Creation of a Liquid Fertilizer Using Abundant Elements

Abstract

The objective of the Liquid Fertilizer experiment was to create a 25 mL aqueous solution using the provided compounds in the lab description. The lab was split into two days where day one focused on finding which compounds containing Nitrogen, Phosphorus, and Potassium would dissolve in water; while day 2 focused on introducing Magnesium into the chosen combination from day 1. Results from day 1 found that the 3 compounds mixed fairly well together, resulting in a clear solution after mixing. Day 2 found that EDTA would need to be introduced in order to block the formation of a precipitate.

However, introducing EDTA still resulted in a small amount of precipitate forming.

Introduction

Nitrogen aids in growth of plants allowing for it to be used in all kinds of fertilizers. It can be found in the chlorophyll molecule and through the process of photosynthesis, nitrogen creates food for the plant. Phosphorus promotes the transfer of energy from the stem to the tips of the plant. In fact, Phosphorus has been found to aid in the development of roots and flowering.

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When a plant is growing and its leaves show a purple color, the plant is indicating that it has a phosphorus deficiency. Potassium has been found to be very abundant in the Earth’s crust. It has also been found through research, to moderate a plant’s metabolism, regulate CO2 intake and aid in the production of ATP. It helps in root development and affects the amount of water pressure in and outside of the plants.

With this information in mind, we attempted to create an aqueous fertilizer using all three of these compounds.

We hypothesized that on each given day, a liquid solution would be formed using the given molecular compounds. According to the laboratory procedures, Magnesium must be introduced to the aqueous solution produced during day 1. However, be aware that the addition of magnesium will cause problems due to the way it reacts with Phosphorus. Thus, prepare to utilize the compound EDTA. Ethylenediaminetetraacetic acid, better known as EDTA, is a chemical that binds to various metals; preventing ionic compound from forming, such as the one between Phosphorus and Magnesium. The objective of this experiment is to create a solution that could be used on plants; therefore, we must ensure the pH of the solution is in the 6-7 range; a healthy acidic range for plant growth.

Methodology

The task at hand was to create a 25mL solution using a volumetric flask. The solution contained , 5 % of Nitrogen, 3% of Phosphorus, 3 % of Potassium and 1% of Magnesium. Using this information, it was necessary to calculate the percent mass for each element within the given compounds. The compounds provided were: Ammonium chloride (𝑁𝐻4𝐶𝑙) , Trisodium Phosphatedodecahydrate (𝑁𝑎3𝑃𝑂4 × 12𝐻2𝑂), Potassium Chloride (KCl), and Magnesium sulphate (𝑀𝑔𝑆𝑂4 × 7𝐻2𝑂). After calculating the required mass of each compound in grams, a scoopula was used to scoop and place the compounds on a scale. Once the collection process was completed, the compounds were placed into a volumetric flask, water was added and mixed until a clear solution was present. pH paper was then used to find out whether a base or acid would be needed to reach a pH of 6-7. A pH of 9 was recorded, resulting in the addition of 9 drops of Hydrochloric acid to lower the pH to 7. Finally, we added water up until the 25 mL mark on the volumetric flask.

The next step of this experiment was to introduce magnesium. We weighed out the desired grams of 𝑀𝑔𝑆𝑂4 × 7𝐻2𝑂 and placed it in a recreated solution of 𝑁𝐻4𝐶𝑙, 𝑁𝑎3𝑃𝑂4 × 12𝐻2𝑂, and KCL from day 1. Since a precipitate formed, EDTA was introduced into this solution. The necessary mass of EDTA was calculated using a 1:1 ratio of EDTA and Magnesium. A second solution was made, but this time, EDTA and Magnesium were placed in the volumetric flask first and mixed with water. We then proceeded to place the other compounds 𝑁𝐻4𝐶𝑙, 𝑁𝑎3𝑃𝑂4 × 12𝐻2𝑂, KCL into the flask and continued to mix until the solution was clear (for the most part). Finally, the pH was measured, resulting in a pH of 8. We then proceeded to add Hydrochloric Acid, using about 7 drops until the solution had a pH of 7.

Finally, water was added to the 25 mL line and the molarity of each compound within the solution was calculated. We then proceeded to clean up our lab station.

Results

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Calculations: Equation #1

The calculation above is the conversion of percent by mass to grams of the compound. Since we needed to use .3 % Potassium, this was represented as 3 grams of 100 grams of solution. The next step requires you to cancel out grams of solution by putting 1 gram of solution over 1 mL of solution. Since a 25 mL solution was required, we then multiplied by 25 mL of solution to get 75 g of K. Knowing the grams of Potassium, we were then able to divide by Potassium’s molar mass. Knowing there is a 1:1 ratio of Potassium to Potassium chloride, 1 mol of KCl divided by 1 mol of K could be implied, thus allowing us to multiply by the molar mass of KCl. With this last step, the necessary amount of KCl was found to be .143 g. With this process, you should be able to calculate the mass for the rest of the compounds.

Molarities of each compound: Equation #2

To find the molarity of the compound, .143 grams of KCl was divided by the molar mass. 25mL was then converted to L, thus 1 over .025L was used to get mols over liters. This equation can be used to find the molarities of all the other compounds.

Discussion

The results obtained from the experiment do not support our hypothesis, nor does it support the hypothesis that EDTA would help create a fully aqueous solution. Although we were very close to getting the solution to dissolve fully, we still had a small amount of precipitate left over. This result could have come from various errors such as: an incorrect calculated mass of each compound, weighing out the correct mass of the compounds and not allowing the solution sufficient time to dissolve. Although a sample of how to calculate the mass was provided, it is possible that myself or my lab partner could have miscalculated somewhere. An example of how this could have affected the experiment is the calculation of EDTA. If a calculated amount of EDTA was incorrect, then there could have been an excess of 𝑀𝑔𝑆𝑂4 × 7𝐻2𝑂, that was left unbound and free in the solution. In regard to weighing out the compounds, it is possible that a slight amount of any of the compounds was lost while removing the compounds from the scale.

This could have contributed to a lack of EDTA during the creation of the second solution on day A way to improve the outcome of this experiment is to test other compounds that contain Nitrogen, Phosphorus, and Potassium. We were provided a list of compounds that contained these three elements, but only the compounds used in this experiment were tested. Additionally, (MgNO3)2 was another compound which contained Magnesium, yet was not experimented with due to a lack of time. With better preparation and more effort, all compounds containing Nitrogen, Phosphorus, Potassium and Magnesium could have been experimented with in order to increase the success of this lab. We could have also run more experiments pertaining to the compounds we used in order to obtain more data on those compounds.

The overall experiment was a failure due to the fact that a fully aqueous solution was not formed. With the use of : .477 g of Ammonium chloride (𝑁𝐻4𝐶𝑙), .143 g of Trisodium Phosphatedodecahydrate (𝑁𝑎3𝑃𝑂4 × 12𝐻2𝑂), .92 g of Potassium Chloride (KCl), .254 g of Magnesium sulphate (𝑀𝑔𝑆𝑂4 × 7𝐻2𝑂), and .383 g of EDTA, a small amount of precipitate was formed. With the formation of a precipitate, we realized that we must have made some calculation error involving EDTA. However, we were on the right track since there was less precipitate formed with EDTA than without. Whether more EDTA was needed or not, performing different experiments with different compounds is very important. If we could have explored other mixtures, we may have been able to create an aqueous solution. It is important to be able to synthesize liquid fertilizers containing these elements due to the many benefits they provide plants as well as cutting down the use of harmful chemical fertilizers.