Part BCalculate the mass of solute required to make 2.64 x 102 mL of a magnesium sulfate solution that has an osmoticpressure of 3.95 atm at 301 KExpress your answer using two significant figures.▸ View Available Hint(s)Ο ΑΣΦSubmitPrevious Answers?g

Step 1:To calculate the mass of solute required to make a solution with a given osmotic pressure, we…

Answered: Part B Calculate the mass of solute…

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...

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0.302 grams of an antibiotic was dissolved in enough water at 23.6°C to make 500.0 mL of solution. The solution has an osmotic pressure of 8.34 mm Hg. What is the molar mass of the antibiotic? Can someone please break this down in steps. I am completely lost. I've seen the other post, but they don't make any sense to me the way they are laid out.
What is the molality (mol/kg) of a solution prepared by dissolving 34 g of Calcium Chloride (CaCl2) in 250 mL of water? Assume water has a density of 1.0000 g/mL and the volume does not change. Hint: CaCl2 molar mass = 110.98 g/mol 4.8 m 3.6 m 2.4 m 1.2 m
Please provide only typed answer solution no handwritten solution needed allowed
Part A What mass of sucrose (C12H22 O11) would you combine with 4.68 x 1002 g of water to make a solution with an osmotic pressure of 9.35 atm at 285 K ? (Assume a density of 1.00 g/mL for the solution). Express your answer in grams to three significant figures. ► View Available Hint(s) m = ΨΕ ΑΣΦ ? g
decimal place. No unit or wrong unit means wrong answer. 1. It is desired to prepare cupric sulfate solution by dissolving 250 grams of cupric sulfate in enough water to a volume of 900 mL. The solution has a density of 1.405 g/mL. Calculate: c) mole fraction of solute a) % by weight of solute b) Molality d) Normality 2. The density of toluene, C7H8, is 0.867 g/mL and the density of thiopene, CAH4S , is 1.065
Which of the following ideal solutions will have the lowest freezing point? justify your choice a) 0.1 m magnesium sulfate, MgSO4 b) 0.1 m potassium chloride, KCl c) 0.08 m magnesium chloride, MgCl2 d) 0.04 m sodium sulfate,Na2SO4 e) 0.05 m sodium chloride, NaCl
What is the osmotic pressure (in torr) of a solution formed by dissolving 33.9 mg of fructose (C6H12O6), a nonelectrolyte, in 0.250 L of water at 25°C Enter the VALUE, to TWO decimal places, WITHOUT units. Use DECIMAL, not scientific notation.
A Moving to another question will save this response. pestion 12 If the experimental value of van't Hoff factor for a solute in a 0.30 M solution is 1.53, determine the osmotic pressure in atm of this solution at 34 °C. (the answer should be entered with 3 significant figures; do not enter units; give answer in normal notation--examples include 1.23 and 12.3 and 123 and 123.) K Question 12 of 29 AMoving to another question will save this response V00> BBE %23 24 4. 7. delete w R Y P ente A D F G H K L eck retu B N alt atrol oplion ommand command option
Directions: Do what is asked. The final answer should be in a complete sentence and in the correct number of significant figures. 1. An enzyme that breaks bacterial cell walls is called lysozyme. If a solution containing 0.150 g of this enzyme in 210 mL of the solution has an osmotic pressure of 0.127 kPa at 25 °C. Calculate the molar mass of lysozyme. 2. Glycerin (?3?8?3) is a nonvolatile nonelectrolyte with a density of 1.26 g/mL at 25 °C. Calculate the vapor pressure at 25 °C of a solution made by adding 50.0 mL of glycerin to 500.0 mL of water. The vapor pressure of pure water at 25 °C is 3.17 kPa, and its density is1.00 g/mL. 3. Automotive antifreeze contains ethylene glycol, ?2?6?2, a nonvolatile nonelectrolyte, in water. Calculate the boiling point and freezing point of 25.0% by mass solution of ethylene glycol in water.
When a 0.99 of an unknown compound was dissolved of 85 mL of water an osmotic pressure of 835.5 torrs was measure at 29 Celsius. Calculate the molar mass of the compound [1 atm = 760= torr, R=0.0821 L atm/ mol x K] Short answer Develop the answers concisely, show formulas, values with units, results with units, and correct number figures.
Osmotic pressure data for a solution containing an unknown sugar are given below. Determine the molar mass of the sugar. T (atm) 2.59 5.06 7.61 12.75 18.13 23.72 density (g/L) 33.5 65.7 96.5 155 209 259
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Part B Calculate the mass of solute required to make 2.64 x 102 mL of a magnesium sulfate solution that has an osmotic pressure of 3.95 atm at 301 K Express your answer using two significant figures. ▸ View Available Hint(s) Ο ΑΣΦ Submit Previous Answers ? g