SOLVED:Magnesium Citrate, Mg3(C6H5O7)2, Belongs ... - Numerade

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Magnesium citrate, Mg3(C6H5O7)2, belongs to a class of laxatives called hyperosmotics, which cause rapid emptying of the bowel. When a person consumes a concentrated solution of magnesium citrate, it passes through the intestines, drawing water and promoting diarrhea, usually within 6 hours. Calculate the osmotic pressure of a magnesium citrate laxative solution containing 28.5 g of magnesium citrate in 235 mL of solution at 37 C (approximate body temperature). Assume complete dissociation of the ionic compound. Magnesium citrate, Mg3(C6H5O7)2, belongs to a class of laxativescalled hyperosmotics, which cause rapid emptying of the bowel.When a person consumes a concentrated solution of magnesium citrate,it passes through the intestines, drawing water and promotingdiarrhea, usually within 6 hours. Calculate the osmotic pressure ofa magnesium citrate laxative solution containing 28.5 g of magnesiumcitrate in 235 mL of solution at 37 C (approximate body temperature).Assume complete dissociation of the ionic compound. Show more… Chemistry: Structure and Properties Nivaldo Tro 2nd Edition Chapter 13, Problem 108 View All Chapters

Step 1

Molarity (M) is defined as the number of moles of solute per liter of solution. The molar mass of magnesium citrate, Mg3(C6H5O7)2, is approximately 451.1 g/mol. So, the number of moles of magnesium citrate in the solution is: \[ \text{moles} = Show more…

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Submit Thanks for your feedback! Magnesium citrate, Mg3(C6H5O7)2, belongs to a class of laxatives called hyperosmotics, which cause rapid emptying of the bowel. When a person consumes a concentrated solution of magnesium citrate, it passes through the intestines, drawing water and promoting diarrhea, usually within 6 hours. Calculate the osmotic pressure of a magnesium citrate laxative solution containing 28.5 g of magnesium citrate in 235 mL of solution at 37 C (approximate body temperature). Assume complete dissociation of the ionic compound. Play audio Feedback Powered by NumerAI

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Key Concepts

Osmotic Pressure Osmotic pressure is a colligative property of solutions that represents the pressure required to prevent the net flow of solvent molecules through a semipermeable membrane separating a solution from pure solvent. It is quantitatively determined using the formula ? = i M R T, where ? is the osmotic pressure, i is the van’t Hoff factor, M is the molarity of the solution, R is the gas constant, and T is the temperature in Kelvin. Colligative Properties Colligative properties are characteristics of solutions that depend solely on the number of solute particles present rather than the nature of the solute itself. These properties, which include boiling point elevation, freezing point depression, vapor pressure lowering, and osmotic pressure, are particularly useful in understanding the behavior of solutions when solutes are added. Van’t Hoff Factor The van’t Hoff factor (i) is a measure of the total number of discrete particles that are generated in solution from a single formula unit of solute upon dissociation. For electrolytes that completely dissociate, i is typically greater than one, and it plays a critical role in calculating the osmotic pressure and other colligative properties of the solution. Complete Dissociation Complete dissociation is an assumption used in many colligative property calculations where it is presumed that a solute, particularly an ionic compound, fully separates into its constituent ions when dissolved. This simplifies the calculation of quantities like osmotic pressure by allowing one to directly apply the van’t Hoff factor corresponding to the total number of ions produced. Molarity Molarity (M) is a measure of concentration defined as the number of moles of solute per liter of solution. Accurate calculation of molarity is essential for determining colligative properties like osmotic pressure since it directly impacts the number of solute particles present in the solution. Ideal Gas Law Constant and Temperature in Kelvin The use of the gas constant (R) and the conversion of temperature into Kelvin are critical in osmotic pressure calculations. The gas constant connects the macroscopic properties of gases (or analogous properties in solutions) with temperature, while expressing temperature in Kelvin ensures that the relationships within the ideal gas law, and by extension the osmotic pressure equation, are correctly applied.

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Magnesium citrate, $\mathrm{Mg}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)_{2}$, belongs to a class of laxatives called hyperosmotics, which cause rapid emptying of the bowel. When a concentrated solution of magnesium citrate is consumed, it passes through the intestines, drawing water and promoting diarrhea, usually within 6 hours. Calculate the osmotic pressure of a magnesium citrate laxative solution containing $28.5 \mathrm{~g}$ of magnesium citrate in $235 \mathrm{~mL}$ of solution at $37^{\circ} \mathrm{C}$ (approximate body temperature). Assume complete dissociation of the ionic compound.

Magnesium citrate, $\mathrm{Mg}_{3}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{7}\right)_{2},$ belongs to a class of laxatives called byperosmotic, which cause rapid emptying of the bowel. When a person consumes a concentrated solution of magnesium citrate, it passes through the intestines, drawing water and promoting diarrhea, usually within 6 hours. Calculate the osmotic pressure of a magnesium citrate laxative solution containing 28.5 g of magnesium citrate in 235 $\mathrm{mL}$ of solution at $37^{\circ} \mathrm{C}$ (approximate body temperature). Assume complete dissociation of the ionic compound.

Magnesium citrate, Mg3(C6H5O7)2, belongs to a class of laxatives called hyperosmotics, which are used for rapid emptying of the bowel. When a concentrated solution of magnesium citrate is consumed, it passes through the intestines, drawing water and promoting diarrhea, usually within 6 hours. Part A Calculate the osmotic pressure of a magnesium citrate laxative solution containing 26.5 g of magnesium citrate in 235 mL of solution at 37 °C (approximate body temperature). Assume complete dissociation of the ionic compound.

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