14. Solutions

Henry's Law Calculations

Henry's Law: KH = P/C, Pressure and Concentration + 2 Examples

The presence of the radioactive gas radon (Rn) in well water presents a possible health hazard in parts of the United
States. (a) Assuming that the solubility of radon in water
with 1 atm pressure of the gas over the water at 30 °C is
7.27 * 10-3 M, what is the Henry’s law constant for radon in water at this temperature?

A gas has a Henry’s law constant of 0.112 M>atm. What total 
volume of solution is needed to completely dissolve 1.65 L of 
the gas at a pressure of 725 torr and a temperature of 25 °C?

Henry's Law Calculations Example 2

Henry’s Law Constant for nitrogen in water is 1.67 × 10-4 M • atm–1. If a closed canister contains 0.103 M nitrogen, what would be its pressure in atm?

The Henry's law constant for CO2 in water at 25 °C is 3.1x10^-2 M atm-1. (a) What is the soubility of CO2 in water at this temperature if the soltuion is in contact with air at normal atmospheric pressure?

At ordinary body temperature 137 °C2, the solubility of
N2 in water at ordinary atmospheric pressure (1.0 atm) is
0.015 g>L. Air is approximately 78 mol % N2. (b) At a depth
of 100 ft in water, the external pressure is 4.0 atm. What
is the solubility of N2 from air in blood at this pressure?

Henry's Law Calculations Concept 1

Henry's Law Calculations Concept 2

A saturated solution forms when 0.0537 L of argon, at a pressure 
of 1.0 atm and temperature of 25 °C, is dissolved in 1.0 L of 
water. Calculate the Henry’s law constant for argon.

A scuba diver is breathing compressed air that is 21% (by volume) oxygen at a depth of 66 ft. beneath the surface. The total pressure at this depth is 3.0 atm. The Henry’s law constant (k) for O2 in water at a normal body temperature (37 °C ) is 1.93 * 10-3 mol>(L atm). What is the solubility
of O2 in the blood of the diver at 66 ft. beneath the surface?
(LO 13.9)
(a) 1.22 * 10-3 M (b) 2.76 * 10-2 M
(c) 1.22 * 10-1 M (d) 2.76 * 10-1 M

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

At an altitude of 10,000 ft, the partial pressure of oxygen in the lungs is about 68 mm Hg. What is the concentration in mg/L of dissolved O2 in blood (or water) at this partial pres- sure and a normal body temperature of 37 °C? The solubil- ity of O2 in water at 37 °C and 1 atm partial pressure is 1.93 * 10-3 mol>L.

At 0°C and 1.00 atm, as much as 0.84 g of O2 can dissolve in 1.0 L of water. At 0°C and 4.00 atm, how many grams of O2 dissolve in 1.0 L of water?

Fish generally need an O2 concentration in water of at least 4 mg/L for survival. What partial pressure of oxygen above the water in atmospheres at 0 °C is needed to obtain this concentration? The solubility of O2 in water at 0 °C and 1 atm partial pressure is 2.21 * 10-3 mol>L.

Henry's Law: Relationship Between Pressure and Solubility of a Gas

The atmospheric pressure in a lab is calculated as 1.3 atm. If oxygen gas contributes 62% of this atmospheric pressure, determine its mass (in g) dissolved at room temperature in 25 L of water. The Henry’s Law Constant for oxygen in water at this temperature is 5.3 × 10–5 M/atm.

Solutions: Crash Course Chemistry #27

Henry's Law With Example Problem

Henry's Law Calculations Example 1

Henry's Law

The 2 Point Form of Henry's Law Formula is used when dealing with 2 pressures and 2 solubilities of a given gas.

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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.

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.

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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