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Experiments to investigate factors affecting the rate of diffusion
Investigating diffusion
Diffusion experiment lab report
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When evaluating the results from Investigations 1 and 2, it can be seen that the most influencing factor on the percentage of diffusion was the different surface area of the agar. As predicted in the second hypothesis, the 1cm cube had the highest diffusion percentage with 21.6% of the cube being affected in 8 minutes. This is a significant difference of 18.17% when compared to the 2cm cube’s diffusion percentage of 3.43 and a 20.38% difference from the 2.5cm cube’s result of 1.22%. Investigation 1’s results show that the most successful concentration of acid to diffuse through the phenolphthalein was the 1M with a percentage of 1.81. This is a 0.47% difference from the results of the 2M sulfuric acid. Graph 2 demonstrates that the diffusion percentage continued to incline when the concentration increased however starts to decrease past the 1.8 point. These results were unexpected and so a fifth trial was run in order …show more content…
Overall there were four different methods, two of which can be seen above, each measuring the diffusion of the sulfuric acid. The first method used to measure the impact that influencing factors had on the rate of diffusion was going to be used universally. It focused of cutting the clear agar from the cube and measuring the remaining phenolphthalein to then determine how far the acid diffused into the block. Once testing, this became difficult to obtain exact results and the 20 second intervals between the agars resulted in a busy and cramped work space. For the method Investigation 2, 1cm, 2cm and 3cm blocks were originally planned to be used. However, because majority of the cubes were roughly pre-cut small, the 3cm block was unavailable and so, had to be substituted in for the next largest which was a 2.5cm cube. The third and fourth attempts are the methods that can be referred to in the above investigations and were successful in producing
The Effect of Solute Concentration on the Rate of Osmosis Aim: To test and observe how the concentration gradient between a potato and water & sugar solution will affect the rate of osmosis. Introduction: Osmosis is defined as, diffusion, or net movement, of free water molecules from high to low concentration through a semi-permeable membrane. When a substance, such as sugar (which we will be using in the experiment we are about to analyse), dissolves in water, it attracts free water molecules to itself, and in doing so, stops them from moving freely. The effect of this, is that the concentration of (free) water molecules in that environment goes down. There are less free water molecules, and therefore less water molecules to pass across a semi-permeable membrane, through which sugar molecules and other molecules attached to them are too big to diffuse across with ease.
has a lower energy state. It will now tend to remain the way it is.
There were some changes in the amount of solvents and products used. For example, 0.5ml of sulfuric acid was used instead of 20ml.
This experiment was completed with minor deviations from the original protocol. A slight mistake was made when solutions were transported from the test tube to the cuvette. The funnel wasn’t rinsed out completely, and this may have led to slight deviations. However, it may not have been enough to make a significant impact upon the results.
Compared that to the reported amount, there was only a 1.3% error, while the class had an average error of 6.35%. These results are quite impressive because the percent errors were quite low for a high school lab. Errors could have occurred during this lab that would have affected the accuracy of the gravimetric analysis. Some errors could include not waiting for a complete filtration of the solution which could have led to a decrease in phosphorous collected or a spill could have occurred. During the last filtration process, it was highly possible that a lost of product could have occurred if the precipitate was able to flow through the filtration paper. In order to prevent this in future investigations, a better filtration paper could be used or the excess water collected in the cup could be refiltered to collect any extra analyte that seeped through. Although the result collected from our group was very close to the reported amount, averaging the result helped other groups who had a high percent error, such as 12%, get a closer mass value and percentage of
Samples were taken from the three main bottles that contained the three solutions that were needed in the experiment. 10 ml of solution A was placed on a 50 ml Erlenmeyer flask. This solution had transparent water like consistency and appearance. 3 ml of solution B was put on a 10 ml Erlenmeyer flask. This solution had a blue tint on it. 3 ml of solution C was also placed on another 10 ml Erlenmeyer flask. Like solution A, this last solution had the same transparent water like consistency and appearance. Cork Stoppers were placed on the rim of all the flasks. After making sure that the exteriors were dry, the whole system was weighed all at the same time and the measurement data recorded. Solution B was then poured onto the 50 ml flask, as the blue liquid trickled down slowly, there was toothpaste like precipitate that appeared on the bottom of the flask. It was not until the swirling began did the two solutions mix for before swirling the flask, the two solutions did not readily mix together. While carefully swirling the flask, the toothpaste like precipitate began to mix with the clear liquid.
