14. Solutions

Osmotic Pressure

13 - Solutions and Colligative Properties

A solid mixture of KCl, KNO3, and Ba1NO322 is
20.92 mass % chlorine, and a 1.000 g sample of the mix- ture in 500.0 mL of aqueous solution at 25 °C has an osmotic pressure of 744.7 mm Hg. What are the mass percents of KCl, KNO3, and Ba1NO322 in the mixture?

Suppose that one wishes to use reverse osmosis to reduce the salt content of brackish water containing 0.22 M total salt concentration to a value of 0.01 M, thus render- ing it usable for human consumption. What is the mini- mum pressure that needs to be applied in the permeators (Figure 18.20) to achieve this goal, assuming that the oper- ation occurs at 298 K? (Hint: Refer to Section 13.5.)

The osmotic pressure of blood is 5950.8 mmHg at 41°C. What mass of glucose, C6H12O6, is needed to prepare 5.51 L of solution. The osmotic pressure of the glucose solution is equal to the osmotic pressure of blood.

A 0.100 M ionic solution has an osmotic pressure of 8.3 atm at 
25 °C. Calculate the van’t Hoff factor (i) for this solution.

Desert countries like Saudi Arabia have built reverse osmo-sis plants to produce freshwater from seawater. Assume that seawater has the composition 0.470 M NaCl and 0.068 M MgCl2 and that both compounds are completely
dissociated.
(b) If the reverse osmosis equipment can exert a maximum pressure of 100.0 atm at 25.0 °C, what is the maximum volume of freshwater that can be obtained from 1.00 L of seawater?

The osmotic pressure of a 0.010 M aqueous solution of 
CaCl2 is found to be 0.674 atm at 25 °C. Calculate the van’t 
Hoff factor, i, for the solution.

Magnesium citrate, Mg3(C6H5O7)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 g of magnesium citrate in 235 mL of solution at 37 °C 
(approximate body temperature). Assume complete dissociation 
of the ionic compound.

Osmotic Pressure Concept 1

45: Colligative property: Osmotic pressure

The osmotic pressure of a solution containing 2.10 g of an unknown 
compound dissolved in 175.0 mL of solution at 25 °C 
is 1.93 atm. The combustion of 24.02 g of the unknown 
compound produced 28.16 g CO2 and 8.64 g H2O. What is the 
molecular formula of the compound (which contains only 
carbon, hydrogen, and oxygen)?

Osmotic Pressure Example Problem

Osmotic Pressure Example 1

What is Osmotic Pressure |  Extraclass.com

 Colloidal particles do undergo Brownian movement but consider other choices as well. 

 Colloidal dispersions do produce the Tyndall effect but consider other choices as well. 

 Particles of this size would settle out of solution and form a heterogeneous mixture. 

 Correct, because of the particles size and characteristics both Brownian movement and the Tyndall affect are properties of a colloid. 

 All of these properties do not characterize a colloid. 

 A colloid is considered to be a combination of a dispersed substance finely divided in a dispersing medium. 

 Which of the following characterizes a colloid? 

Lysozyme is an enzyme that breaks bacterial cell walls. A 
solution containing 0.150 g of this enzyme in 210 mL of 
solution has an osmotic pressure of 0.953 torr at 25 °C. 
What is the molar mass of lysozyme?

Osmosis and Osmotic Pressure

A dilute aqueous solution of an organic compound soluble 
in water is formed by dissolving 2.35 g of the compound 
in water to form 0.250 L of solution. The resulting solution 
has an osmotic pressure of 0.605 atm at 25 °C. Assuming 
that the organic compound is a nonelectrolyte, what is its 
molar mass?

Human blood gives rise to an osmotic pressure of approxi-mately 7.7 atm at body temperature, 37.0 °C. What must the molarity of an intravenous glucose solution be to give rise to the same osmotic pressure as blood?

An isotonic solution contains 0.90% NaCl mass to volume. Calculate
the percent mass to volume for isotonic solutions containing
each solute at 25 °C. Assume a van’t Hoff factor of 1.9 for
all ionic solutes.
a. KCl

 The temperature must be expressed in kelvins. 

 The molarity of the solution, the Kelvin temperature and the ideal gas constant can be used to calculate the osmotic pressure. 

 Correct, fairly dilute solutions produce appreciable osmotic pressures. 

 The volume of the solution must be used in the calculation. 

 Osmotic pressure can be calculated from the molarity of the solution times the gas constant times the temperature. 

 Determine the osmotic pressure at 22.5 &#176;C of a 2.5 L aqueous solution that contains 50.0 g of sucrose (molar mass = 342.3). 

Seawater contains 34 g of salts for every liter of solution.
Assuming that the solute consists entirely of NaCl (in fact,
over 90% of the salt is indeed NaCl), calculate the osmotic
pressure of seawater at 20 °C

What osmotic pressure in mm Hg would you expect for an aqueous solution of 11.5 mg of insulin 1mol. weight = 59902 
in 6.60 mL of solution at 298 K? What would the height of the water column be in meters? The density of mercury is 
13.534 g/mL at 298 K.

Hemoglobin is a large molecule that carries oxygen in the body. An aqueous solution that contains 2.61 g of hemoglo- bin in 100.0 mL has an osmotic pressure of 7.52 mmHg at 25 °C. What is the molar mass of the hemoglobin? Assume hemoglobin does not dissociate in water. (LO 13.15) 
(a) 1.96 * 103 g>mol (b) 84.8 g/mol 
(c) 6.45 * 104 g>mol (d) 3.65 * 103 g>mol

Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The Colligative Properties

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>