14. Solutions

Boiling Point Elevation

Practice Problem: Colligative Properties

An ethylene glycol solution contains 25.2 g of ethylene glycol (C2H6O2) in 99.5 mL of water. Determine the change in boiling point. Assume a density of 1.00 g/mL for water.

A 100.0-mL aqueous sodium chloride solution is 13.5% NaCl by 
mass and has a density of 1.12 g>mL. What would you add (solute 
or solvent) and what mass of it to make the boiling point of 
the solution 104.4 °C? (Use i = 1.8 for NaCl.)

What is the boiling point of a 0.10 M solution of NaHSO4 if 
the solution has a density of 1.002 g>mL?

Carbon disulfide 1CS22 boils at 46.30 °C and has a density
of 1.261 g>mL. (a) When 0.250 mol of a nondissociating
solute is dissolved in 400.0 mL of CS2, the solution boils at
47.46 °C. What is the molal boiling-point-elevation constant for CS2?

Boiling Point Elevation Concept 1

13 - Solutions and Colligative Properties

Molality and Colligative Properties

Carbon dioxide is dissolved in 722 mL of benzene with a density of 1.59 g/mL. What mass of carbon dioxide would you add to make the boiling point of the solution 104.7°C?

A 1.2 m aqueous solution of an ionic compound with the formula
MX2 has a boiling point of 101.4 °C. Calculate the van’t
Hoff factor (i) for MX2 at this concentration.

Boiling Point Elevation Example 1

What is the molality of glucose in an aqueous solution if the boiling point of the solution is 103.15°C?

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

Adrenaline is the hormone that triggers the release of extra
glucose molecules in times of stress or emergency. A solution of 0.64 g of adrenaline in 36.0 g of CCl4 elevates the
boiling point by 0.49 °C. Calculate the approximate molar
mass of adrenaline from this data.

A solution prepared by dissolving 5.00 g of aspirin, C9H8O4, in 215 g of chloroform has a normal boiling point that is elevated by ΔT = 0.47 °C over that of pure chloro- form. What is the value of the molal boiling-point-elevation constant for chloroform?

Freezing Point Depression and Boiling Point Elevation

Pure water boils at 100°C. What is the new boiling point of water after the addition of 13.12 g aluminum chloride, AlCl3, to 615 g water? &nbsp;

A solution of citric acid, C6H8O7, in 50.0 g of acetic acid has a boiling point elevation of ΔT = 1.76 °C. What is the 
molality of the solution if the molal boilin# g-point-elevation 
constant for acetic acid is Kb = 3.07 1°C kg2>mol.

The following phase diagram shows part of the liquid–vapor phase-transition boundaries for pure ether and a solution of a nonvolatile solute in ether. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/479be825df9c9942-1672768368453.jpg" alt="" />
(b) What is the approximate mo#lal concentration of the sol-ute? [Kb for ether is 2.021°C kg2>mol.]

Boiling point elevation and freezing point depression | Chemistry | Khan Academy

Boiling Point of the solvent will increase with the addition of a solute.

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[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 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

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>

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