Assignment is to reply to (2) peers with individual references, Provide follow up questions and useful information to peers. Original topic is provided to have a better idea on discussion, do not reply to original topic.
Original topic:A concentrated phosphoric acid solution is 85.5% H3PO4 by mass and has a density of 1.69 g/mL at 25°C. What is the molarity of H3PO4? What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 5.6 g of urea in 30.1 g of methanol, CH3OH? How will an understanding of this concept help you in your healthcare career?
PEER (1) Amy
The molar mass of H3PO4 is 98 grams per mole.
85.5 percent of the total mass
1.69 g / mL density
Relationship between mass percent and molarity (formula)
molarity = mass percent x 10 x density / molar mass molarity = mass percent x 10 x density / molar mass molarity = mass percent
= 98 x 85.5 x 10 x 1.69
(14.7 M)
14.7 M molarity
Molarity and percent solution are two important methods for determining concentration. Different solutes dissolve to varying degrees in various solvents and under various conditions. A solution with a considerable amount of solute is said to be concentrated qualitatively. Dilute refers to a solution that contains just a modest amount of solute. We utilize numbers to express ourselves quantitatively; thus, molarity and percent solution (Cannoy, 2018).
————————————–
mass / molar mass = moles of urea
= 5.6 / 60 = 5.6 / 60 = 5.6 / 60 =
0.0933%
Methanol moles = 30.1 / 32
0.961
urea mole fraction = urea moles divided by total moles
0.0933 / 0.0933 + 0.961 = 0.0933 / 0.0933 + 0.961
0.00902
0.0902 mole fraction of urea
The mole fraction of urea is defined as the ratio between the number of moles of urea and the total number of moles present in the solution (Moffett, 2018). Dose miscalculation is a common cause of medication mistakes. Nurses must be confident in their ability to calculate drug doses in order to safely give medications to patients as directed. The proper administration of medications is a core nursing skill that necessitates a wide range of knowledge and abilities. Calculating medicine doses and rates of drug administration in order to administer them to the patient as prescribed is one of the qualifications necessary.
References:
Cannoy, B. (2018, April 13). How to measure concentration using molarity and percent solution. How to Measure Concentration Using Molarity and Percent Solution. Retrieved September 28, 2021, from https://www.dummies.com/education/science/chemistry/how-to-measure-concentration-using-molarity-and-percent-solution/.
Moffett, K. (2018, February 9). Find the mass of urea, “Co”(“NH”_2)_2, needed to prepare “49.0 g” of a solution in water in which the mole fraction of urea is 7.58 * 10^(−2)?: Socratic. Socratic.org. Retrieved September 28, 2021, from https://socratic.org/questions/find-the-mass-of-urea-ch4n2o-needed-to-prepare-49-0-g-of-a-solution-in-water-in-#:~:text=Explanation%3A,moles%20present%20in%20the%20solution.&text=with%20murea%20being%20the,being%20the%20mass%20of%20water.
Peer (2) Evelyn
What is MOLARITY?
The molarity (M) of a solution is the number of moles of solute dissolved in one liter of solution. To calculate the molarity of a solution, you divide the moles of solute by the volume of the solution expressed in liters (CK12 Intermediate, n.d.).
What is the molarity of H3PO4?
Given that: % = 85.5 %
Density = 1.69 g/mL
Gram molecular weight = 98.0 g/mol
Formula: Molarity = % x density x 10 / gram molecular weight
M = 85.5 x 1.69 x 10 / 98.0
M = Molarity of H3PO4 = 14.7 mol / L
What is the mole fraction of urea, CO(NH2)2, in a solution prepared by dissolving 5.6 g of urea in 30.1 g of methanol, CH3OH?
Moles of urea = mass / molar mass = 5.6 / 60. = 0.093 mol
Moles of methanol = mass / molar mass = 30.1 / 32. = 0.94 mol
Mole fraction of urea = moles of urea / total moles of solution = 0.093 / ( 0.093 + 0.94 ) = 0.0900
Mole fraction of urea = 0.090
Mole fraction of methanol = 1 – 0.09 = 0.91
How will an understanding of this concept help you in your healthcare career?
In healthcare understanding this concept can help you can mix two medicine with definite and accurate proportion . Knowing the molarity of a solution is meaningful because by knowing it you can not only know if it is diluted or concentrated, but also the actual concentration (Why Is This Important? – Main View | Unit 6.5 – Molarity | BIO 101 Fall 2013 – Emerging Technologies | MATCOnline, n.d.).
references:
CK12 Intermediate. (n.d.). Molarity | Chemistry for Non-Majors. Lumenlearning. Retrieved September 29, 2021, from https://courses.lumenlearning.com/cheminter/chapter/molarity/
P. (n.d.). Phosphoric acid. PubChem. Retrieved September 29, 2021, from https://pubchem.ncbi.nlm.nih.gov/compound/Phosphoric-acid
Why is this important? – Main View | Unit 6.5 – Molarity | BIO 101 Fall 2013 – Emerging Technologies | MATCOnline. (n.d.). Matconline. Retrieved September 29, 2021, from https://matconline.matc.net/ICS/Academics/BIO/BIO_101/IndieStu-BIO_101-Fall_2013/Unit_65_-_Molarity.jnz?portlet=Welcome
