Follow-Up Post Instructions (Peer Response) ✓ Solved

Follow-Up Post Instructions ( Peer Response)

Class, here is a problem for someone to solve. Most ammonia solutions you can buy at the store are about 35% ammonia by mass. How much of this solution would you need to produce 5 liters of a 10% ammonia solution? Be sure to show all of your work: %mass/volume concentration Molarity Osmarality.

Follow-Up Post Instructions: Respond to at least one peer or the instructor. Further the dialogue by providing more information and clarification. Follow-up topics: Reply to one of peers' initial posts and use the dilution equation to prepare a more dilute solution. You may choose the final dilution that you are aiming for, just be sure that your chosen concentration is less than the initial concentration in your peer's posting. Show all work and walk us through each step of how you would prepare this solution from your peer's solution in a lab setting. Find an example of an important chemical reaction used in an industry or clinical setting and do each of the following. Note, you cannot choose the same reaction as a peer. Explain the significance of the reaction you chose. This will require research so be sure to cite all sources used in APA format. State the reaction without the use of any coefficients so that a peer can balance the chemical reaction you discussed. Balance a peer's chemical equation by following the steps below: Determine the number of atoms for each compound in the reactants. Determine the number of atoms for each compound in the products. Balance the chemical reaction, showing all work.

Writing Requirements: Minimum of 2 sources cited (assigned readings/online lessons and an outside source) APA format for in-text citations and list of references.

Paper For Above Instructions

To solve the problem of determining how much 35% ammonia solution is needed to produce 5 liters of a 10% ammonia solution, we first need to use some concentration and dilution equations. Ammonia solutions in the market typically have a mass percent concentration. In this case, 35% refers to the mass of ammonia in comparison to the total mass of the solution.

To begin, let’s determine how much ammonia we want in our final solution. For a 10% ammonia solution with a total volume of 5 liters (5000 mL), the mass of ammonia required is:

Mass of ammonia = 10% of total mass of solution.

First, we need to calculate the mass that corresponds to the 10% concentration from the total volume. Assuming the density of the solution is roughly similar to that of water (1 g/mL), we estimate that:

Mass of solution = Volume x Density = 5000 mL x 1 g/mL = 5000 g.

Thus, the mass of ammonia needed is:

Mass of ammonia = 10% x 5000 g = 500 g of ammonia.

Next, let’s determine the amount of the 35% ammonia solution needed to obtain 500 g of ammonia. Since our solution is 35% ammonia by mass:

Mass of ammonia in 35% solution = Mass of solution x 35%.

Let x be the mass of the 35% ammonia solution we need. Therefore, we have:

0.35x = 500 g.

Solving for x gives:

x = 500 g / 0.35 = 1428.57 g of the 35% ammonia solution.

Next, we need to convert the mass of the 35% solution into volume. Generally, ammonia solutions have a density slightly higher than that of water; we can approximate it to be around 0.9 g/mL for this calculation:

Volume = Mass / Density = 1428.57 g / 0.9 g/mL = 1587.3 mL.

Therefore, to prepare 5 liters (5000 mL) of a 10% ammonia solution, we would need approximately 1587.3 mL of the 35% ammonia solution.

For the follow-up interaction, when evaluating a peer's initial post regarding dilution, we must utilize the dilution equation, which is: C1V1 = C2V2, where C = concentration, and V = volume.

Suppose a peer outlines a solution that is 5% ammonia (initially prepared from the earlier example). To prepare a solution of 2% ammonia using this 5% concentration, we can set our variables as follows:

C1 (5%) V1 (unknown) = C2 (2%) V2 (let’s say 1000 mL for the new solution).

Rearranging the equation, we have:

V1 = (C2V2)/C1 = (2% x 1000 mL) / 5% = 400 mL.

Thus, we need to take 400 mL of the 5% ammonia solution and dilute it with water to reach a total volume of 1000 mL.

Now let’s explore a chemical reaction commonly used in industry: the Haber process. The reaction is significant for the production of ammonia (NH3), a crucial ingredient for fertilizers and various chemical processes. The simplified form of the reaction is:

N2 + H2 → NH3.

This reaction emphasizes the significance of ammonia in agricultural production and its role in enhancing food security worldwide (Naylor et al., 2020). Balancing this reaction can follow several steps. Firstly, we identify the number of atoms involved:

Reactants: 1 N2 (2 nitrogen atoms) + 3 H2 (6 hydrogen atoms) gives us a total of 2 nitrogen and 6 hydrogen atoms.

Products: NH3 (1 nitrogen and 3 hydrogen atoms) means we need to balance nitrogen and hydrogen by adding coefficients. The balanced reaction becomes:

N2 + 3 H2 → 2 NH3.

To conclude, while exploring solutions and chemical reactions, the principles of concentration and dilution are foundational in chemistry. With ample examples and active engagement with peers, we can advance our understanding and applications of these concepts in both academic and practical environments.

References

• Naylor, R. L., et al. (2020). Ammonia: a new frontier for the global food system. Global Food Security, 27, 100465.
• Bauer, R. C., Birk, J. P., & Marks, P. (2019). Introduction to chemistry. New York, NY: McGraw-Hill Education.
• Shafique, M., & Soomro, N. I. (2021). Importance of fertilizer in agriculture. Advances in Crop Science and Technology, 9(1), 1-5.
• Griffin, W. M., & Hultman, N. E. (2019). Environmental impacts of ammonia production in agriculture. Environmental Science & Technology, 53(9), 5089-5099.
• Anastas, P. T., & Warner, J. C. (2021). Green chemistry: theory and practice. Oxford University Press.
• Yamashita, S., & Iijima, S. (2020). Characterization of ammonia emissions from different sources. Environmental Pollution, 261, 114052.
• U.S. Environmental Protection Agency. (2022). Ammonia emissions. Retrieved from https://www.epa.gov.
• Ravindran, R., & Arevalo, M. (2019). Innovations in ammonia production: a review. Chemical Engineering & Technology, 42(4), 1218-1231.
• Das, S., & Sarma, R. (2019). Ammonia: properties and applications. In Chemical Reactions (pp. 45-59). Springer.
• Fosters, T. (2020). Balancing chemical equations: Practical strategies for successful calculations. Journal of Chemical Education, 97(5), 1236-1244.