**Osmotic Pressure Calculation***Problem Statement:*What will be the osmotic pressure exerted by an aqueous solution of 500 mL volume at 25°C if it contains 12.54 g of dissolved magnesium chloride?*Explanation:*To solve this problem, we'll need to use the formula for osmotic pressure:\[ \pi = iMRT \]where:- \( \pi \) is the osmotic pressure,- \( i \) is the van’t Hoff factor,- \( M \) is the molarity of the solution,- \( R \) is the ideal gas constant (0.0821 L·atm/mol·K),- \( T \) is the temperature in Kelvin.**Steps to solve:**1. **Determine the molarity (\( M \)) of the solution:** - Calculate the moles of magnesium chloride (MgCl\(_2\)). The molar mass of MgCl\(_2\) is approximately 95.21 g/mol. - Convert the mass of MgCl\(_2\) to moles: \[ \text{moles of MgCl}_2 = \frac{12.54 \, \text{g}}{95.21 \, \text{g/mol}} \] - Convert the volume from mL to L: \[ 500 \, \text{mL} = 0.500 \, \text{L} \] - Molarity \( M \) = \(\frac{\text{moles of solute}}{\text{volume of solution in L}}\).2. **Identify the van't Hoff factor (\( i \)) for MgCl\(_2\):** - MgCl\(_2\) dissociates into three ions: \( \text{Mg}^{2+} \) and \( 2 \, \text{Cl}^- \), so \( i = 3 \).3. **Calculate the osmotic pressure using the formula:** - Convert the temperature to Kelvin: \( T = 25°C + 273.15 \). - Substitute the values into the osmotic pressure formula to find \( \pi \).Use this framework to perform the calculations and arrive at the final osmotic pressure.

Molar mass of Mgcl2 = 95g/mol Osmotic pressure= iCRT i = 3 as Mgcl2 dissociates to give 3 ions 1…

Answered: What will be the osmotic pressure…

What will be the osmotic pressure exerted by an aqueous solution of 500 mL volume at 25°C if it contains 12.54g dissolved magnesium chloride?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The freezing point of a solution that contains 1.1 g of an unknown compound, (A), dissolved in 12 g of benzene is found to be 2.97 °C. The freezing point of pure benzene is 5.48 °C. The freezing point depression constant of benzene is 5.12 °C/molal. What is the molecular weight of the unknown compound?
Calculate the freezing point of a solution that contains 5 grams of sucrose in 1000.00 grams of water, if the Kf of water is 1.86 K kg mol-1.
Calculate the molality of a solution composed of 4.5g of AgNO3 in 250mL of aqueous solution.
What is the mole fraction of acetone, C3H6O, in the vapor phase from a solution consisting of a mixture of acetone and ethyl acetate, CH3COOCH2CH3, at 30.00 °C, if the total pressure above the solution is 202.2 torr? The vapor pressures of pure acetone and NaN at 30.00 °C are 285.0 torr and 118.0 torr, respectively.
Bovine serum albumin (BSA) is a biochemically useful protein. A 0.303 g0.303 g sample of bovine serum albumin is dissolved in water to make 0.137 L0.137 L of solution, and the osmotic pressure of the solution at 25 ∘C25⁢ ∘C is found to be 0.826 mbar.0.826 mbar. Calculate the molecular mass of bovine serum albumin.
When 2.73 g2.73 g of a nonelectrolyte solute is dissolved in water to make 815 mL815 mL of solution at 21 °C,21 °C, the solution exerts an osmotic pressure of 961 torr.961 torr. What is the molar concentration of the solution?
What is the mole fraction of propanol, CH3CH2CH2OH, in the vapor phase from a solution consisting of a mixture of propanol and isopropanol, (CH3)2CHOH, at 25.00 °C, if the total pressure above the solution is 35.29 torr? The vapor pressures of pure propanol and NaN at 25.00 °C are 20.90 torr and 45.20 torr, respectively.
7) A 300.0 mL aqueous solution containing 0.512 g of an unknown polymer has an osmotic pressure of 32.9 torr at 29.5°C. What is the molar mass of the polymer? 29.5°C +273 =303.5K
The colligative molality of seawater is approximately 1.10 m. Calculate the vapor pressure of sea water at 20 °C. The vapor pressure of pure water at 20 °C is 17.54 Torr.
Omotic Pressure is a technique used to find the length of a polymer using its Molar Mass. If a 32.25 mg sample of PVC (polyvinyl chloride) is dissolved in benzene to 25.00 mL total solution at 30.00 oC, its osmotic pressure is 7.268 mm Hg. What is the Molar mass of the PVC? = i MRT760 mm Hg = 1.00 atmR = 0.08206 L-atm / mol K
The vapor pressure of an aqueous solution of barium chloride at 26 °C is 0.03172 atm. The vapor pressure of pure water at the same temperature is 0.03316 atm. Estimate the freezing point of the solution. For water, Kfp = 1.86 °C/m. °C
What is the mole fraction of solvent in a solution of aqueous sucrose (a nonelectrolyte) that has a vapor pressure of 23.47 torr at 25 °C? The vapor pressure of pure water at 25 °C is 23.77 torr.