Introduction The goal of this experiment was to determine whether the procedure for developing an anticancer agent, potassium tris (oxalato) ferrate (III) trihydrate salt, was a reliable and productive method or not. This was determined by calculating the theoretical yield, percent yield, and purity of the iron salt from the reaction used to produce the iron salt. The experimental procedure was obtained from a scientific journal and was followed by the experimenter, and the amount of salt produced was compared to the theoretical yield to calculate the percent yield. The purity of the salt was determined by calculating the percent mass of oxalate, potassium, and iron (III) in the salt. Experimental The first part of this experiment involved …show more content…
Oxalate Analysis Trial 1: 0.143 g N KMnO4 0.1060 g of iron salt Volume of KMnO4 used- 13.15 mL of N KMnO4 Normality of KMnO4: 0.1000 N KMnO4 Trial 2: 0.143 g N KMnO4 0.1072 g of iron salt Volume of KMnO4 used- 13.21 mL of N KMnO4 Normality of KMnO4: 0.1000 N KMnO4 Sample Calculation for % Weight of Oxalate in Sample: Equivalent weight of C2O42-: 88 g C2O42- = 44 g C2O42- 2 equivalents 1 equivalent % C2O4= V(N MnO4-)(88g C2O42-) X 100% 2 eq sample weight Trial 1: % C2O4= (0.01315 L MnO4-)(88g C2O42-) X 100% 2 eq = 80.13% % weight of oxalate 0.1060 g salt Trial 2: 77.53% weight of oxalate Average: 78.80% oxalate by mass in iron …show more content…
The percent yield of the salt, as compared to the theoretical yield of 9.40 grams, was 70.64%. Errors in this experiment can be drawn from numerous different areas. For example, the iron salt decomposes when it is exposed to light, which could have resulted in some of the salt decomposing leading to a lower calculated percent yield. Also, when the salt was first filtrated, there could have been a loss of solid, leading to a lower percent yield. Another risk for error in this experiment was contaminated glassware. Numerous glass containers were used, and many held substances that would skew the results of experiment if they were not washed properly. If the experiment was performed perfectly, the percent yield would have been 100%. the actual % mass would be closer to the theoretical, creating a smaller % error. Given that 70.64% of the theoretically possible 9.40 grams of salt were produced, the experimental procedure relatively effective at producing the salt. This method of producing the iron salt could be reproduced by the pharmaceutical company based on the experiment’s productivity and
This is an experimental lab that tested if drinking water passes the United States maximum phosphate standard. The results of this lab can help the American who drink the water know if there are too much phosphate in the water. Each group made a Potassium phosphate dilution from a stock solution. The concentration of the solution that needed to made affected the amount of Potassium phosphate that was diluted. To create a calibration curve, each group used the different concentrated Potassium phosphate solutions in their test. The lab utilized a spectrophotometer to figure out the absorbance of the five different Potassium phosphate solution and the absorbance of an unknown concentration solution. The absorbance of the unknown solution was used
I did accomplish the purpose of the lab. First, I determined the percentage of water in alum hydrate, and the percentage of water in an unknown hydrate. The results are reasonable because they are close to the example results. Second, I calculated the water of crystallization of an unknown hydrate. Furthermore, I developed the laboratory skills for analyzing a hydrate.
The cold pack experiment lab allowed us, the students, to apply theories learned in class to actual real life experiments; such experiments prepare us for future tasks the will be put forth to determine. Our main trajectory through this assignment was to determine what our unknown salt was, through experimental analysis. The main purpose of this lab was for us to determine what the given unknown salt is. For this experiment, my group and I were given unknown salt 7. Information recognized before starting the lab, were the materials needed, background information on the math required to determine the unknown(s). In addition, other background sources before starting the experiment included having previous knowledge of chemical formulas, understanding concepts learned throughout class and how a calorimetry works. Furthermore in order to determine how to complete the lab, we needed information upon how to properly keep the temperature of the water from decreasing or increasing, and this required that we needed to know what an insulator is and how to use ...
We’d note down the weight. Then we’d get our solutions ready. We were only given a 100% solution and a 0% solution, so we had to mix them in the right ratio to get all the solutions we needed. We decided to do 5 different types of solutions so we would have a wide range of results and it would be more accurate. We’d use 100%, 75%, 50%, 25%, 0% solutions in our experiment.
