NATURE OF SOLUTIONS

A  solution consist of  solute, the substance that dissolves, and solvent, the substance in

which the solute dissolves. A solution may have one or more solutes dissolved in a given solvent. 

**

      The particles of solute are the size of individual small molecules or individual small ions. One nanometer is about the maximum diameter for a solute particle.

     The mixture does not separate on standing. In a gravity environment the solution will not come apart due to any difference in density of the materials in the solution.

     The mixture does not separate by common fiber filter. The entire solution will pass through the filter.

     Once it is completely mixed, the mixture is homogeneous. If you take a sample of the solution from any point in the solution, the proportions of the materials will be the same.

     The mixture appears clear rather than cloudy. It may have some color to it, but it seems to be transparent otherwise. The mixture shows no Tyndall effect. Light is not scattered by the solution. If you shine a light into the solution, the pathway of the light through the solution is not revealed to an observer out of the pathway.

     The solute is completely dissolved into the solvent up to a point characteristic of the solvent, solute, and temperature. At a saturation point the solvent no longer can dissolve any more of the solute. If there is a saturation point, the point is distinct and characteristic of the type of materials and temperature of the solution.

     The solution of an ionic material into water will result in an electrolyte solution. The ions of solute will separate in water to permit the solution to carry an electric current.

     The solution shows an increase in osmotic pressure between it and a reference solution as the amount of solute is increased.

     The solution shows an increase in boiling point as the amount of solute is increased.

     The solution shows a decrease in melting point as the amount of solute is increased.

     A solution of a solid non-volatile solute in a liquid solvent shows a decrease in vapor pressure above the solution as the amount of solute is increased.

^^

  Other Terms [ NATURE OF SOLUTIONS ]   :

Soluble -  a substance that dissolves in another substance. Examples are salt and sugars are soluble in water.

Insoluble – substance that does not dissolve in another. Example copper and mercury do not dissolve in water.

Miscible – liquids which are soluble in each other

Immiscible – liquids that do not mix

Electrolyte- is a substance that dissolves in water to form a solution that conducts electric current.

Non- electrolyte- is a substance that dissolves in water to give a solution that does not conduct electric current.

TYPES OF SOLUTIONS

In chemistry, a solution is a homogeneous mixture composed of two or more substances. In such a mixture, a solute is dissolved in another substance, known as a solvent. The solvent does the dissolving.

TYPES	EXAMPLES	SOLUTE	SOLVENT
Gaseous Solutions         Gas in Gas	Air	Oxygen	Nitrogen
Liquid Solutions Gas in Liquid Liquid in Liquid Solid in Liquid	Soda water Antifreeze Sea water	Carbon dioxide Ethylene glycol Sodium chloride	Water Water Water
Solid Solutions   Liquid in Solid Solid in Solid Gas in Solid	Dental amalgam Steel Charcoal filter	Mercury Carbon Poisonous Gases	Silver Iron Carbon

Gaseous Solutions

A gaseous solution is when two or more gases are mixed together and become uniformly intermingled. The atmosphere is a gaseous solution. It consists of nitrogen, oxygen, argon, carbon dioxide, water, methane, and some other minor components.

Read more: http://wiki.answers.com/Q/What_is_gaseous_solution#ixzz1AM3esLjD

Examples of Gaseous Solutions: 

Liquid Solutions

Liquid solutions are the most common type of solutions. In liquid solutions, the solvent is always a liquid. The solute may be a gas, a liquid, or a solid.

                                                                                                                

Read more: http://www.tutornext.com/help/liquid-solutions-chemistry

Examples of Liquid Solutions: 

Solid Solutions

A  solid solution is a solid-state solution of one or more solutes in a solvent. Such a mixture is considered a solution rather than a compound when the crystal structure of the solvent remains unchanged by addition of the solutes, and when the mixture remains in a single homogeneous phase.This often happens when the two elements (generally metals) involved are close together on the periodic table; conversely, a chemical compound is generally a result of the non proximity of the two metals involved on the periodic table.