All the tablets were kept in the oven where the temperature was around 70°C for the next day in order to dry them. The tablets with the container were weighted together again after making sure that they were completely dry without moisture in order to determine the erosion percentage by applying the following formula
To determine the suitability of phenolphthalein and screened methyl orange as acid base indicators for detecting the end points of acid-base titrations.
However, the method of volumetric analysis is highly dependent on a pure standard which the amount of substance present is accurately known. Prior to estimation of the acetic acid, sodium hydroxide (NaOH) was used as the standard solution. Thus, the concentration of the sodium hydroxide (NaOH) was first determined because sodium
In conclusion my hypothesis was correct towards this experiment, the concentration with the most Dettol disinfectant had the least bacterial growth and the least Dettol disinfectant had the most bacterial growth occurring in our agar plates, the experiment was successful to show the soil bacterial growth and how well the Dettol disinfectant works to prevent the growth.
This experiment conducted used the Gravimetric Analysis method to determine the concentration of an unknown sulfate solution. The unknown sulfate solution was pipetted into a smaller beaker, acidified, heated, decanted through filtration, dried, cooled and weighed. What was found at the end of the result was Barium Sulfate precipitate which weighed 0.1783 grams. The concentration of the unknown sulfate solution was found to be 2.9385 g/L and its molarity was 0.0306M.
Turn on the lamp and as soon as the substance begins to move start timing 10 min. After ten minutes measure in millimeters the distance the solution has
It is the ability of the analytical method to relate the obtained results over a specific given range through mathematical equations or proportional to the concentration of the analyte in the sample in that specific range. Accordingly, Linearity is an important tool to assure that the response of the Area Under Concentration will be later translated into the correct percentage of that analyte in the sample
Preparation of Agar containing Petri Dishes: Standard laboratory beaker was thoroughly cleaned and dried before any use. 100ml of tap water was poured into the beaker. The hot plate was switched onto number 1 and left for three minutes to prepare for heating. At the end of three minutes the beaker containing 100 ml of water was placed on hot plate. The water was allowed to heat to 100 °C which would effectively stop any bacterial growth in water. Thermometer was used to measure the temperature of water. 2.3g of Agar powder, measured by using a mass scale, was added to the water while it was being heated. The water was stirred with a rod to make it sure that the agar mixes well and forms a homogenous solution. Once the temperature of the solution rose up to 95°C, the hot plate was slowed down to 0.5 to allow the temperature to rise slowly to 100°C (Fig 3). Once the temperature reached 100°C, the beaker was moved away from the hot plate using a pair of tongs and placed onto the heatproof mat. The next step was to prepare 30 petri dishes which were provided by the lab in packed sterile form. Each petri dish was opened partially
Several factors affect the action of disintegrants such as: ratio of the disintegrant in tablet, particle size, molecular structure, compression force, method of incoroporation, compatibility with other excipients, adding more than one disintegrant, addition of surfactant, tablet hardness the tablets, API nature , mixing, screening and others [5,10,11]. In 1980, Rundic and co-workers found that larger CPV grades (with larger particle size) are more efficient than smaller one [12]. Later in 1981, Smallenbroek et al studied the effect of particle size of the disintegrant on the disintegration of tablet, they found that larger particle size are more efficient than smaller one [13]. Later, Rundic and co-workers studied the effect of crosslinking