In this experiment, there were several objectives. First, this lab was designed to determine the difference, if any, between the densities of Coke and Diet Coke. It was designed to evaluate the accuracy and precision of several lab equipment measurements. This lab was also designed to be an introduction to the LabQuest Data and the Logger Pro data analysis database. Random, systematic, and gross errors are errors made during experiments that can have significant effects to the results. Random errors do not really have a specific cause, but still causes a few of the measurements to either be a little high or a little low. Systematic errors occur when there are limitations or mistakes on lab equipment or lab procedures. These kinds of errors cause measurements to be either be always high or always low. The last kind of error is gross errors. Gross errors occur when machines or equipment fail completely. However, gross errors usually occur due to a personal mistake. For this experiment, the number of significant figures is very important and depends on the equipment being used. When using the volumetric pipette and burette, the measurements are rounded to the hundredth place while in a graduated cylinder, it is rounded to the tenth place.
The overarch purpose of this lab was to see if the amount of salt concentration impacted whether a potato stick grew, shrunk, or stayed the same in size/mass. Our hypothesis was, if potato slices are added to 0%, 1%, and 2% salt solutions, then the solution is hypotonic and will have a positive net gain. And, if the potato is add to the 3% solution, then the solution will be isotonic and the weight will stay the same. However, after testing the data and gathering helpful information, the hypothesis does not support the results of the lab. The potato in the 0% solution originally weighed (potato 1) 2.2 grams and (Potato 2) 1.9 grams.
The purpose of this lab was to calculate the percent composition by mass of oxygen in potassium chlorate.
One possible source of experimental error could be not having a solid measurement of magnesium hydroxide nor citric acid. This is because we were told to measure out between 5.6g-5.8g for magnesium hydroxide and 14g-21g for citric acid. If accuracy measures how closely a measured value is to the accepted value and or true value, then accuracy may not have been an aspect that was achieved in this lab. Therefore, not having a solid precise measurement and accurate measurement was another source of experimental error.
The purpose of this experiment is to become familiar with metal and nonmetal ions and with tests to determine the presence or absence of these important ions as well as to estimate approximate amounts. This experiment is divided into three sections: cations (six tests), anions (four tests), and identification of an unknown salt. For Fe+3 (Iron) test, place about 2 mL of 5% iron(III) chloride (FeCl3) solution in a test tube and add 10% ammonium thiocyanate (NH4SCN) solution until a deep red color appears. Mix the two solutions gently and record the observations on the data sheet. Next is a flame test for Na+1 (Sodium).
Chemistry is a science that makes measurements and use data to draw conclusions. Although chemistry is about measurements all data can have a margin of error if one does not correctly follow procedure of the lab. Error may also occur even if everything is done correctly. In this experiment, you will be finding the error within certain calculations using raw data, and the determination error which will allow you to find the density of different substances. To calculate error in the experiment we will be using two terms precision and accuracy.
The aim of the experiment was to determine the osmolarity of the potato. In the experiment, the % mass change increased from -4.2% to 6.5% and drops to -16%. In 1%, 4% and 5% concentrations, the potato showed up as hypertonic and 2% and 3% concentrations are hypotonic. The standard deviation of concentration 3% showed up as 8, which is extremely high. It shows that the experiment of the concentration 3% was not accurate.
There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
Moisture is heavy, and thus it can change the results of the experiment, as we only want the weight of magnesium and the magnesium oxide.
This experiment consists of titrating the ferrous ion with permanganate ion to study the oxidation-reduction reaction. The ions react in acidic solution to give ferric ion and a reduced ionic form of manganese. All the reactants and products except permanganate ion are weakly colored, whereas permanganate is a very intensely colored ion. Then a solution of permanganate is removed as long as there is a ferrous ion present to react with it. But as soon as the entire ferrous ion has been oxidized, the next small portion of added permanganate colors the solution. The first appearance of a permanent pink color indicates the endpoint of the experiment. From the titration it will be able to calculate the percentage of iron in the sample from the data.
Results & Discussion:The actual, theoretical, and percent yield of sodium chloride (NaCl) was found to be 1.14g, .700g, and 61.4%,