14. Solutions

Intro to Henry's Law

Henry's Law and Gas Solubility Explained

Solutions: Crash Course Chemistry #27

One of the possible consequences of climate change is an increase in the temperature of ocean water. The oceans serve as a “sink” for CO2 by dissolving large amounts of it. <img src="https://lightcat-files.s3.amazonaws.com/problem_images/2c0b10fd4ed7d4e9-1668622815034.jpg" alt="" /> (a) The figure below shows the solubility of CO2 in water as a function of temperature. Does CO2 behave more or less similarly to other gases in this respect?

Henry's Law

Increasing the temperature will increase the solubility of CH4.

Increasing the temperature will decrease the solubility of NaCl.

Both NaCl and CH4 are quite soluble in water.

Neither NaCl nor CH4 are soluble in water.

Which of the following is true for the solubility of NaCl(s) and CH4(g) in water? &nbsp;

Scuba divers breathing air at increased pressure can suffer from
oxygen toxicity—too much oxygen in their bloodstream—
when the partial pressure of oxygen exceeds about 1.4 atm.
What happens to the amount of oxygen in a diver’s bloodstream
when he or she breathes oxygen at elevated pressures?
How can this be reversed?

Henry's Law: Explanation, Limitations and Applications - Explained Details (Animation)

Henrys Law: A physical description

Henry's Law Explained - Gas Solubility & Partial Pressure - Chemistry Problems

Pressure and Gas Solubility (Henry's Law)

Intro to Henry's Law Example 1

Intro to Henry's Law Concept 1

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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

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

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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