Read more:

http://www.britannica.com/EBchecked/topic/553329/solid-solution

Examples of Solid Solutions: 

Concentration of Solutions

Concentrations of Solutions

There are a number of ways to express the relative amounts of solute and solvent in a solution. This page describes calculations for four different units used to express concentration:

• Percent Composition (by mass)
• Molarity
• Molality
• Mole Fraction
• Parts per Million
• Mass Per Unit Volume
• Percent by Volume

Percent Composition (by mass)

We can consider percent by mass (or weight percent, as it is sometimes called) in two ways:

• The parts of solute per 100 parts of solution.
• The fraction of a solute in a solution multiplied by 100.

We need two pieces of information to calculate the percent by mass of a solute in a solution:

• The mass of the solute in the solution.
• The mass of the solution.

Use the following equation to calculate percent by mass:

Molarity

Molarity tells us the number of moles of solute in exactly one liter of a solution. (Note that molarity is spelled with an "r" and is represented by a capital M.)

We need two pieces of information to calculate the molarity of a solute in a solution:

• The moles of solute present in the solution.
• The volume of solution (in liters) containing the solute.

To calculate molarity we use the equation:

PLEASE WATCH THIS VIDEO FOR SOLVING PROCEDURES :]

Molality

Molality, m, tells us the number of moles of solute dissolved in exactly one kilogram of solvent. (Note that molality is spelled with two "l"'s and represented by a lower case m.)

We need two pieces of information to calculate the molality of a solute in a solution:

• The moles of solute present in the solution.
• The mass of solvent (in kilograms) in the solution.

To calculate molality we use the equation:

PLEASE WATCH THIS VIDEO FOR SOLVING PROCEDURES :]

Mole Fraction

The mole fraction, X, of a component in a solution is the ratio of the number of moles of that component to the total number of moles of all components in the solution.

To calculate mole fraction, we need to know:

• The number of moles of each component present in the solution.

The mole fraction of A, X_A, in a solution consisting of A, B, C, ... is calculated using the equation:

To calculate the mole fraction of B, X_B, use:

 PLEASE WATCH THIS VIDEO FOR SOLVING PROCEDURES :]

Parts per Million

Parts per million - ppm -  is commonly used as a measure of small levels of pollutants in air, water, body fluids, etc. Parts per million is the mass ratio between the pollutant component and the solution and ppm is defined as

ppm = 1,000,000 m_c / m_s         (1)

where

m_c = mass of component (kg, lb_m)

m_s = mass of solution (kg, lb_m)

In the metric system ppm can be expressed in terms of milligram versus kg where

·         1 mg/kg = 1 part per million

Alternatively mass related units to measure very small concentration levels used are

·         ppb - parts per billion (1 / 1,000,000,000)

·         ppt - parts per trillion (1 / 1,000,000,000,000)

An alternatively mass related unit to measure larger concentration levels are weight percent which can be expressed like

weight percent = 100 m_c / m_s         (1)

PLEASE WATCH THIS VIDEO FOR SOLVING PROCEDURES :]

Volume related Concentration Units

Mass per Unit Volume

The concentration of a component can be measured as mass per unit volume as mg/liter, mg/cm³, etc.

Weight of substance added to one unit volume of water to give one part per million (ppm)

1 ppm

    = 2.72 pounds per acre-foot

    = 1,233 grams per acre-foot

    = 1.233 kilograms per acre-foot

    = 0.0283 grams per cubic foot

    = 0.0000624 pounds per cubic foot

    = 0.0038 grams per US gallon

    = 0.058419 grains per US gallon

    = 0.07016 grains per Imperial gallon

    = 1 milligram per liter

    = 1 microlitre ( μL ) per liter

    = 0.001 gram per litre

    = 8.345 pounds per million gallons of water

PLEASE WATCH THIS VIDEO FOR SOLVING PROCEDURES :]

Percent by Volume

Volume percent can be expressed as volume per unit volume as

percent by volume = 100 v_c /(v_c + v_s)         (3)

where

v_c = volume component

v_s = volume solvent

CLICK HERE FOR PRACTICE/ TEST QUIZ :D