. Then, a Kimwipe was used to clean the exterior of the cuvette. Once cleaned, the cuvette was transported by only holding the top edges.
We then found the maximum wavelength at which each dye displayed the maximum absorbance based on the peaks in each curve. For allura red, this peak occurred at 500 nm. For sunset yellow, this peak occurred at 480 nm. Using our data from the calibration curve (Table 2), we were able to find the extinction coefficient using Beer’s Law. Beer’s Law states .
(1) The purpose of the separation lab procedure was to help my group members and I successfully formulate our own plan before completing the experiment, handling multiple materials and substances, etc. It acted as a step-by-step plan that guided us throughout the experiment and ensured that we were well prepared ahead of time (ie. knowing what kind of materials were necessary and gathering the correct measurements of each substance); this made the experiment day much less hectic for all of us. It made reaching our goals (achieving > 85% recovery for each substance) more realistic and convenient. (2)We predicted that we would be able to easily separate each substance from the mixture through the use of our designed procedure. By using a bar magnet, we predicted that all the iron (and only the iron) would attract and quickly maneuver its way through the beaker and into the
How was accuracy ensured in the analysis of the complaint sample and whilst carrying out the food tests? Cations and Anions One of the main ways we ensured the accuracy of our practical was by making accurate and detailed observations of the practical. This is extremely important as you cannot carry out an experiment and record the results by just guessing or estimating the results. This could also impact on any calculations massively.
Objective: In this lab, students learned the different methods there is to separate substances from one another. They practiced the process of decantation, extraction, filtration, and sublimation. Introduction: Theory: Before being able to isolate the components in a mixture, the students should’ve become familiar with the physical properties of each of the substances. The students were given an unknown sample which has a combination of three different components.
The hydrate was suppose to lose water from evaporation but the crystals did not lose that much mass after being heated. This led to a very high relative range, 79.34%, that is above the other components in the iron salt lab. Also in this stage of the lab we did not evenly distribute the crystals between the beakers and did not put more grams in each container when we had extra grams to spare. To lower the errors during this process we could of put iron crystals under the heat stove longer and used more crystals in each trial. Likewise, errors occurred during the titration
The first is atomic absorption (AA) spectroscopy which is a more sensitive tool of measurement in that it excites individual metal atoms. The second is ultraviolet-visible (UV-Vis) spectroscopy which is a less sensitive tool of measurement in that it excites the whole molecule or ion. Atomic spectroscopy is used for the measurement of metallic elements at major and trace levels. In AA spectroscopy, light of a specific frequency is passed through a flame containing free atoms. Absorbance of light is measured and is proportional to the concentration of atoms.
This lab consisted of determining whether a certain liquid was an acid or base and experimenting with the pH of various substances when either acid or base was added to them. The lab was executed by using two different types of indicators as well as a titration in the end. The first indicator used was litmus paper. Through litmus paper, it is possible to decide whether a liquid is an acid or a base. By placing one slip of red litmus paper by one slip of blue litmus paper and dropping beads of the liquid on each, determining whether the liquid was a base or an acid was possible.
Compare the color of the unknown substance with a flame color chart. Record down the observations into
Research Question: To investigate and compare how different temperature (5℃, 15℃, 25℃, 35℃, 45℃) can affect the concentration of carbon dioxide in soda water through titration with sodium hydroxide solution. Introduction: Carbon dioxide plays an important role in soft drinks. Soda water is manufactured by pumping carbon dioxide into water under high pressure. Carbon dioxide dissolves in water to form carbonic acid, which is the fizz we find in soft drinks. CO2 + H2O ⇌
(Larsen, n.d.). A protein can be quantitatively assayed by many spectrophotometric methods. Generally, most methods used are by a chromophore. A chromophore is the color that appears when a molecule absorbs a specific wavelength of visible light and transmits or reflects others. (Encyclopædia Britannica,
Background Information: The spectrophotometer is an
Practical I: Acid-base equilibrium & pH of solutions Aims/Objectives: 1. To determine the pH range where the indicator changes colour. 2. To identify the suitable indicators for different titrations. 3.
For each sample, take the absorption spectra to observe at what wavelength the molecule experiences excitation. The sample then needs to be purged with nitrogen for five minutes to ensure that oxygen does not react with the sample. Using the excitation wavelength found from the absorption spectra, the emission spectra can be performed.
In direct titrations, the number of moles of acid can be easily derived by simply manipulating with the values of acid and base given in the experiment. In back titration, excessive volumes of acid are always added. Of which, only a certain quantity would be neutralised. The number of moles of acid is eventually derived from titrating this excess acid with a strong base and using mole fractions to calculate. The quantity of acid neutralised is obtained by subtracting the moles of acid given at the start of the experiment, with the moles of acid titrated.